By increasing the scan rate, the intensity of the peak increases not only in the anodic direction, but also in the cathodic side. The peaks are not well defined, most likely because of the low concentration of the platinum-doped reduced graphene oxide in the modified electrode. The effect of varying the scan rate results in the slight shifting of the peak potentials to higher values, indicating a quasi-reversible electron transfer. The plot of the peak height *vs.* square-root of the scan rate is illustrated in **Figure 13**, on the right. Both, the anodic and the cathodic peak currents reveal linear response at all scan rates with very good correlation factors above 0.9. These results indicate that the electrochemical process is, as previously observed, controlled by the diffusion of the electroactive species. Modified electrodes containing platinum-doped graphene materials cause an increase of the current, however due to the low concentration, the peaks are not well defined. Reported literature data showed that the electrochemical response of graphene modified electrodes can be improved by increasing the amount of graphene into the electrode [15]. The electrochemical data and areas of the electrodes presented in **Table 4** reveal that the Pt-doped rGO modified electrode has a higher electroactive area than the graphene oxide electrode.

We have shown earlier that Au/rGO modified electrode exhibits an enhancement of the current response when compared to classical glassy carbon, which translates in better electrocatalytic activity for both oxidation and reduction processes. The Au/rGO modified electrode showed a current almost four times higher than bare carbon paste electrode.

A comparison of the cyclic voltammograms of GO, Pt- and Au-doped graphene material electrodes is shown in **Figure 14**. The cyclic voltammetric response of the gold-containing modified electrode shows well defined redox peaks with a peak-to-peak separation, ΔE, of 200 mV. Thus, it was clearly revealed that the insertion of gold onto the modified graphene oxide electrodes gives improved electrochemical response for the ferri/ferro redox signal. Noble Metal Dispersed on Reduced Graphene Oxide and Its Application in PEM Fuel Cells http://dx.doi.org/10.5772/intechopen.80941 85

**Figure 13.** Cyclic voltammograms for 1.0 mM K3 Fe(CN)6 in 0.5 M KCl solution on Pt/rGO modified electrode, v = 20–120 mV s−1 (left) and plot of I *vs*. v½ (right).

are shifted by approximately −80 mV for Pt/rGO, when compared with the potential of bare carbon paste electrode. An increase in the peak currents and a decrease in the separation

currents, ΔE is the separation between the peak potentials and A is the area of an electrode, with the corresponding

 **(A) Ic**

1. CPE 2.40·10−6 −3.23·10−6 325 0.0165 2.  Au/rGO 9.45·10−6 −1.47·10−5 200 0.2020 4. Pt/rGO 5.01·10−6 −8.04·10−6 153 0.0660

comparison to the bare CPE (ΔEp = 385 mV), indicating that the electron transfer reaction was kinetically and thermodynamically favored at the graphene oxide modified electrode

By increasing the scan rate, the intensity of the peak increases not only in the anodic direction, but also in the cathodic side. The peaks are not well defined, most likely because of the low concentration of the platinum-doped reduced graphene oxide in the modified electrode. The effect of varying the scan rate results in the slight shifting of the peak potentials to higher values, indicating a quasi-reversible electron transfer. The plot of the peak height *vs.* square-root of the scan rate is illustrated in **Figure 13**, on the right. Both, the anodic and the cathodic peak currents reveal linear response at all scan rates with very good correlation factors above 0.9. These results indicate that the electrochemical process is, as previously observed, controlled by the diffusion of the electroactive species. Modified electrodes containing platinum-doped graphene materials cause an increase of the current, however due to the low concentration, the peaks are not well defined. Reported literature data showed that the electrochemical response of graphene modified electrodes can be improved by increasing the amount of graphene into the electrode [15]. The electrochemical data and areas of the electrodes presented in **Table 4** reveal that the Pt-doped rGO modified electrode has a higher electroactive area than the gra-

We have shown earlier that Au/rGO modified electrode exhibits an enhancement of the current response when compared to classical glassy carbon, which translates in better electrocatalytic activity for both oxidation and reduction processes. The Au/rGO modified electrode

A comparison of the cyclic voltammograms of GO, Pt- and Au-doped graphene material electrodes is shown in **Figure 14**. The cyclic voltammetric response of the gold-containing modified electrode shows well defined redox peaks with a peak-to-peak separation, ΔE, of 200 mV. Thus, it was clearly revealed that the insertion of gold onto the modified graphene oxide electrodes gives improved electrochemical response for the ferri/ferro redox signal.

showed a current almost four times higher than bare carbon paste electrode.

were observed for all modified electrodes in

represent the anodic and cathodic peak

 **(A) ΔE (mV) A (cm2**

and Ic

**)**

between the peak potentials (ΔEp) at 20 mV s−1

**Table 4.** Electrochemical data from CV measurements at 20 mV/s; Ia

84 Electrocatalysts for Fuel Cells and Hydrogen Evolution - Theory to Design

**Entry Electrode type Ia**

surface.

measurements units.

phene oxide electrode.

However, the parameter of most significant importance is represented by the position of the voltammetric peak, rather than the magnitude of the wave. In the case of the metal-doped graphene modified electrodes, the larger peak current is likely due to a slightly larger surface area at the electrode (see **Table 4**).

**Figure 14.** Overlay of the cyclic voltammograms for GO, Pt-doped rGO and Au-doped rGO modified electrodes for the redox process of 1.0 mM K3 Fe(CN)6 in 0.5 M KCl solution (v = 20 mV s−1 ).

In order to better investigate the electroanalytical outcome of these graphene modified electrodes, we performed differential pulse voltammetry (DPV) measurements. The DPV experiments were meant to support the cyclic voltammetry investigations, as it is clearly known that DPV can assist in resolving the signals due to species with close half-wave potentials, as it measures the difference between two currents, before the end of the pulse and before its application. The strength of this technique is evident when poor electrochemical signals are obtained in cyclic voltammetry, enabling the registration of well-defined signals through the elimination of the non-Faradaic processes. Moreover, DPV provides useful information when the resolving of the voltammetric signals given by two species with close half-wave potentials is needed, producing easily quantifiable peak shaped responses.

**Figure 15** compares the differential pulse voltammograms of the graphene modified carbon paste electrodes, as well as the classical glassy carbon electrode. In all cases, sharp and wellresolved peaks are observed. The anodic (right side) and cathodic (left side) peaks are higher for the metal-doped reduced graphene oxide modified electrodes with the highest peak current being observed for the gold doped reduced graphene oxide modified electrode. An important parameter of an electrode material is its electronic properties, namely, the density of electronic states (DOS). The DOS of graphene materials has been reported as being high and it can be increased by varying the amounts of loaded graphene. Gold has a DOS of 0.28 states atom−1 eV−1 with high conductivity due to high proportion of atomic orbitals. Thus, the Au-doped rGO modified electrodes are highly sensitive for electrochemical investigation of the ferri/ferro redox system.

The active surface areas of the graphene modified electrodes were estimated according to the slope of the Ia *vs.* square root of the scan rates plot for a 1.0 mM K3 [Fe(CN)6 ], solution using 0.50 M KCl electrolyte, according to Randles–Sevcik equation [16]:

$$I\_i = 2.69 \cdot 10^5 \cdot n^{32} \cdot D^{12} \cdot A \cdot \mathbf{c} \cdot \mathbf{v}^{12} \tag{3}$$

where Ia

the scan rate.

For n = 1 and D = 6.68 × 10−6 cm2 s−1

system PEMFC with active area of 25 cm2

) gases (H2

and N2

NI c-RIO hardware was used to control the PEMFC system.

4000 with 0.4 mgPt cm−2

0.2 mgPt cm−2

150 mL min−1

times higher than the graphene oxide modified electrode.

as simultaneous CV characterization and degradation testing tool.

loading (case 2); commercial Pt/C 0.2 mgPt cm−2

refers to the anodic peak current, n to the electron transfer number, A to the surface

Noble Metal Dispersed on Reduced Graphene Oxide and Its Application in PEM Fuel Cells

areas were calculated for all the used modified electrodes. The results show that metal-doped graphene oxide materials cause an increase in the active surface of the electrode. The comparison between modified GO electrode and Au-doped rGO reveals a higher active surface of the latter electrode which recommends this material as an electrocatalyst for the ORR reaction in fuel cells. Also, the Pt-doped rGO modified electrode exhibits an electrode active surface two

Under PEMFC conditions at cell voltage of around 1.0 V during no-load, the Pt metal dissolution is expected. Moreover, Pt oxides are produced at potentials higher than 0.6 VSHE. In particularly at potentials above 0.95 VSHE, oxygen atoms can replace Pt atoms, thus the potential cycling cause remarkable changes of the catalyst structure. The catalyst exposure to such an accelerated test namely the potential cycling between 0.0–1.2 VSHE lead to a fast catalyst aging, opposed to the constant potential holding test [17]. Thus, the potential cycling could be used

For this purpose, the in-situ electrochemical evaluation was performed in a single fuel cell

electrodes and membrane electrode assembly fabrication procedure was reported in our previous studies [11–13]. For actual study, the Pt loading was established at 0.2 mgPt cm−2

anode of all developed fuel cells. The cathode catalyst layer was modified by taking into account three FC configurations, as follows: deposition of commercial Pt/C catalyst Hispec

loading (case 3).The fuel cell test station included specific devices such as configured workstation, fuel cell, DS electronic load, bubble-type humidifiers. The PEMFC was operated at 0.7 V for 1 h for membrane electrode assembly conditioning. After steady state operating conditions were maintained, the cyclic voltammetry measurements were performed in a H2

mode cell, from 0.025 to 1.2 V at a scan rate of 0.05 V/s. The flow rates of reactants (50 and

and pressure were fixed at 70°C and 1 bar pressure. The developed control system based on

Carbon corrosion causes the detachment of metal nanoparticles and thus electrical isolation and electrocatalytic inactivity. Taking into account the instabilities due to catalyst support which lead to diminishing of FC performance, we investigated the support aging. **Figures 16**–**18** present the cyclic voltammograms before and catalyst exposure to 2000 cycles between 0.025 and 1.2 V potential cycling. Our preliminary results indicated that the oxidation and reduction signals approx at 0.025–0.3 V decreased differently after accelerated test, indicating the loss in electrochemical surface area for all cases, more pronounced being recorded for commercial catalyst. In case 1 it is easily to observe the change in hydrogen adsorption/desorption on Pt both for hydrogen oxidation and hydrogen reduction. In case 2 and 3, insignificant changes

loading (case 1); commercial Pt/C 0.2 mgPt cm−2

[Fe(CN)6

http://dx.doi.org/10.5772/intechopen.80941

using the slope of the Ip–ν1/2 relation, the microscopic

(ElectroChem, USA). A detailed description of the

) were adjusted using flow controllers. The cell temperature

] and ν is

87

for

/N2

and Pt/rGO with

and Au/rGO with 0.2 mgAu cm−2

area of the electrode, D is the diffusion coefficient, c the concentration of K3

**Figure 15.** DPV voltammograms for graphene modified electrodes and commercially available glassy carbon electrode (GC): oxidation (left) and reduction (right) with optimized DPV parameters: modulation amplitude of 25 mV and step potential 5 mV.

where Ia refers to the anodic peak current, n to the electron transfer number, A to the surface area of the electrode, D is the diffusion coefficient, c the concentration of K3 [Fe(CN)6 ] and ν is the scan rate.

For n = 1 and D = 6.68 × 10−6 cm2 s−1 using the slope of the Ip–ν1/2 relation, the microscopic areas were calculated for all the used modified electrodes. The results show that metal-doped graphene oxide materials cause an increase in the active surface of the electrode. The comparison between modified GO electrode and Au-doped rGO reveals a higher active surface of the latter electrode which recommends this material as an electrocatalyst for the ORR reaction in fuel cells. Also, the Pt-doped rGO modified electrode exhibits an electrode active surface two times higher than the graphene oxide modified electrode.

Under PEMFC conditions at cell voltage of around 1.0 V during no-load, the Pt metal dissolution is expected. Moreover, Pt oxides are produced at potentials higher than 0.6 VSHE. In particularly at potentials above 0.95 VSHE, oxygen atoms can replace Pt atoms, thus the potential cycling cause remarkable changes of the catalyst structure. The catalyst exposure to such an accelerated test namely the potential cycling between 0.0–1.2 VSHE lead to a fast catalyst aging, opposed to the constant potential holding test [17]. Thus, the potential cycling could be used as simultaneous CV characterization and degradation testing tool.

For this purpose, the in-situ electrochemical evaluation was performed in a single fuel cell system PEMFC with active area of 25 cm2 (ElectroChem, USA). A detailed description of the electrodes and membrane electrode assembly fabrication procedure was reported in our previous studies [11–13]. For actual study, the Pt loading was established at 0.2 mgPt cm−2 for anode of all developed fuel cells. The cathode catalyst layer was modified by taking into account three FC configurations, as follows: deposition of commercial Pt/C catalyst Hispec 4000 with 0.4 mgPt cm−2 loading (case 1); commercial Pt/C 0.2 mgPt cm−2 and Pt/rGO with 0.2 mgPt cm−2 loading (case 2); commercial Pt/C 0.2 mgPt cm−2 and Au/rGO with 0.2 mgAu cm−2 loading (case 3).The fuel cell test station included specific devices such as configured workstation, fuel cell, DS electronic load, bubble-type humidifiers. The PEMFC was operated at 0.7 V for 1 h for membrane electrode assembly conditioning. After steady state operating conditions were maintained, the cyclic voltammetry measurements were performed in a H2 /N2 mode cell, from 0.025 to 1.2 V at a scan rate of 0.05 V/s. The flow rates of reactants (50 and 150 mL min−1 ) gases (H2 and N2 ) were adjusted using flow controllers. The cell temperature and pressure were fixed at 70°C and 1 bar pressure. The developed control system based on NI c-RIO hardware was used to control the PEMFC system.

Carbon corrosion causes the detachment of metal nanoparticles and thus electrical isolation and electrocatalytic inactivity. Taking into account the instabilities due to catalyst support which lead to diminishing of FC performance, we investigated the support aging. **Figures 16**–**18** present the cyclic voltammograms before and catalyst exposure to 2000 cycles between 0.025 and 1.2 V potential cycling. Our preliminary results indicated that the oxidation and reduction signals approx at 0.025–0.3 V decreased differently after accelerated test, indicating the loss in electrochemical surface area for all cases, more pronounced being recorded for commercial catalyst. In case 1 it is easily to observe the change in hydrogen adsorption/desorption on Pt both for hydrogen oxidation and hydrogen reduction. In case 2 and 3, insignificant changes

**Figure 15.** DPV voltammograms for graphene modified electrodes and commercially available glassy carbon electrode (GC): oxidation (left) and reduction (right) with optimized DPV parameters: modulation amplitude of 25 mV and step

In order to better investigate the electroanalytical outcome of these graphene modified electrodes, we performed differential pulse voltammetry (DPV) measurements. The DPV experiments were meant to support the cyclic voltammetry investigations, as it is clearly known that DPV can assist in resolving the signals due to species with close half-wave potentials, as it measures the difference between two currents, before the end of the pulse and before its application. The strength of this technique is evident when poor electrochemical signals are obtained in cyclic voltammetry, enabling the registration of well-defined signals through the elimination of the non-Faradaic processes. Moreover, DPV provides useful information when the resolving of the voltammetric signals given by two species with close half-wave potentials

**Figure 15** compares the differential pulse voltammograms of the graphene modified carbon paste electrodes, as well as the classical glassy carbon electrode. In all cases, sharp and wellresolved peaks are observed. The anodic (right side) and cathodic (left side) peaks are higher for the metal-doped reduced graphene oxide modified electrodes with the highest peak current being observed for the gold doped reduced graphene oxide modified electrode. An important parameter of an electrode material is its electronic properties, namely, the density of electronic states (DOS). The DOS of graphene materials has been reported as being high and it can be increased by varying the amounts of loaded graphene. Gold has a DOS of 0.28

Au-doped rGO modified electrodes are highly sensitive for electrochemical investigation of

The active surface areas of the graphene modified electrodes were estimated according to the

with high conductivity due to high proportion of atomic orbitals. Thus, the

*a* = 2.69 · 105 · *n*3/2 · *D*1/2 · *A* · *c* · *v*1/2 (3)

[Fe(CN)6

], solution using

is needed, producing easily quantifiable peak shaped responses.

86 Electrocatalysts for Fuel Cells and Hydrogen Evolution - Theory to Design

slope of the Ia *vs.* square root of the scan rates plot for a 1.0 mM K3

0.50 M KCl electrolyte, according to Randles–Sevcik equation [16]:

potential 5 mV.

states atom−1 eV−1

the ferri/ferro redox system.

*I*

**Figure 16.** Cyclic voltammetry of commercial Pt/C for 2000 cycles in following operation conditions: temperature 70°C; scan rate 50 mV/s.

The graphene based material modified electrodes presented herein can significantly contribute to the fundamental understanding of graphene electrochemistry and its application as an electrode material. Future work can be directed to exploring these modified electrodes towards the application of graphene materials in ORR reactions for the development of per-

**Figure 18.** Cyclic voltammetry of Au/rGO for 2000 cycles in following operation conditions: temperature 70°C; scan rate

Noble Metal Dispersed on Reduced Graphene Oxide and Its Application in PEM Fuel Cells

http://dx.doi.org/10.5772/intechopen.80941

89

In conclusion, we have successfully synthesized PtNP/rGO and Au NP/rGO nanomaterials. The successful incorporation of Au and Pt nanoparticles into the graphene oxide structure was confirmed. SEM and STEM images show the good spatial distribution of metal nanoparticles onto the layered graphene sheets. Electrocatalytic performance of the prepared materials towards the ORR reaction using cyclic voltammetry and differential pulse voltammetry show that metal-doped graphene oxide materials caused an increase in the active surface of the electrodes. The results obtained by electrochemical characterizations suggest that metaldispersed nanoparticles on reduced graphene oxide holds a great application potential as a promising electrocatalyst for oxygen reduction reaction due to the advantages of facile preparation and increased catalytic performance. It can be anticipated that the PtNP/rGO and AuNP/rGO composite materials hold great potential for developing novel ORR electrodes for PEM fuel cells. This imparts a high level of confidence that the materials developed as ORR electrocatalysts will be used in our future studies for the fabrication of cathodes for PEM fuel cell, the goal being the improvement of the fuel cell in terms of performance, life time and durability. Therefore, the reason for designed ORR electrocatalyst involves the advantage of improved catalytic activity due to the incorporation of a noble metal (platinum/gold) and

ameliorated durability from the 1-dimensional structure.

forming fuel cells.

50 mV/s.

**4. Conclusions**

**Figure 17.** Cyclic voltammetry of Pt/rGO for 2000 cycles in following operation conditions: temperature 70°C; scan rate 50 mV/s.

were observed for reduction signal, which recommend Pt- and Au-doped rGO as potential ORR catalyst for a more comprehensive investigation.

Clearly, there are many types of GO modified electrodes and each is performing for different redox system, but the electrochemistry of graphene materials is far from being fully explored. Noble Metal Dispersed on Reduced Graphene Oxide and Its Application in PEM Fuel Cells http://dx.doi.org/10.5772/intechopen.80941 89

**Figure 18.** Cyclic voltammetry of Au/rGO for 2000 cycles in following operation conditions: temperature 70°C; scan rate 50 mV/s.

The graphene based material modified electrodes presented herein can significantly contribute to the fundamental understanding of graphene electrochemistry and its application as an electrode material. Future work can be directed to exploring these modified electrodes towards the application of graphene materials in ORR reactions for the development of performing fuel cells.

### **4. Conclusions**

were observed for reduction signal, which recommend Pt- and Au-doped rGO as potential

**Figure 17.** Cyclic voltammetry of Pt/rGO for 2000 cycles in following operation conditions: temperature 70°C; scan rate

**Figure 16.** Cyclic voltammetry of commercial Pt/C for 2000 cycles in following operation conditions: temperature 70°C;

Clearly, there are many types of GO modified electrodes and each is performing for different redox system, but the electrochemistry of graphene materials is far from being fully explored.

ORR catalyst for a more comprehensive investigation.

88 Electrocatalysts for Fuel Cells and Hydrogen Evolution - Theory to Design

scan rate 50 mV/s.

50 mV/s.

In conclusion, we have successfully synthesized PtNP/rGO and Au NP/rGO nanomaterials. The successful incorporation of Au and Pt nanoparticles into the graphene oxide structure was confirmed. SEM and STEM images show the good spatial distribution of metal nanoparticles onto the layered graphene sheets. Electrocatalytic performance of the prepared materials towards the ORR reaction using cyclic voltammetry and differential pulse voltammetry show that metal-doped graphene oxide materials caused an increase in the active surface of the electrodes. The results obtained by electrochemical characterizations suggest that metaldispersed nanoparticles on reduced graphene oxide holds a great application potential as a promising electrocatalyst for oxygen reduction reaction due to the advantages of facile preparation and increased catalytic performance. It can be anticipated that the PtNP/rGO and AuNP/rGO composite materials hold great potential for developing novel ORR electrodes for PEM fuel cells. This imparts a high level of confidence that the materials developed as ORR electrocatalysts will be used in our future studies for the fabrication of cathodes for PEM fuel cell, the goal being the improvement of the fuel cell in terms of performance, life time and durability. Therefore, the reason for designed ORR electrocatalyst involves the advantage of improved catalytic activity due to the incorporation of a noble metal (platinum/gold) and ameliorated durability from the 1-dimensional structure.

### **Acknowledgements**

This work is supported by the Ministry of Research and Innovation from Romania by the National Plan of R&D, Project No. PN 18 12 01 02, PN 18 12 01 04 and by Executive Agency for Higher Education, Research, Development and Innovation, under Project M-ERA.net 37/2016. The authors wish to thank Dr. Izabela Jinga from the Centre of Organic Chemistry 'Costin D. Nenitescu' Romanian Academy for her work in the electrochemical experimental study.

[5] Li M, Zhang L, Xu Q, Niu J, Xia Z. N-doped graphene as catalysts for oxygen reduction and oxygen evolution reactions: Theoretical considerations. Journal of Catalysis.

Noble Metal Dispersed on Reduced Graphene Oxide and Its Application in PEM Fuel Cells

http://dx.doi.org/10.5772/intechopen.80941

91

[6] Agnoli S, Favaro M. Doping graphene with boron: A review of synthesis methods, physicochemical characterization, and emerging applications. Journal of Materials Chemistry

[7] Jiang L, Fan Z. Design of advanced porous graphene materials: From graphene nanomesh to 3D architectures. Nanoscale. 2014;**6**:1922-1945. DOI: 10.1039/C3NR04555B [8] Yanan T, Zongxian Y, Xianqi D. Trapping of metal atoms in the defects on graphene. The

[9] Marinoiu A, Cobzaru C, Carcadea E, Raceanu M, Atkinson I, Varlam M, et al. An experimental approach for finding low cost alternative support material in PEM fuel cells.

[10] Marinoiu A, Teodorescu C, Carcadea E, Raceanu M, Varlam M, Cobzaru C, et al. Convenient graphene based materials as potential candidates for low cost fuel cell catalysts. Reaction Kinetics Mechanisms and Catalysis. 2016;**118**:281-296. DOI: 10.1007/

[11] Marinoiu A, Raceanu M, Carcadea E, Varlam M, Stefanescu I. Doped Graphene as non-metallic catalyst for fuel cells. Materials Science. 2017;**23**:108-113. DOI: 10.5755/j01.

[12] Marinoiu A, Raceanu M, Carcadea E, Varlam M, Balan D, Ion-Ebrasu D, et al. Iodinedoped graphene for enhanced electrocatalytic oxygen reduction reaction in proton exchange membrane fuel cell applications. Journal of Electrochemical Energy Conversion

[13] Marinoiu A, Raceanu M, Carcadea E, Varlam M, Stefanescu I. Low cost iodine intercalated graphene for fuel cells electrodes. Applied Surface Science. 2017;**424**:93-100. DOI:

[14] Sun CL, Lee HH, Yang JM, Wu CC. The simultaneous electrochemical detection of ascorbic acid, dopamine, and uric acid using graphene/size-selected Pt nanocompos-

[17] Dana S, Hulstede J, Wagner P, Kruusenberg I, Tommeveski K, Dyck A, et al. Stability of Pt nanoparticles on alternative carbon supports for oxygen reduction reaction. Journal

ites. Biosensors & Bioelectronics. 2011;**26**:3450. DOI: 10.1016/j.apsusc.2017.01.295 [15] Lin WJ, Liao CS, Jhang JH, Tsai YC. Graphene modified basal and edge plane pyrolytic graphite electrodes for electrocatalytic oxidation of hydrogen peroxide and β-nicotinamide adenine dinucleotide. Electrochemistry Communications. 2009;**11**:2153

[16] Bard AJ, Faulkner LR. Electrochemical Methods. New York: Wiley; 1980

Journal of Chemical Physics. 2011;**135**:224704. DOI: 10.1063/1.3666849

2014;**314**:66-72. DOI: 10.1016/j.jcat.2014.03.011

A. 2016;**4**:5002-5025. DOI: 10.1039/C5TA10599D

Revue Roumaine de Chimie. 2016;**61**(4-5):433-440

and Storage. 2017;**14**:31001. DOI: 10.1115/1.4036684

of the Electrochemical Society. 2017;**164**:995

s11144-016-1016-7

ms.23.2.16216

10.1016/j.apsusc.2017.01.295

### **Conflict of interest**

The authors declare that there is no conflict of interest.

### **Author details**

Adriana Marinoiu1 \*, Mircea Raceanu1 , Elena Carcadea1 , Aida Pantazi2 , Raluca Mesterca2 , Oana Tutunaru2 , Simona Nica3 , Daniela Bala4 , Mihai Varlam1 and Marius Enachescu2

\*Address all correspondence to<EMAIL_ADDRESS>
1 RD Institute for Cryogenics and Isotopic Technologies—ICSI, Rm Valcea, Romania

2 Center for Surface Science and Nanotechnology, Politehnica University of Bucharest, Romania

3 Centre of Organic Chemistry 'Costin D. Nenitescu' Romanian Academy, Romania

4 Department of Physical Chemistry, Faculty of Chemistry, University of Bucharest, Romania

### **References**

[5] Li M, Zhang L, Xu Q, Niu J, Xia Z. N-doped graphene as catalysts for oxygen reduction and oxygen evolution reactions: Theoretical considerations. Journal of Catalysis. 2014;**314**:66-72. DOI: 10.1016/j.jcat.2014.03.011

**Acknowledgements**

**Conflict of interest**

**Author details**

Adriana Marinoiu1

Oana Tutunaru2

Romania

Romania

**References**

C2NR33839D

10.1039/C4CC05055J

The authors declare that there is no conflict of interest.

90 Electrocatalysts for Fuel Cells and Hydrogen Evolution - Theory to Design

\*, Mircea Raceanu1

\*Address all correspondence to<EMAIL_ADDRESS>
, Simona Nica3

48-49. DOI: 10.1126/science.1172083

This work is supported by the Ministry of Research and Innovation from Romania by the National Plan of R&D, Project No. PN 18 12 01 02, PN 18 12 01 04 and by Executive Agency for Higher Education, Research, Development and Innovation, under Project M-ERA.net 37/2016. The authors wish to thank Dr. Izabela Jinga from the Centre of Organic Chemistry 'Costin D. Nenitescu' Romanian Academy for her work in the electrochemical experimental study.

, Elena Carcadea1

, Mihai Varlam1

, Daniela Bala4

1 RD Institute for Cryogenics and Isotopic Technologies—ICSI, Rm Valcea, Romania

3 Centre of Organic Chemistry 'Costin D. Nenitescu' Romanian Academy, Romania 4 Department of Physical Chemistry, Faculty of Chemistry, University of Bucharest,

2 Center for Surface Science and Nanotechnology, Politehnica University of Bucharest,

[1] Gasteiger HA, Marković NM. Just a dream—Or future reality? Science. 2009;**324**(5923):

[2] Zhu C, Dong S. Recent progress in graphene-based nanomaterials as advanced electrocatalysts towards oxygen reduction reaction. Nanoscale. 2013;**5**:1753-1767. DOI: 10.1039/

[3] Lale IS et al. Engineered catalyst layer design with graphene-carbon black hybrid supports for enhanced platinum utilization in PEM fuel cell. International Journal of

[4] Shuo D, Anli S, Li T, Wang S. Molecular doping of graphene as metal-free electrocatalyst for oxygen reduction reaction. Chemical Communications. 2014;**50**:10672-10675. DOI:

Hydrogen Energy. 2017;**42**(2):1085-1092. DOI: 10.1016/j.ijhydene.2016.08.210

, Aida Pantazi2

, Raluca Mesterca2

and Marius Enachescu2

,

**Section 2**

**Electrocatalysts for Water Splitting**

**Electrocatalysts for Water Splitting**

**Chapter 5**

**Provisional chapter**

**Electrocatalytic Properties of Molybdenum and**

**Electrocatalytic Properties of Molybdenum and**

Valeriy Kublanovsky and Yuliya Yapontseva

Valeriy Kublanovsky and Yuliya Yapontseva

Additional information is available at the end of the chapter

Additional information is available at the end of the chapter

molybdenum, tungsten, spillover, corrosion

http://dx.doi.org/10.5772/intechopen.79058

**Abstract**

**1. Introduction**

**Tungsten Alloys in the Hydrogen Evolution Reaction**

The search for new electrode materials which are able to intensify the currently used process for the electrolytic production of pure hydrogen is an important scientific and technical problem. Promising materials for making electrodes or for the modification of currently used nickel cathodes are alloys of iron subgroup metals with molybdenum or tungsten, which show a higher catalytic activity in the hydrogen reduction reaction compared with pure nickel or cobalt and have a high corrosion resistance in aggressive media. The present chapter demonstrates that the catalytic, magnetic, and corrosive properties of coatings depend not only on the chemical composition of the alloy but also on its phase composition and morphology so that even coatings having the same chemical composition, but obtained under different conditions, possess different properties. Thus, by changing the electrolyte composition and the electrolysis parameters, one can obtain coatings with optimal set of functional properties and the distribution of metals on the surface which ensure hydrogen spillover and, hence, a high rate of the desired reaction.

**Keywords:** electrocatalytic activity, hydrogen evolution, electrodeposition,

The amount of energy consumed in the world has been steadily increasing in the recent decades, and the nonrenewable fossil energy sources account for over 80% of it [1]. In view of this, the search for efficient, environmentally appropriate methods for the generation of renewable energy is a vital present-day scientific problem [2]. One such promising trends is fuel cells [3, 4], the operation of which is directly bound up with the availability of high-purity hydrogen.

**Tungsten Alloys in the Hydrogen Evolution Reaction**

© 2016 The Author(s). Licensee InTech. This chapter is distributed under the terms of the Creative Commons Attribution License (http://creativecommons.org/licenses/by/3.0), which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

© 2018 The Author(s). Licensee IntechOpen. This chapter is distributed under the terms of the Creative Commons Attribution License (http://creativecommons.org/licenses/by/3.0), which permits unrestricted use,

distribution, and reproduction in any medium, provided the original work is properly cited.

DOI: 10.5772/intechopen.79058

#### **Electrocatalytic Properties of Molybdenum and Tungsten Alloys in the Hydrogen Evolution Reaction Electrocatalytic Properties of Molybdenum and Tungsten Alloys in the Hydrogen Evolution Reaction**

DOI: 10.5772/intechopen.79058

Valeriy Kublanovsky and Yuliya Yapontseva Valeriy Kublanovsky and Yuliya Yapontseva

Additional information is available at the end of the chapter Additional information is available at the end of the chapter

http://dx.doi.org/10.5772/intechopen.79058

#### **Abstract**

The search for new electrode materials which are able to intensify the currently used process for the electrolytic production of pure hydrogen is an important scientific and technical problem. Promising materials for making electrodes or for the modification of currently used nickel cathodes are alloys of iron subgroup metals with molybdenum or tungsten, which show a higher catalytic activity in the hydrogen reduction reaction compared with pure nickel or cobalt and have a high corrosion resistance in aggressive media. The present chapter demonstrates that the catalytic, magnetic, and corrosive properties of coatings depend not only on the chemical composition of the alloy but also on its phase composition and morphology so that even coatings having the same chemical composition, but obtained under different conditions, possess different properties. Thus, by changing the electrolyte composition and the electrolysis parameters, one can obtain coatings with optimal set of functional properties and the distribution of metals on the surface which ensure hydrogen spillover and, hence, a high rate of the desired reaction.

**Keywords:** electrocatalytic activity, hydrogen evolution, electrodeposition, molybdenum, tungsten, spillover, corrosion

### **1. Introduction**

The amount of energy consumed in the world has been steadily increasing in the recent decades, and the nonrenewable fossil energy sources account for over 80% of it [1]. In view of this, the search for efficient, environmentally appropriate methods for the generation of renewable energy is a vital present-day scientific problem [2]. One such promising trends is fuel cells [3, 4], the operation of which is directly bound up with the availability of high-purity hydrogen.

© 2016 The Author(s). Licensee InTech. This chapter is distributed under the terms of the Creative Commons Attribution License (http://creativecommons.org/licenses/by/3.0), which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited. © 2018 The Author(s). Licensee IntechOpen. This chapter is distributed under the terms of the Creative Commons Attribution License (http://creativecommons.org/licenses/by/3.0), which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

At the present time, the wide use of pure hydrogen is economically inexpedient in comparison, e.g., with the use of natural gas, because of the high cost of its production. The industrial method for hydrogen production by the electrolysis of alkaline aqueous solutions [5] has a number of disadvantages, such as the large expenditure of energy, low efficiency of the process, and the necessity of using noble metals as catalysts. Low carbon steel, which is corrosion-nonresistant in alkaline medium, and nickel also possess a catalytic effect in the hydrogen evolution reaction [6]; nevertheless, the problem of search for electrode materials with lower hydrogen evolution overpotential and high corrosion resistance remains vital. For instance, platinum group catalysts can be replaced by cheaper materials, such as nickel, molybdenum, and iron-chromium and iron-manganese alloys, in electrolysis in ionic liquids [7]. However, if the high cost of ionic liquids themselves is taken into account, there is no considerable reduction in the cost of materials for pure hydrogen production.

#### **1.1. Hydrogen electroreduction mechanism and spillover effect**

In the general form, the hydrogen electroreduction process in an alkaline medium is described by the Volmer (1)—Heyrovsky (2)—Tafel (3) mechanism with the following stages:

$$\text{Me} + \text{H}\_{2}\text{O} + \text{e} \rightarrow \text{MeH}\_{\text{ads}} \text{\textasciicircum} \tag{1}$$

$$\rm MeH\_{ads} + H\_2O + e \rightarrow H\_2 + Me + OH^- \tag{2}$$

$$\text{2MeH}\_{\text{ads}} \rightarrow \text{H}\_2 + \text{2Me} \tag{3}$$

hydrogen reduction reaction both in acidic [10–13] and in alkaline aqueous solutions [14–17], meet these requirements, and that the use of the electrochemical method for the deposition of thin alloy coatings makes it possible to reduce the cost of electrode materials and hence the

**Figure 1.** Dependence of the exchange current density of hydrogen evolution reaction in acid solutions against hydrogen-

Electrocatalytic Properties of Molybdenum and Tungsten Alloys in the Hydrogen Evolution Reaction

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97

The synergetic action of alloys in comparison with individual metals is explained by researchers not only by the type of formed alloy and its chemical composition but also by the difference in the mechanism of hydrogen electroreduction on the metals, as well as by the phenomenon of interfacial diffusion of adsorbed hydrogen, hydrogen spillover. The authors of [18] showed the frequent occurrence of this phenomenon in various catalytic processes and catalyst types. Spillover is called the transport of active species, sorbed or formed on one phase, to another phase, which does not sorb and form these species. A study of the synergetic effect of alloys of cobalt and nickel with molybdenum and tungsten with allowance for hydrogen spillover was carried out in [19] for hydrodesulphurization reaction as an example, and it was suggested that different process stages occur on different catalyst phases, between which hydrogen spillover takes place. The spillover phenomenon is of great practical importance, the study of which will help to design new multi-

As applied to the alloys of molybdenum and tungsten with iron group metals, the spillover phenomenon can account for the synergetic effect of these alloys, in the case of which the discharge step on Mo(W) takes place quickly, and on Co(Ni, Fe), the electrochemical desorption step is fast. Thus, in order that this mechanism may be effected, the active centers of different nature must be at the distance from one another that makes possible the surface diffusion of

phase catalysts, where the catalytic reaction takes place by interfacial diffusion.

hydrogen adatoms, and hence the alloy must be a solid solution or an intermetallic.

cost of produced hydrogen.

metal bond energy. Reprinted with permission from Ref. [8].

The rate of electrocatalytic reaction depends on the energy of adsorbed species, i.e., on the energy of hydrogen atoms. The plot of the exchange current density of hydrogen evolution reaction against hydrogen-metal bond energy passes through a maximum and has a volcanolike shape (**Figure 1**).

At low Ме▬Н bond energy, the process is controlled by the discharge step, reaction (1). At very high Ме▬Н bond energy, the process is controlled by the electrochemical desorption step, reaction (2). On nickel, cobalt, and iron, the rate-determining step changes from reaction (1) to (2) with increasing polarization. Thus, the most important parameter that determines electrocatalytic activity is the energy of bonding of adsorbed species to the catalyst [9]. When catalysts consisting of two metals are used, the formation of several alloy types, such as mechanical mixtures, solid solutions, and intermetallics is possible. From an analysis of the mechanism of electrocatalytic processes, metal-metal bond energy, and the properties of different alloy types, the authors of [9] conclude that the alloys formed by the metals that are on the different branches of the volcano plot and especially the alloys formed by d-metals with unoccupied d-orbitals (of groups IV–VI) and d-metals of group VIII with a large number of filled d-orbitals possess electrocatalytic activity.

It is known from literature that transition-metal alloys, viz. alloys of iron subgroup metals with molybdenum and tungsten, which show electrocatalytic properties with respect to Electrocatalytic Properties of Molybdenum and Tungsten Alloys in the Hydrogen Evolution Reaction http://dx.doi.org/10.5772/intechopen.79058 97

At the present time, the wide use of pure hydrogen is economically inexpedient in comparison, e.g., with the use of natural gas, because of the high cost of its production. The industrial method for hydrogen production by the electrolysis of alkaline aqueous solutions [5] has a number of disadvantages, such as the large expenditure of energy, low efficiency of the process, and the necessity of using noble metals as catalysts. Low carbon steel, which is corrosion-nonresistant in alkaline medium, and nickel also possess a catalytic effect in the hydrogen evolution reaction [6]; nevertheless, the problem of search for electrode materials with lower hydrogen evolution overpotential and high corrosion resistance remains vital. For instance, platinum group catalysts can be replaced by cheaper materials, such as nickel, molybdenum, and iron-chromium and iron-manganese alloys, in electrolysis in ionic liquids [7]. However, if the high cost of ionic liquids themselves is taken into account, there is no

In the general form, the hydrogen electroreduction process in an alkaline medium is described

Me + H2 O + e → MeHads + OH− (1)

MeHads + H2 O + e → H2 + Me + OH− (2)

2MeHads → H2 + 2Me (3)

The rate of electrocatalytic reaction depends on the energy of adsorbed species, i.e., on the energy of hydrogen atoms. The plot of the exchange current density of hydrogen evolution reaction against hydrogen-metal bond energy passes through a maximum and has a volcano-

At low Ме▬Н bond energy, the process is controlled by the discharge step, reaction (1). At very high Ме▬Н bond energy, the process is controlled by the electrochemical desorption step, reaction (2). On nickel, cobalt, and iron, the rate-determining step changes from reaction (1) to (2) with increasing polarization. Thus, the most important parameter that determines electrocatalytic activity is the energy of bonding of adsorbed species to the catalyst [9]. When catalysts consisting of two metals are used, the formation of several alloy types, such as mechanical mixtures, solid solutions, and intermetallics is possible. From an analysis of the mechanism of electrocatalytic processes, metal-metal bond energy, and the properties of different alloy types, the authors of [9] conclude that the alloys formed by the metals that are on the different branches of the volcano plot and especially the alloys formed by d-metals with unoccupied d-orbitals (of groups IV–VI) and d-metals of group VIII with a large number of

It is known from literature that transition-metal alloys, viz. alloys of iron subgroup metals with molybdenum and tungsten, which show electrocatalytic properties with respect to

considerable reduction in the cost of materials for pure hydrogen production.

by the Volmer (1)—Heyrovsky (2)—Tafel (3) mechanism with the following stages:

**1.1. Hydrogen electroreduction mechanism and spillover effect**

96 Electrocatalysts for Fuel Cells and Hydrogen Evolution - Theory to Design

like shape (**Figure 1**).

filled d-orbitals possess electrocatalytic activity.

**Figure 1.** Dependence of the exchange current density of hydrogen evolution reaction in acid solutions against hydrogenmetal bond energy. Reprinted with permission from Ref. [8].

hydrogen reduction reaction both in acidic [10–13] and in alkaline aqueous solutions [14–17], meet these requirements, and that the use of the electrochemical method for the deposition of thin alloy coatings makes it possible to reduce the cost of electrode materials and hence the cost of produced hydrogen.

The synergetic action of alloys in comparison with individual metals is explained by researchers not only by the type of formed alloy and its chemical composition but also by the difference in the mechanism of hydrogen electroreduction on the metals, as well as by the phenomenon of interfacial diffusion of adsorbed hydrogen, hydrogen spillover. The authors of [18] showed the frequent occurrence of this phenomenon in various catalytic processes and catalyst types. Spillover is called the transport of active species, sorbed or formed on one phase, to another phase, which does not sorb and form these species. A study of the synergetic effect of alloys of cobalt and nickel with molybdenum and tungsten with allowance for hydrogen spillover was carried out in [19] for hydrodesulphurization reaction as an example, and it was suggested that different process stages occur on different catalyst phases, between which hydrogen spillover takes place. The spillover phenomenon is of great practical importance, the study of which will help to design new multiphase catalysts, where the catalytic reaction takes place by interfacial diffusion.

As applied to the alloys of molybdenum and tungsten with iron group metals, the spillover phenomenon can account for the synergetic effect of these alloys, in the case of which the discharge step on Mo(W) takes place quickly, and on Co(Ni, Fe), the electrochemical desorption step is fast. Thus, in order that this mechanism may be effected, the active centers of different nature must be at the distance from one another that makes possible the surface diffusion of hydrogen adatoms, and hence the alloy must be a solid solution or an intermetallic.

## **2. Electrocatalytic properties of nickel alloys**

Nickel is the most commonly used cathode material in electrolyzers for hydrogen production [20] due to its catalytic properties, corrosion resistance in alkaline medium, and low cost. A possible way of intensifying the process and improving the required properties is electrode surface modification by molybdenum and tungsten alloys; therefore, many papers are devoted to the study of the electrodeposition and catalytic activity of NiMo and NiW alloys. For instance, the authors of [21] studied the electrodeposition of a NiMo alloy on a copper and a nickel substrate from a citrate electrolyte with рН 9.5 and a concentration ratio of the metals of 1/12. The best catalytic activity was found for a coating containing 41 wt.% molybdenum, and it was shown that the hydrogen evolution overpotential at the obtained alloy is lower compared with pure nickel in the model 1 М NaOH solution. In the study [22], a citrate electrolyte with рН 6.0 was also used, and it was shown that it is possible to deposit an alloy containing 28.5 аt.% Мо, which reduces the hydrogen evolution overpotential in 8 M NaOH at 90°С from 122 to 21 mV·dec-1 relative to nickel. The authors of [23] found that when a SAS is added to a citrate-ammonia electrolyte for deposition, nanocrystalline coatings having catalytic activity at a molybdenum content of 19.59 аt.% can be obtained. Chialvo and co-authors [24] studied the catalytic activity of thermal NiMo alloys as a function of the amount of molybdenum (0–25 аt.%) and showed that the higher the Мо content, the lower the hydrogen overpotential. From an analysis of literature data, it can be concluded that there is no unambiguous dependence of electrocatalytic activity on the chemical composition of the coating; for each particular deposition electrolyte, activity is proportional to the molybdenum content, but from the comparison of a large number of papers, it becomes clear that the determining factor is electrolysis conditions, which determine the morphology, the true surface area, the presence of cracks, or an oxide phase on the alloy surface. Therefore, the catalytic properties of electrocatalytic alloys are determined experimentally in each particular case.

coatings were deposited in a solution containing 0.1 mol L−1 of CoSO4

noticeable effect only at a concentration of 4.5 g L−1.

Cit (where Cit—citrate ions), 0.2 mol L−1 of K4

and in solutions containing SASs: 2 mL L−1 of water-soluble resin neonol, whose efficiency was shown when electrodepositing Co-W alloys from a citrate-ammonia electrolyte [27], and 1.5 g L−1 and 4.5 g L−1 of a nonionic SAS, OP-10 emulsifier. All experiments were performed under forced convection conditions in a current density range of 5.0–30.0 mА сm−2 at 50°С and

Electrocatalytic Properties of Molybdenum and Tungsten Alloys in the Hydrogen Evolution Reaction

It can be seen from **Figure 2** that the composition of the coatings deposited from a citratepyrophosphate electrolyte is constant regardless of deposition current density and addition of SASs. All coatings containing on an average 22 аt.% W, nevertheless, differ in the current efficiency of their deposition and in the morphology of the produced surface. A small increase in current efficiency for alloys is observed in the case of adding a SAS (neonol or OP-10) to the electrolyte. For instance, at 5.0 mА сm−2 in the presence of neonol, the current efficiency reaches 68%, and a compact, bright, adherent coating is formed. The addition of OP-10 has a

The addition of SASs to the electrolyte and deposition current density affects greatly the quality and morphology (**Figure 3**). For instance, in the electrolyte without additives at a current density of 5.0 mА сm−2, compact bright coatings are deposited. When the current density is increased to 10.0 mА сm−2, the coating becomes more stressed, and microcracks appear, and at 30.0 mА сm−2, the formation of spherulites is observed. The addition of neonol makes it possible to obtain high-quality fine-crystalline deposits in a wider current density range, and the addition OP-10, on the contrary, facilitates the formation of spherulites and favors surface

The electrocatalytic properties of СоW coatings in the hydrogen reduction reaction were investigated by stationary voltammetry in 1.0 and 6.0 mol L−1 KОН solutions because KOH is used in industrial water electrolysis, and under experimental conditions, i.e., at room tem-

**Figure 2.** Dependence of the composition (a) and current efficiency (b) of Co-W alloys obtained from electrolyte: 1—

without additives; 2—neonol; and 3 and 4—OP-10 (1.5 and 4.5 g L−1) on the deposition current density.

perature, the solution has a maximum electrical conductivity at 28 wt.% KОН.

0.2 mol L−1 of Na3

electrolyte рН 8.5.

development.

, 0.2 mol L−1 of Na2

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, 0.5 mol L−1 of Na2

P2 O7 WO4 ,

SO4

99

On the basis of investigations carried out by the authors of [25], it was concluded that molybdenum-bearing alloys are more active in the hydrogen evolution reaction in alkaline medium than tungsten-bearing alloys. When investigating the properties of Ni-Mo, Ni-W, Co-Mo, and Co-W alloys, it was also found that cobalt alloys show a higher catalytic activity than nickel alloys.

### **3. Electrocatalytic properties of cobalt alloys**

The main characteristics of electrocatalytic activity in HER are reaction exchange current and hydrogen reduction overpotential. Therefore, the main method for studying this process is voltammetry.

### **3.1. Tungsten alloys**

In the study [26], an investigation on the electrocatalytic properties of Co-W alloys electrodeposited from a polyligand citrate-pyrophosphate electrolyte had been carried out. The coatings were deposited in a solution containing 0.1 mol L−1 of CoSO4 , 0.2 mol L−1 of Na2 WO4 , 0.2 mol L−1 of Na3 Cit (where Cit—citrate ions), 0.2 mol L−1 of K4 P2 O7 , 0.5 mol L−1 of Na2 SO4 and in solutions containing SASs: 2 mL L−1 of water-soluble resin neonol, whose efficiency was shown when electrodepositing Co-W alloys from a citrate-ammonia electrolyte [27], and 1.5 g L−1 and 4.5 g L−1 of a nonionic SAS, OP-10 emulsifier. All experiments were performed under forced convection conditions in a current density range of 5.0–30.0 mА сm−2 at 50°С and electrolyte рН 8.5.

**2. Electrocatalytic properties of nickel alloys**

98 Electrocatalysts for Fuel Cells and Hydrogen Evolution - Theory to Design

are determined experimentally in each particular case.

**3. Electrocatalytic properties of cobalt alloys**

alloys.

voltammetry.

**3.1. Tungsten alloys**

Nickel is the most commonly used cathode material in electrolyzers for hydrogen production [20] due to its catalytic properties, corrosion resistance in alkaline medium, and low cost. A possible way of intensifying the process and improving the required properties is electrode surface modification by molybdenum and tungsten alloys; therefore, many papers are devoted to the study of the electrodeposition and catalytic activity of NiMo and NiW alloys. For instance, the authors of [21] studied the electrodeposition of a NiMo alloy on a copper and a nickel substrate from a citrate electrolyte with рН 9.5 and a concentration ratio of the metals of 1/12. The best catalytic activity was found for a coating containing 41 wt.% molybdenum, and it was shown that the hydrogen evolution overpotential at the obtained alloy is lower compared with pure nickel in the model 1 М NaOH solution. In the study [22], a citrate electrolyte with рН 6.0 was also used, and it was shown that it is possible to deposit an alloy containing 28.5 аt.% Мо, which reduces the hydrogen evolution overpotential in 8 M NaOH at 90°С from 122 to 21 mV·dec-1 relative to nickel. The authors of [23] found that when a SAS is added to a citrate-ammonia electrolyte for deposition, nanocrystalline coatings having catalytic activity at a molybdenum content of 19.59 аt.% can be obtained. Chialvo and co-authors [24] studied the catalytic activity of thermal NiMo alloys as a function of the amount of molybdenum (0–25 аt.%) and showed that the higher the Мо content, the lower the hydrogen overpotential. From an analysis of literature data, it can be concluded that there is no unambiguous dependence of electrocatalytic activity on the chemical composition of the coating; for each particular deposition electrolyte, activity is proportional to the molybdenum content, but from the comparison of a large number of papers, it becomes clear that the determining factor is electrolysis conditions, which determine the morphology, the true surface area, the presence of cracks, or an oxide phase on the alloy surface. Therefore, the catalytic properties of electrocatalytic alloys

On the basis of investigations carried out by the authors of [25], it was concluded that molybdenum-bearing alloys are more active in the hydrogen evolution reaction in alkaline medium than tungsten-bearing alloys. When investigating the properties of Ni-Mo, Ni-W, Co-Mo, and Co-W alloys, it was also found that cobalt alloys show a higher catalytic activity than nickel

The main characteristics of electrocatalytic activity in HER are reaction exchange current and hydrogen reduction overpotential. Therefore, the main method for studying this process is

In the study [26], an investigation on the electrocatalytic properties of Co-W alloys electrodeposited from a polyligand citrate-pyrophosphate electrolyte had been carried out. The It can be seen from **Figure 2** that the composition of the coatings deposited from a citratepyrophosphate electrolyte is constant regardless of deposition current density and addition of SASs. All coatings containing on an average 22 аt.% W, nevertheless, differ in the current efficiency of their deposition and in the morphology of the produced surface. A small increase in current efficiency for alloys is observed in the case of adding a SAS (neonol or OP-10) to the electrolyte. For instance, at 5.0 mА сm−2 in the presence of neonol, the current efficiency reaches 68%, and a compact, bright, adherent coating is formed. The addition of OP-10 has a noticeable effect only at a concentration of 4.5 g L−1.

The addition of SASs to the electrolyte and deposition current density affects greatly the quality and morphology (**Figure 3**). For instance, in the electrolyte without additives at a current density of 5.0 mА сm−2, compact bright coatings are deposited. When the current density is increased to 10.0 mА сm−2, the coating becomes more stressed, and microcracks appear, and at 30.0 mА сm−2, the formation of spherulites is observed. The addition of neonol makes it possible to obtain high-quality fine-crystalline deposits in a wider current density range, and the addition OP-10, on the contrary, facilitates the formation of spherulites and favors surface development.

The electrocatalytic properties of СоW coatings in the hydrogen reduction reaction were investigated by stationary voltammetry in 1.0 and 6.0 mol L−1 KОН solutions because KOH is used in industrial water electrolysis, and under experimental conditions, i.e., at room temperature, the solution has a maximum electrical conductivity at 28 wt.% KОН.

**Figure 2.** Dependence of the composition (a) and current efficiency (b) of Co-W alloys obtained from electrolyte: 1 without additives; 2—neonol; and 3 and 4—OP-10 (1.5 and 4.5 g L−1) on the deposition current density.

solution: [Co]:[Mo] = 20:1; 10:1: 5:1; 1:1 in a current density range of 10–100 mА сm−2 at 50°С. The studies of hydrogen electroreduction on Со-Мо alloys were carried out in solutions with

KOH. The voltammetric measurements for the determination of the kinetic parameters of hydrogen reduction were made at 25°С. The current-potential curves were recorded under potentiostatic conditions with a step of 20 mV. Before each experiment, argon was passed

In order to show clearly the catalytic effect of the alloy in comparison with an individual metal, current-potential curves of hydrogen reduction on pure cobalt deposited from a citrate-pyrophosphate electrolyte at a current density of 30 mА сm−2 and a temperature of

**Figure 5** shows current-potential curves of hydrogen electroreduction in an acidic, an alkaline, and a neutral medium on electrolytic cobalt cathodes and cathodes made of Со-Мо

Because of differences in electroreduction mechanism at different pH values, the lowest hydrogen evolution overpotential on cobalt is observed in an acidic medium and the highest in a neutral medium, as is the case with the dependence obtained for a mercury electrode and described in [30]. In the case of cobalt cathode, the coefficient *b* of the Tafel portion of the polarization curve for the acidic, alkaline, and neutral media was 0.122, 0.142, and 0.125 V, and the exchange current density was 1.93, 4.59 × 10−2 and 6.31 × 10−3 mА сm−2, respectively.

**Figure 5** shows a considerable decrease in hydrogen evolution overpotential on the alloy. For instance, at the current density of 10 mА сm−2, the overpotential value in the alkaline medium

The plots shown in **Figure 6** have been obtained on alloys electrodeposited at different current densities of 10–100 mА сm−2. The abscissa of the figure gives the ratio of the amounts of the metals in the alloy, and not the exact percentage because of the peculiarities of EDX

**Figure 5.** Stationary current-potential curves of the electroreduction of hydrogen evolution on electrolytic cobalt (a) and Co-Mo alloys (b) with the ratio [Mo]/[Mo] + [Co] = 0.33 electrodeposited at the current density 30 mA cm−2, in media with

alloys electrodeposited at the same current density and temperature.

SO4

Electrocatalytic Properties of Molybdenum and Tungsten Alloys in the Hydrogen Evolution Reaction

; 0.5 mol L−1 Na2

SO4

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; and 1.0 mol L−1

101

different mineralization and рН, viz. 0.01 mol L−1 H2

through the solution for 30 min.

50°С have been obtained.

is lower by over 200 mV.

different pH: 1—H2

SO4

, 2—KOH, and 3—Na2

SO4 .

**Figure 3.** Microphotographs of the surface of alloys obtained from electrolytes (a) without additives and (b) neonol at a current density of 10.0 mА сm−2 and (c) OP-10 at 30.0 mА сm−2.

**Figure 4.** (a) Volt-ampere curves for the electroreduction of hydrogen in a solution of 1.0 mol L−1 KOH on cobalt (1) and CoW alloys (2 and 3) electrodeposited from the electrolyte without additives at 10.0 and 20.0 mA cm−2, respectively. (b) Volt-ampere curves for the electroreduction of hydrogen in 6.0 mol L−1 KOH solution on CoW alloys, obtained from electrolytes: 1—without additives; 2—neonol; and 3 and 4—OP-10 (1.5 and 4.5 g L−1) at a current density of 10.0 mA cm−2.

**Figure 4a** shows a considerable decrease in hydrogen overpotential on CoW alloys relative to electrolytic cobalt. For instance, at the current density of 30.0 mА сm−2, the overpotential decreases by 360 mV. As one would expect, a higher electrocatalytic activity is observed for the coating with more developed surface with spherulites morphology.

**Figure 4b** shows the effect of SASs added to an electrolyte for the deposition of CoW alloys on their electrocatalytic properties in a solution analogous to industrial electrolyte for hydrogen production. It can be seen that in this particular case, the addition of SAS rather has adverse effects, i.e., smoothing the surface during electrodeposition improves the mechanical and corrosive properties of the coating, but reduces its true surface area.

#### **3.2. Molybdenum alloys**

In the study [28], cobalt and Со-Мо alloys were deposited from a citrate-pyrophosphate electrolyte, proposed earlier [29], with the different concentration ratio of the metals in the solution: [Co]:[Mo] = 20:1; 10:1: 5:1; 1:1 in a current density range of 10–100 mА сm−2 at 50°С. The studies of hydrogen electroreduction on Со-Мо alloys were carried out in solutions with different mineralization and рН, viz. 0.01 mol L−1 H2 SO4 ; 0.5 mol L−1 Na2 SO4 ; and 1.0 mol L−1 KOH. The voltammetric measurements for the determination of the kinetic parameters of hydrogen reduction were made at 25°С. The current-potential curves were recorded under potentiostatic conditions with a step of 20 mV. Before each experiment, argon was passed through the solution for 30 min.

In order to show clearly the catalytic effect of the alloy in comparison with an individual metal, current-potential curves of hydrogen reduction on pure cobalt deposited from a citrate-pyrophosphate electrolyte at a current density of 30 mА сm−2 and a temperature of 50°С have been obtained.

**Figure 5** shows current-potential curves of hydrogen electroreduction in an acidic, an alkaline, and a neutral medium on electrolytic cobalt cathodes and cathodes made of Со-Мо alloys electrodeposited at the same current density and temperature.

Because of differences in electroreduction mechanism at different pH values, the lowest hydrogen evolution overpotential on cobalt is observed in an acidic medium and the highest in a neutral medium, as is the case with the dependence obtained for a mercury electrode and described in [30]. In the case of cobalt cathode, the coefficient *b* of the Tafel portion of the polarization curve for the acidic, alkaline, and neutral media was 0.122, 0.142, and 0.125 V, and the exchange current density was 1.93, 4.59 × 10−2 and 6.31 × 10−3 mА сm−2, respectively.

**Figure 5** shows a considerable decrease in hydrogen evolution overpotential on the alloy. For instance, at the current density of 10 mА сm−2, the overpotential value in the alkaline medium is lower by over 200 mV.

The plots shown in **Figure 6** have been obtained on alloys electrodeposited at different current densities of 10–100 mА сm−2. The abscissa of the figure gives the ratio of the amounts of the metals in the alloy, and not the exact percentage because of the peculiarities of EDX

**Figure 4a** shows a considerable decrease in hydrogen overpotential on CoW alloys relative to electrolytic cobalt. For instance, at the current density of 30.0 mА сm−2, the overpotential decreases by 360 mV. As one would expect, a higher electrocatalytic activity is observed for

**Figure 4.** (a) Volt-ampere curves for the electroreduction of hydrogen in a solution of 1.0 mol L−1 KOH on cobalt (1) and CoW alloys (2 and 3) electrodeposited from the electrolyte without additives at 10.0 and 20.0 mA cm−2, respectively. (b) Volt-ampere curves for the electroreduction of hydrogen in 6.0 mol L−1 KOH solution on CoW alloys, obtained from electrolytes: 1—without additives; 2—neonol; and 3 and 4—OP-10 (1.5 and 4.5 g L−1) at a current density of 10.0 mA cm−2.

**Figure 3.** Microphotographs of the surface of alloys obtained from electrolytes (a) without additives and (b) neonol at a

current density of 10.0 mА сm−2 and (c) OP-10 at 30.0 mА сm−2.

100 Electrocatalysts for Fuel Cells and Hydrogen Evolution - Theory to Design

**Figure 4b** shows the effect of SASs added to an electrolyte for the deposition of CoW alloys on their electrocatalytic properties in a solution analogous to industrial electrolyte for hydrogen production. It can be seen that in this particular case, the addition of SAS rather has adverse effects, i.e., smoothing the surface during electrodeposition improves the mechanical and cor-

In the study [28], cobalt and Со-Мо alloys were deposited from a citrate-pyrophosphate electrolyte, proposed earlier [29], with the different concentration ratio of the metals in the

the coating with more developed surface with spherulites morphology.

rosive properties of the coating, but reduces its true surface area.

**3.2. Molybdenum alloys**

**Figure 5.** Stationary current-potential curves of the electroreduction of hydrogen evolution on electrolytic cobalt (a) and Co-Mo alloys (b) with the ratio [Mo]/[Mo] + [Co] = 0.33 electrodeposited at the current density 30 mA cm−2, in media with different pH: 1—H2 SO4 , 2—KOH, and 3—Na2 SO4 .

bright coatings are deposited in spite of the presence of microcracks. Increasing the deposition current density to 100 mА сm−2 results in the formation of spherulites and considerable surface

Electrocatalytic Properties of Molybdenum and Tungsten Alloys in the Hydrogen Evolution Reaction

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103

The conclusion that the electrocatalytic activity decreases with increasing refractory metal content may contradict papers, published earlier, on the properties of Co-Mo coatings [17, 14]. However, attention should be called on how the coating composition was changed. There are several ways of influencing the chemical composition of alloys, viz. changing the electrolyte composition and pH, temperature, current density, hydrodynamic regime, etc. For instance, in the study [14], a change in alloy composition is achieved by changing both deposition current density and electrolyte composition and in the study [17], by changing pH and, hence, the concentration ratio of different complex species that are able to be discharged to form an alloy. Thus, it is impossible to obtain a rigorous dependence of catalytic activity on the composition of coating deposited under different conditions, because the electrolysis conditions influence not only chemical but also phase composition, which in turn influences the

The effect of change in the composition of the solution for alloy electrodeposition on the electrocatalytic properties is clearly seen in **Figure 8**, which shows current-potential curves of hydrogen electroreduction on cobalt and alloys deposited at a current density of 30 mА сm−2 from electrolytes containing different sodium molybdate concentrations. It is seen from the figure that the highest hydrogen evolution overpotential is observed on cobalt deposits and the lowest on the alloy deposited from the electrolyte with [Co]:[Mo] = 10:1. The kinetic parameters of hydrogen electroreduction in an alkaline medium are presented in **Table 1**.

The difference in the value of hydrogen exchange current on alloys with the same chemical

**Figure 8.** Polarization curves obtained in KOH solution on cobalt (1) and Co-Mo alloys with the ratio of metals [Mo]/ [Mo]+[Co] equal to (2)—0.11, (3)—0.19, (4)—0.23, and (5)—0.33, respectively, electrodeposited at 30 mA·cm−2 from

development. This regularity is observed for all investigated solutions.

properties of the alloy as a whole.

composition is seen in **Figure 9**.

electrolytes [Co]:[Mo] = 20:1, 10:1, 5:1, 1:1, respectively.

**Figure 6.** Dependence of the exchange current densities of the hydrogen electroreduction reaction on the ratio of molybdenum to cobalt in alloys electrodeposited at current densities of 10, 30, and 100 mA cm−2 from the solution with a [Co]:[Mo] ratio of 1:1 in various media: 1—H2 SO4 , 2—KOH, and 3—Na2 SO4 .

analysis, in which the coating surface layer, on which a large amount of oxygen and carbon are adsorbed. The adsorbed light elements can be removed by polishing the surface or treating it with argon ions. Both in this and in the initial case, the ratio of the metals in the alloy remains constant, as was shown in [17], with a coating depth of up to 100 nm. Thus, the ratio of molybdenum and cobalt in the surface layer, determined by EDX analysis, corresponds to the volumetric chemical composition of the alloy.

In the alloys deposited from an electrolyte with the concentration ratio [Co]:[Mo] = 1:1, the amount of molybdenum decreases and the exchange current density of the hydrogen reduction reaction increases with increasing deposition current density, which can be accounted for in terms of the value which the surface morphology and the true electrode area have, as was shown in [17]. **Figure 7** shows surface micrographs of alloys electrodeposited at two current densities of 10 and 100 mА сm−2. It can be seen that at a low current density, smooth, fine-crystalline, and

**Figure 7.** The morphology of Co-Mo alloys precipitated from electrolytes [Co]:[Mo] = 1:1 (a and b) and [Co]:[Mo] = 5:1 (c and d) at current densities of: a and c—10 mA cm−2; b and d—100 mA cm−2 and the ratio of metals [Mo]/[Mo] + [Co] equal to 0.39, 0.27, 0.28, and 0.21, respectively.

bright coatings are deposited in spite of the presence of microcracks. Increasing the deposition current density to 100 mА сm−2 results in the formation of spherulites and considerable surface development. This regularity is observed for all investigated solutions.

The conclusion that the electrocatalytic activity decreases with increasing refractory metal content may contradict papers, published earlier, on the properties of Co-Mo coatings [17, 14]. However, attention should be called on how the coating composition was changed. There are several ways of influencing the chemical composition of alloys, viz. changing the electrolyte composition and pH, temperature, current density, hydrodynamic regime, etc. For instance, in the study [14], a change in alloy composition is achieved by changing both deposition current density and electrolyte composition and in the study [17], by changing pH and, hence, the concentration ratio of different complex species that are able to be discharged to form an alloy. Thus, it is impossible to obtain a rigorous dependence of catalytic activity on the composition of coating deposited under different conditions, because the electrolysis conditions influence not only chemical but also phase composition, which in turn influences the properties of the alloy as a whole.

The effect of change in the composition of the solution for alloy electrodeposition on the electrocatalytic properties is clearly seen in **Figure 8**, which shows current-potential curves of hydrogen electroreduction on cobalt and alloys deposited at a current density of 30 mА сm−2 from electrolytes containing different sodium molybdate concentrations. It is seen from the figure that the highest hydrogen evolution overpotential is observed on cobalt deposits and the lowest on the alloy deposited from the electrolyte with [Co]:[Mo] = 10:1. The kinetic parameters of hydrogen electroreduction in an alkaline medium are presented in **Table 1**.

analysis, in which the coating surface layer, on which a large amount of oxygen and carbon are adsorbed. The adsorbed light elements can be removed by polishing the surface or treating it with argon ions. Both in this and in the initial case, the ratio of the metals in the alloy remains constant, as was shown in [17], with a coating depth of up to 100 nm. Thus, the ratio of molybdenum and cobalt in the surface layer, determined by EDX analysis, corresponds to

**Figure 6.** Dependence of the exchange current densities of the hydrogen electroreduction reaction on the ratio of molybdenum to cobalt in alloys electrodeposited at current densities of 10, 30, and 100 mA cm−2 from the solution with

, 2—KOH, and 3—Na2

SO4 .

SO4

In the alloys deposited from an electrolyte with the concentration ratio [Co]:[Mo] = 1:1, the amount of molybdenum decreases and the exchange current density of the hydrogen reduction reaction increases with increasing deposition current density, which can be accounted for in terms of the value which the surface morphology and the true electrode area have, as was shown in [17]. **Figure 7** shows surface micrographs of alloys electrodeposited at two current densities of 10 and 100 mА сm−2. It can be seen that at a low current density, smooth, fine-crystalline, and

**Figure 7.** The morphology of Co-Mo alloys precipitated from electrolytes [Co]:[Mo] = 1:1 (a and b) and [Co]:[Mo] = 5:1 (c and d) at current densities of: a and c—10 mA cm−2; b and d—100 mA cm−2 and the ratio of metals [Mo]/[Mo] + [Co]

the volumetric chemical composition of the alloy.

102 Electrocatalysts for Fuel Cells and Hydrogen Evolution - Theory to Design

a [Co]:[Mo] ratio of 1:1 in various media: 1—H2

equal to 0.39, 0.27, 0.28, and 0.21, respectively.

The difference in the value of hydrogen exchange current on alloys with the same chemical composition is seen in **Figure 9**.

**Figure 8.** Polarization curves obtained in KOH solution on cobalt (1) and Co-Mo alloys with the ratio of metals [Mo]/ [Mo]+[Co] equal to (2)—0.11, (3)—0.19, (4)—0.23, and (5)—0.33, respectively, electrodeposited at 30 mA·cm−2 from electrolytes [Co]:[Mo] = 20:1, 10:1, 5:1, 1:1, respectively.

In **Figure 9**, attention should be called on how the current efficiency of the deposition of the alloy and its electrocatalytic activity correlate with each other. In spite of the fact that the current efficiency was measured for a citrate-pyrophosphate electrolyte for deposition, this electrolyte is a weakly alkaline salt solutions, in which the alloys that are formed also exhibit electrocatalytic activity against the parallel cathodes process, with hydrogen electroreduction; therefore, the plots shown in **Figure 9** are of antibate character. Therefore, alloys, electrodeposited at high current densities up to 100 mA cm−2 and having the highest catalytic activity (for all deposition electrolytes) are deposited with the lowest current

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From the obtained data, it can be concluded that in the case of Со-Мо alloys electrodeposited from citrate-pyrophosphate electrolytes, the hydrogen exchange current decreases for each particular electrolyte with increasing amount of molybdenum in the alloy. However, in a series of electrolytes with the different concentration ratio of the discharging metals, the alloys that differ greatly in chemical composition can have the same electrocatalytic activity; this can be seen in **Figure 10**, which shows values of hydrogen exchange currents and stationary potentials for alloys deposited at the same current density, but from different

An extreme form is typical both of the plots of hydrogen exchange current density vs. the ratio of the alloy components and of the stationary potential values of the alloy in the КОН

Thus, the optimal electrolyte for the making of electrocatalytic Со-Мо alloys is the electrolyte with a cobalt and molybdenum concentration ratio of 10:1, which occupies an intermediate position in the series of investigated solutions; so, increasing or decreasing the concentration of sodium molybdate and hence of molybdenum in the alloy results in the deterioration of the

**Figure 10.** The dependence of the exchange current (1 and 2) and the stationary potential (3 and 4) in the KOH solution

on the molybdenum and cobalt ratio in alloys deposited at current densities, mА cm−2. 1: 3—30; and 2: 4—10.

efficiency.

electrolytes.

solution.

catalytic properties of the coating.

Here, jdep. is the current density of alloy deposition; Е0 is the stationary potential of the alloy in a КОН solution; *а* and *b* are coefficients in the Tafel equation; and j0 is hydrogen exchange current density. \* The ratio of the metals was calculated based on their atomic fraction in alloys.

**Table 1.** Kinetic parameters of hydrogen reduction reaction in a 1 mol L−1 KОН.

**Figure 9.** The dependence of the exchange current of the hydrogen reduction in a 1.0 mol L−1 KOH solution (1 and 2) and the current efficiency (3 and 4) of the Co-Mo alloys electrodeposited in the electrolytes [Co]:[Mo] = 5:1 and [Co]:[Mo] = 1:1 on the ratio of metals in the alloy.

In **Figure 9**, attention should be called on how the current efficiency of the deposition of the alloy and its electrocatalytic activity correlate with each other. In spite of the fact that the current efficiency was measured for a citrate-pyrophosphate electrolyte for deposition, this electrolyte is a weakly alkaline salt solutions, in which the alloys that are formed also exhibit electrocatalytic activity against the parallel cathodes process, with hydrogen electroreduction; therefore, the plots shown in **Figure 9** are of antibate character. Therefore, alloys, electrodeposited at high current densities up to 100 mA cm−2 and having the highest catalytic activity (for all deposition electrolytes) are deposited with the lowest current efficiency.

From the obtained data, it can be concluded that in the case of Со-Мо alloys electrodeposited from citrate-pyrophosphate electrolytes, the hydrogen exchange current decreases for each particular electrolyte with increasing amount of molybdenum in the alloy. However, in a series of electrolytes with the different concentration ratio of the discharging metals, the alloys that differ greatly in chemical composition can have the same electrocatalytic activity; this can be seen in **Figure 10**, which shows values of hydrogen exchange currents and stationary potentials for alloys deposited at the same current density, but from different electrolytes.

An extreme form is typical both of the plots of hydrogen exchange current density vs. the ratio of the alloy components and of the stationary potential values of the alloy in the КОН solution.

Thus, the optimal electrolyte for the making of electrocatalytic Со-Мо alloys is the electrolyte with a cobalt and molybdenum concentration ratio of 10:1, which occupies an intermediate position in the series of investigated solutions; so, increasing or decreasing the concentration of sodium molybdate and hence of molybdenum in the alloy results in the deterioration of the catalytic properties of the coating.

**Figure 10.** The dependence of the exchange current (1 and 2) and the stationary potential (3 and 4) in the KOH solution on the molybdenum and cobalt ratio in alloys deposited at current densities, mА cm−2. 1: 3—30; and 2: 4—10.

**Figure 9.** The dependence of the exchange current of the hydrogen reduction in a 1.0 mol L−1 KOH solution (1 and 2) and the current efficiency (3 and 4) of the Co-Mo alloys electrodeposited in the electrolytes [Co]:[Mo] = 5:1 and [Co]:[Mo] = 1:1

on the ratio of metals in the alloy.

**Electrolyte j**

**dep. (mА сm−2) Е0**

104 Electrocatalysts for Fuel Cells and Hydrogen Evolution - Theory to Design

Here, jdep. is the current density of alloy deposition; Е0

The ratio of the metals was calculated based on their atomic fraction in alloys.

**Table 1.** Kinetic parameters of hydrogen reduction reaction in a 1 mol L−1 KОН.

are coefficients in the Tafel equation; and j0

\*

Co 30 −0.821 0.190 0.142 4.59 × 10−2 — [Co]:[Mo] = 20:1 10 −0.910 0.181 0.134 4.46 × 10−2 0.22

[Co]:[Mo] = 10:1 10 −0.940 0.125 0.091 9.23 × 10−2 0.25

[Co]:[Mo] = 5:1 10 −0.920 0.130 0.155 1.25 × 10−1 0.28

[Co]:[Mo] = 1:1 10 −0.900 0.189 0.146 5.08 × 10−2 0.39

 **(V)** *а b* **j**

30 −0.985 0.038 0.077 3.21 × 10−1 0.11

20 −1.005 0.045 0.058 1.67 × 10−1 0.23 30 −1.025 0.025 0.056 3.58 × 10−1 0.19

30 −0.980 0.050 0.062 1.56 × 10−1 0.23 100 −1.000 0.035 0.053 2.19 × 10−1 0.21

 −0.935 0.110 0.089 5.81 × 10−2 0.37 −0.980 0.083 0.080 9.17 × 10−2 0.33 −0.965 0.069 0.077 1.27 × 10−1 0.30 −1.010 0.043 0.068 2.33 × 10−1 0.27

is hydrogen exchange current density.

**0**

 **(mА сm−2) [Мо]/([Мо] + [Со])\***

is the stationary potential of the alloy in a КОН solution; *а* and *b*

It is known [10] that the electrocatalytic activity of electrode material can be increased by several ways, e.g., by increasing the true working surface area of the catalyst, viz. by making the catalyst not in the form of a continuous film, but in the form of nanofibers [31]. The true surface area must be estimated when fabricating continuous alloy coatings, as this was done in [17]; it should be noted, however, that the factor of surface development is not determining in the ascertainment of the causes of the electrocatalytic activity of the materials under investigation. Another important factor is the nature of the metals comprising the alloy, which was shown in [25], but the physicochemical properties of one metal do not account for the synergetic effect in the use of alloys. The phenomenon that describes most reliably the synergetic action of two or more metals is spillover effect, which was described in [10–12]. Since hydrogen evolution occurs on Со and Мо with different rate-determining steps, as was said above, the occurrence of hydrogen spillover makes it possible to bring about a fact reaction (1) on molybdenum atoms and a rapid electrochemical desorption (2) on cobalt atoms.

Because of this, the synergetic effect of the alloy will manifest itself when the atoms are arranged in an optimal manner to perform sequential reaction steps. This is possible when the alloy is an intermetallic, an amorphous phase, or solid solutions with nanosized crystals.

and compact deposits are formed. Since the chemical composition of the coatings deposited from a citrate-pyrophosphate electrolyte is almost constant, the dependence of polarization resistance on deposition current density can be attributed to a difference in surface morphology and the appearance of microcracks on increasing the deposition current. On the whole, the corrosion rate of the obtained alloys is comparable with that in an analogous solution of electrolytic chromium deposited from Cr(III) and Cr(VI) baths in the study [33] (**Figure 12**). The parameters of the corrosion process, determined by the electrochemical impedance method, have been calculated on the basis of an equivalent circuit comprising the ohmic resistance of the solution, corrosion resistance, a constant phase element, and Warburg impedance (**Table 3**). The corrosion studies, carried out by us, of CoW alloys in a 6.0 mol L−1 КОН solution showed that the corrosion resistance in a concentrated КОН solution (**Figure 12**) is two order of magnitude lower than in a model NaCl solution; nevertheless, the coatings can be considered corrosion proof. It was noted that the coatings obtained for the experiment are of the worst quality in comparison with others, since they are intermediate at the transition from fine crystalline to spherulite deposits. The deposits of these two types are dense and smooth, and only at 10.0 mА сm−2, the largest number of cracks is observed, which accordingly affects the properties of coatings; nevertheless, the coatings have a low corrosion rate and are passivated in alkaline solution.

**j (mА сm−2) W (аt.%) R (kОhm сm−2) Rp (kОhm сm−2) Еcorr (V) Jcorr × 105**

Here, j is alloy deposition current density; W is tungsten content, аt.%; R is corrosion resistance determined by the impedance method; Rp is corrosion resistance determined by voltammetry; Еcorr is corrosion potential; and jcorr is

1 5.0 23.3 18.0 41.2 −0.782 1.35 2 10.0 24.0 18.8 6.9 −0.834 8.53 3 20.0 20.8 12.8 16.6 −0.786 5.24  **(А сm−2)**

**Figure 11.** Electrochemical impedance spectra (a) and current-potential curves (b) obtained in the case of corrosion of coatings electrodeposited from a citrate-pyrophosphate electrolyte at the current densities mА cm−2: 1—5.0; 2—10.0; and

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3—20.0.

corrosion current density.

**Table 2.** Corrosion parameters of alloys in a 3.5% NaCl solution.

When we attempted to investigate the coatings obtained by us by X-ray phase analysis, we have not obtained somewhat well-defined peaks of phases, i.e., the coatings were either very fine-crystalline, below the device sensitivity level, or amorphous. However, different properties (e.g., corrosion or magnetic properties) of Co-Mo alloys of the same composition have also been obtained by us earlier. Their phase composition has been studied by us by stripping analysis and shown in [32].

### **4. Corrosion properties**

Some of the main characteristics of modern catalytic materials are not only their activity in the desired reaction but also mechanical strength and corrosion resistance in aggressive media; therefore, the comprehensive investigation of the physicochemical properties of the electrode material is an important scientific and technical problem.

### **4.1. Tungsten alloys**

In the study [26], the corrosion characteristics of electrolytic Co-W alloys deposited from a citrate-pyrophosphate electrolyte in 3.5% NaCl and 6 mol L−1 KOH solutions at 25°С have been determined by EIS and stationary voltammetry (**Figure 11**).

The impedance hodographs obtained at a stationary potential in a corrosive medium can be described by a circuit comprising the ohmic resistance of the solution, charge transfer (corrosion) resistance, and a constant phase element. The corrosion parameters calculated in accordance with this equivalent circuit are listed **Table 2**.

The coating deposited at a current density of 5.0 mА сm−2 has the highest corrosion stability because in the region of kinetic control of electrochemical reaction, most fine-crystalline

Electrocatalytic Properties of Molybdenum and Tungsten Alloys in the Hydrogen Evolution Reaction http://dx.doi.org/10.5772/intechopen.79058 107

It is known [10] that the electrocatalytic activity of electrode material can be increased by several ways, e.g., by increasing the true working surface area of the catalyst, viz. by making the catalyst not in the form of a continuous film, but in the form of nanofibers [31]. The true surface area must be estimated when fabricating continuous alloy coatings, as this was done in [17]; it should be noted, however, that the factor of surface development is not determining in the ascertainment of the causes of the electrocatalytic activity of the materials under investigation. Another important factor is the nature of the metals comprising the alloy, which was shown in [25], but the physicochemical properties of one metal do not account for the synergetic effect in the use of alloys. The phenomenon that describes most reliably the synergetic action of two or more metals is spillover effect, which was described in [10–12]. Since hydrogen evolution occurs on Со and Мо with different rate-determining steps, as was said above, the occurrence of hydrogen spillover makes it possible to bring about a fact reaction (1)

106 Electrocatalysts for Fuel Cells and Hydrogen Evolution - Theory to Design

on molybdenum atoms and a rapid electrochemical desorption (2) on cobalt atoms.

analysis and shown in [32].

**4. Corrosion properties**

**4.1. Tungsten alloys**

material is an important scientific and technical problem.

dance with this equivalent circuit are listed **Table 2**.

been determined by EIS and stationary voltammetry (**Figure 11**).

Because of this, the synergetic effect of the alloy will manifest itself when the atoms are arranged in an optimal manner to perform sequential reaction steps. This is possible when the alloy is an intermetallic, an amorphous phase, or solid solutions with nanosized crystals. When we attempted to investigate the coatings obtained by us by X-ray phase analysis, we have not obtained somewhat well-defined peaks of phases, i.e., the coatings were either very fine-crystalline, below the device sensitivity level, or amorphous. However, different properties (e.g., corrosion or magnetic properties) of Co-Mo alloys of the same composition have also been obtained by us earlier. Their phase composition has been studied by us by stripping

Some of the main characteristics of modern catalytic materials are not only their activity in the desired reaction but also mechanical strength and corrosion resistance in aggressive media; therefore, the comprehensive investigation of the physicochemical properties of the electrode

In the study [26], the corrosion characteristics of electrolytic Co-W alloys deposited from a citrate-pyrophosphate electrolyte in 3.5% NaCl and 6 mol L−1 KOH solutions at 25°С have

The impedance hodographs obtained at a stationary potential in a corrosive medium can be described by a circuit comprising the ohmic resistance of the solution, charge transfer (corrosion) resistance, and a constant phase element. The corrosion parameters calculated in accor-

The coating deposited at a current density of 5.0 mА сm−2 has the highest corrosion stability because in the region of kinetic control of electrochemical reaction, most fine-crystalline

**Figure 11.** Electrochemical impedance spectra (a) and current-potential curves (b) obtained in the case of corrosion of coatings electrodeposited from a citrate-pyrophosphate electrolyte at the current densities mА cm−2: 1—5.0; 2—10.0; and 3—20.0.

and compact deposits are formed. Since the chemical composition of the coatings deposited from a citrate-pyrophosphate electrolyte is almost constant, the dependence of polarization resistance on deposition current density can be attributed to a difference in surface morphology and the appearance of microcracks on increasing the deposition current. On the whole, the corrosion rate of the obtained alloys is comparable with that in an analogous solution of electrolytic chromium deposited from Cr(III) and Cr(VI) baths in the study [33] (**Figure 12**).

The parameters of the corrosion process, determined by the electrochemical impedance method, have been calculated on the basis of an equivalent circuit comprising the ohmic resistance of the solution, corrosion resistance, a constant phase element, and Warburg impedance (**Table 3**).

The corrosion studies, carried out by us, of CoW alloys in a 6.0 mol L−1 КОН solution showed that the corrosion resistance in a concentrated КОН solution (**Figure 12**) is two order of magnitude lower than in a model NaCl solution; nevertheless, the coatings can be considered corrosion proof. It was noted that the coatings obtained for the experiment are of the worst quality in comparison with others, since they are intermediate at the transition from fine crystalline to spherulite deposits. The deposits of these two types are dense and smooth, and only at 10.0 mА сm−2, the largest number of cracks is observed, which accordingly affects the properties of coatings; nevertheless, the coatings have a low corrosion rate and are passivated in alkaline solution.

Here, j is alloy deposition current density; W is tungsten content, аt.%; R is corrosion resistance determined by the impedance method; Rp is corrosion resistance determined by voltammetry; Еcorr is corrosion potential; and jcorr is corrosion current density.

**Table 2.** Corrosion parameters of alloys in a 3.5% NaCl solution.

**Figure 12.** Spectra of electrochemical impedance (a) and current-potential curves (b), obtained in the case of corrosion in a 6.0 mol L−1 KOH solution, for coatings electrodeposited at a current density of 10.0 mA cm−2 from electrolytes 1—no additives; 2—neonol; 3 and 4—OP-10 (1.5 and 4.5 g L−1).

The corrosion test of the obtained coatings was carried out in a sulfate-chloride solution. The calculation of corrosion resistance from electrochemical impedance data has been performed on the basis of an equivalent circuit comprising the ohmic resistance of the solution, charge

**Figure 13.** Dependence of the ratio of the metals content (a) and current efficiency (b) for alloys electrodeposited from

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Alloy samples electrodeposited from an electrolyte with [Co]/[Mo] = 5/1 with increasing current density, i.e., with decreasing molybdenum content (**Figure 13**, curve 2), and an alloy electrodeposited from an analogous citrate electrolyte containing no pyrophosphate at 30 mА сm−2, have been investigated. **Figure 14** and **Table 4** show no clear correlation between the molybdenum content of the alloy and corrosion resistance. Besides, the coatings deposited from solutions with the same ratio of the metals in the presence and absence of pyrophosphate are similar in

The anticorrosion resistance of Co-Mo coatings is usually associated with the percentage content of molybdenum in them as a more corrosion-resistant metal, and the magnetic properties

**Figure 14.** Stationary current-potential curves (a) and electrochemical impedance spectra (b) of the corrosion of alloys deposited from polyligand electrolyte (1–3) and a citrate electrolyte (4) at the deposition current densities, mА cm−2:

anticorrosion properties despite the difference in their chemical composition.

electrolytes with a concentration ratios [Co]/[Mo] = 1/1 and [Co]/[Mo] = 5/1 on current density.

transfer resistance, and a constant phase element.

1—10; 2 and 4—30; and 3—50.

**Table 3.** Corrosion parameters of alloys in a 6 mol L−1 КОН solution.

#### **4.2. Molybdenum alloys**

To determine the corrosion properties of electrolytic Со-Мо alloys in the study [34], the coatings were deposited from a citrate-pyrophosphate electrolyte with different concentration ratios of the metals: [Co]/[Mo] = 1/1 and [Co]/[Mo] = 5/1. The aim of the authors was a large percentage of a component having ferromagnetic properties, i.e., cobalt. To fabricate cobaltrich alloys, electrolytes with low sodium molybdate content and, hence, with small amount of molybdenum in the coating are used.

As is seen from **Figure 13**, the amount of molybdenum in the alloy electrodeposited from an electrolyte at [Co]/[Mo] = 5/1 decreased relative to the alloy deposited from an electrolyte with [Co]/[Mo] = 1/1; in this case, however, no direct proportionality between the molybdenum content of the alloy and solution is observed. For instance, the concentration ratio of molybdate and cobalt in the electrolyte was 0.2 and changed from 0.4 to 0.27 in the coating. The amount of cobalt in the deposit changes only slightly on increasing the current density, but the percentage of nonmetallic impurities, mainly oxygen, increases, which affect the internal stresses in the deposit. Nevertheless, this change in the concentration ratio of the metals in the solution leads to a great increase in current efficiency for the alloy at low current densities (**Figure 13b**). Thus, it can be stated that in terms of the cobalt content of the alloy, the most optimal conditions for the deposition of magnetic coatings are current densities of 10–50 mА сm−2.

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**Figure 13.** Dependence of the ratio of the metals content (a) and current efficiency (b) for alloys electrodeposited from electrolytes with a concentration ratios [Co]/[Mo] = 1/1 and [Co]/[Mo] = 5/1 on current density.

The corrosion test of the obtained coatings was carried out in a sulfate-chloride solution. The calculation of corrosion resistance from electrochemical impedance data has been performed on the basis of an equivalent circuit comprising the ohmic resistance of the solution, charge transfer resistance, and a constant phase element.

Alloy samples electrodeposited from an electrolyte with [Co]/[Mo] = 5/1 with increasing current density, i.e., with decreasing molybdenum content (**Figure 13**, curve 2), and an alloy electrodeposited from an analogous citrate electrolyte containing no pyrophosphate at 30 mА сm−2, have been investigated. **Figure 14** and **Table 4** show no clear correlation between the molybdenum content of the alloy and corrosion resistance. Besides, the coatings deposited from solutions with the same ratio of the metals in the presence and absence of pyrophosphate are similar in anticorrosion properties despite the difference in their chemical composition.

The anticorrosion resistance of Co-Mo coatings is usually associated with the percentage content of molybdenum in them as a more corrosion-resistant metal, and the magnetic properties

**4.2. Molybdenum alloys**

of molybdenum in the coating are used.

additives; 2—neonol; 3 and 4—OP-10 (1.5 and 4.5 g L−1).

108 Electrocatalysts for Fuel Cells and Hydrogen Evolution - Theory to Design

**Table 3.** Corrosion parameters of alloys in a 6 mol L−1 КОН solution.

To determine the corrosion properties of electrolytic Со-Мо alloys in the study [34], the coatings were deposited from a citrate-pyrophosphate electrolyte with different concentration ratios of the metals: [Co]/[Mo] = 1/1 and [Co]/[Mo] = 5/1. The aim of the authors was a large percentage of a component having ferromagnetic properties, i.e., cobalt. To fabricate cobaltrich alloys, electrolytes with low sodium molybdate content and, hence, with small amount

**Figure 12.** Spectra of electrochemical impedance (a) and current-potential curves (b), obtained in the case of corrosion in a 6.0 mol L−1 KOH solution, for coatings electrodeposited at a current density of 10.0 mA cm−2 from electrolytes 1—no

 **(А сm−2)**

**Electrolyte W (аt.%) R (kOhm сm−2) Rp (kOhm сm−2) Еcorr (V) Jcorr × 103**

 24.0 0.92 0.58 −1.03 0.84 23.7 0.46 0.37 −1.05 0.11 24.0 0.34 0.40 −1.04 0.17 22.6 0.40 0.48 −1.03 0.12

As is seen from **Figure 13**, the amount of molybdenum in the alloy electrodeposited from an electrolyte at [Co]/[Mo] = 5/1 decreased relative to the alloy deposited from an electrolyte with [Co]/[Mo] = 1/1; in this case, however, no direct proportionality between the molybdenum content of the alloy and solution is observed. For instance, the concentration ratio of molybdate and cobalt in the electrolyte was 0.2 and changed from 0.4 to 0.27 in the coating. The amount of cobalt in the deposit changes only slightly on increasing the current density, but the percentage of nonmetallic impurities, mainly oxygen, increases, which affect the internal stresses in the deposit. Nevertheless, this change in the concentration ratio of the metals in the solution leads to a great increase in current efficiency for the alloy at low current densities (**Figure 13b**). Thus, it can be stated that in terms of the cobalt content of the alloy, the most optimal condi-

tions for the deposition of magnetic coatings are current densities of 10–50 mА сm−2.

**Figure 14.** Stationary current-potential curves (a) and electrochemical impedance spectra (b) of the corrosion of alloys deposited from polyligand electrolyte (1–3) and a citrate electrolyte (4) at the deposition current densities, mА cm−2: 1—10; 2 and 4—30; and 3—50.

**Table 4.** Dependence of the corrosion parameters of Со-Мо alloys on alloy composition.

of coatings—with a cobalt content as a metal with ferromagnetic properties. However, the functional properties of coatings can depend not only on the chemical composition of the alloy but also on its phase composition, morphology, thickness, porosity, and other factors.

To study the phase composition, the electrochemical method of linear stripping voltammetric analysis (LSVA) was used [35]. An advantage of this method, besides simplicity, is the possibility to follow the dissolution dynamics of the alloy. Before the stripping analysis, a 0.5 μM thick layer of Co or Co-Mo alloys were deposited onto the working electrode from a citratepyrophosphate electrolyte with the concentration ratios of the metals [Co]/[Mo] = 1/1 and [Co]/

is saturation magnetization.

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111

Electrocatalytic Properties of Molybdenum and Tungsten Alloys in the Hydrogen Evolution Reaction

**Deposition electrolyte j (mА сm−2) t (°С) Н (Oe) MR (Gs) МS (Gs)** [Co]/[Mo] = 1/1 30 25 155 5.0 113 [Co]/[Mo] = 1/1 40 50 117 20.0 290 [Co]/[Mo] = 5/1 10 50 102 252 927

Here, Н is coercive force, MR is remanent magnetization, and МS

The electrolyte for the anodic dissolution of the obtained alloy deposits must meet the following requirements: it must have a high electrical conductivity, be nonaggressive toward the coating, and not cause spontaneous chemical dissolution. In this electrolyte, an electrochemical side reaction paralleling the anodic dissolution of the deposit under investigation must be ruled out. The use of various acids as working solutions was considered inexpedient since the electrochemical process in such electrolytes is paralleled by the chemical dissolution of the coating under analysis. Alkaline solutions are unsuitable for use as working electrolytes because of passivation processes on the surface of samples under investigation. The optimal solution for the anodic dissolution of coatings under investigation is NaCl solution, which makes it possible to obtain on the current-potential curves clear peaks corresponding to the dissolution potentials of the various phases of the alloy. The stripping analysis of coatings was performed in a 0.5 М NaCl solution at 25°С on a rotating disk electrode at a rotational

**Figure 15** shows a current-potential curve of the dissolution of freshly deposited cobalt (curve 1) in a 0.5 М NaCl solution. The observed dissolution peaks are traditionally attributed to the complex phase structure of metals and alloys, but their number depends on the electrolyte in which dissolution is performed [35]. The plot of cobalt dissolution current vs. potential exhibits three peaks, which we further use in order to distinguish the peaks of dissolution of the alloy from the peaks of cobalt dissolution. The figure shows plots except the oxygen and chlorine evolution curve. It can be seen that in the case of dissolution of alloys, the magnitude of the peaks and their number are different. For instance, for the alloys deposited from an electrolyte with the same concentration ratio of the metals, the magnitude of peak 1 is the same, but besides it, only one large peak is observed for the alloy obtained at 50°С and 40 mА сm−2, whereas two peaks are observed for the alloy obtained at 25°С and 30 mА сm−2. However, for the alloy deposited from an electrolyte with lower molybdate content, the magnitude of peak 1 is much larger than for other alloys. Based on the potentials of the peaks, the known cathodic quantity of electricity, the phase diagram of the double layer, and stoichiometry, it can be suggested that peaks 1 and 3 relate to cobalt dissolution and peak 2 to

the dissolution of a solid solution of the chemical compound СоМо in cobalt.

[Mo] = 5/1 at a current density of 10–100 mА сm−2 and a temperature of 25 and 50°С.

**Table 6.** Magnetic properties of alloys having the same chemical composition (21.2 аt.% Мо).

speed of 774 rpm.

When studying the corrosion and magnetic properties of Со-Мо coatings [32] deposited from a citrate-pyrophosphate electrolyte, it was found that for the coatings obtained under different electrolysis conditions and having the same chemical composition, the corrosion stability and magnetic parameters are different; it was suggested that the properties of the alloy largely depend on its phase composition.

In the study, the corrosion and magnetic properties of coatings with same Mo content of the alloy (21.2 аt.%), deposited from a citrate-pyrophosphate electrolyte under different electrolysis conditions, have been investigated. The corrosion stability of the coatings was studied in a solution containing 7 g L−1 Na2 SO4 and 7 g L−1 NaCl at рН 6.0 and 24 ± 1°С (**Table 5**). The magnetic properties (**Table 6**) of the obtained deposits were determined by means of a vibrating sample magnetometer in fields of up to 20 kOe at room temperature (**Table 5**).

The magnetic characteristics of such Alloys are also given. Their calculated values are listed in **Table 6**. The main criteria for evaluating the properties of soft-magnetic materials are low coercive force, low remanent magnetization and high saturation magnetization, as well as the ability to reach saturation magnetization in low intensity fields. It is evident from **Table 6** that the largest saturation magnetization values—927 Gs were obtained at a magnetic field intensity of 3 kOe for the alloys deposited from an electrolyte with a ratio of 5:1. For the coatings deposited from an electrolyte with a ratio of 1:1, no saturation magnetization is observed even at 20 kOe; the maximum value obtained under experimental conditions for alloys deposited at 25° and 50°С was 113 and 290 Gs, respectively. Thus, it can be concluded that the alloy deposited from an electrolyte with the concentration ratio of the metals [Co]/[Mo] = 5/1. We assumed that such a difference in functional properties for the coatings having the same chemical composition may be due to a difference in their phase composition.

**Table 5.** Corrosion properties of alloys having the same chemical composition (21.2 аt.% Мо).

**Table 6.** Magnetic properties of alloys having the same chemical composition (21.2 аt.% Мо).

of coatings—with a cobalt content as a metal with ferromagnetic properties. However, the functional properties of coatings can depend not only on the chemical composition of the alloy but also on its phase composition, morphology, thickness, porosity, and other factors. When studying the corrosion and magnetic properties of Со-Мо coatings [32] deposited from a citrate-pyrophosphate electrolyte, it was found that for the coatings obtained under different electrolysis conditions and having the same chemical composition, the corrosion stability and magnetic parameters are different; it was suggested that the properties of the alloy

**Electrolyte j (mА сm−2) Мо (аt.%) R (Оhm) Rp (Оhm) Еcorr (V) Jcorr (А сm−2)** Citrate-pyrophosphate 10 21.5 5.05 × 102 2.97 × 103 −0.627 3.58 × 10−4

Citrate 30 23.9 4.57 × 103 8.06 × 103 −0.804 2.83 × 10−5

30 17.4 5.71 × 103 1.77 × 104 −0.804 829 × 10−6 50 16.0 7.02 × 102 3.55 × 102 −0.677 6.40 × 10−4

In the study, the corrosion and magnetic properties of coatings with same Mo content of the alloy (21.2 аt.%), deposited from a citrate-pyrophosphate electrolyte under different electrolysis conditions, have been investigated. The corrosion stability of the coatings was studied in

magnetic properties (**Table 6**) of the obtained deposits were determined by means of a vibrat-

The magnetic characteristics of such Alloys are also given. Their calculated values are listed in **Table 6**. The main criteria for evaluating the properties of soft-magnetic materials are low coercive force, low remanent magnetization and high saturation magnetization, as well as the ability to reach saturation magnetization in low intensity fields. It is evident from **Table 6** that the largest saturation magnetization values—927 Gs were obtained at a magnetic field intensity of 3 kOe for the alloys deposited from an electrolyte with a ratio of 5:1. For the coatings deposited from an electrolyte with a ratio of 1:1, no saturation magnetization is observed even at 20 kOe; the maximum value obtained under experimental conditions for alloys deposited at 25° and 50°С was 113 and 290 Gs, respectively. Thus, it can be concluded that the alloy deposited from an electrolyte with the concentration ratio of the metals [Co]/[Mo] = 5/1. We assumed that such a difference in functional properties for the coatings having the same

ing sample magnetometer in fields of up to 20 kOe at room temperature (**Table 5**).

chemical composition may be due to a difference in their phase composition.

**Table 5.** Corrosion properties of alloys having the same chemical composition (21.2 аt.% Мо).

**Deposition electrolyte j (mА сm−2) t (°С) Rр (Оhm) Еcorr (V) Jcorr (А сm−2)** [Co]/[Mo] = 1/1 30 25 2.71 × 103 −0.804 8.44 × 10−5 [Co]/[Mo] = 1/1 40 50 9.82 × 102 −0.808 2.54 × 10−4 [Co]/[Mo] = 5/1 10 50 2.97 × 103 −0.627 3.58 × 10−4

and 7 g L−1 NaCl at рН 6.0 and 24 ± 1°С (**Table 5**). The

SO4

**Table 4.** Dependence of the corrosion parameters of Со-Мо alloys on alloy composition.

110 Electrocatalysts for Fuel Cells and Hydrogen Evolution - Theory to Design

largely depend on its phase composition.

a solution containing 7 g L−1 Na2

Here, j is deposition current density.

To study the phase composition, the electrochemical method of linear stripping voltammetric analysis (LSVA) was used [35]. An advantage of this method, besides simplicity, is the possibility to follow the dissolution dynamics of the alloy. Before the stripping analysis, a 0.5 μM thick layer of Co or Co-Mo alloys were deposited onto the working electrode from a citratepyrophosphate electrolyte with the concentration ratios of the metals [Co]/[Mo] = 1/1 and [Co]/ [Mo] = 5/1 at a current density of 10–100 mА сm−2 and a temperature of 25 and 50°С.

The electrolyte for the anodic dissolution of the obtained alloy deposits must meet the following requirements: it must have a high electrical conductivity, be nonaggressive toward the coating, and not cause spontaneous chemical dissolution. In this electrolyte, an electrochemical side reaction paralleling the anodic dissolution of the deposit under investigation must be ruled out. The use of various acids as working solutions was considered inexpedient since the electrochemical process in such electrolytes is paralleled by the chemical dissolution of the coating under analysis. Alkaline solutions are unsuitable for use as working electrolytes because of passivation processes on the surface of samples under investigation. The optimal solution for the anodic dissolution of coatings under investigation is NaCl solution, which makes it possible to obtain on the current-potential curves clear peaks corresponding to the dissolution potentials of the various phases of the alloy. The stripping analysis of coatings was performed in a 0.5 М NaCl solution at 25°С on a rotating disk electrode at a rotational speed of 774 rpm.

**Figure 15** shows a current-potential curve of the dissolution of freshly deposited cobalt (curve 1) in a 0.5 М NaCl solution. The observed dissolution peaks are traditionally attributed to the complex phase structure of metals and alloys, but their number depends on the electrolyte in which dissolution is performed [35]. The plot of cobalt dissolution current vs. potential exhibits three peaks, which we further use in order to distinguish the peaks of dissolution of the alloy from the peaks of cobalt dissolution. The figure shows plots except the oxygen and chlorine evolution curve. It can be seen that in the case of dissolution of alloys, the magnitude of the peaks and their number are different. For instance, for the alloys deposited from an electrolyte with the same concentration ratio of the metals, the magnitude of peak 1 is the same, but besides it, only one large peak is observed for the alloy obtained at 50°С and 40 mА сm−2, whereas two peaks are observed for the alloy obtained at 25°С and 30 mА сm−2. However, for the alloy deposited from an electrolyte with lower molybdate content, the magnitude of peak 1 is much larger than for other alloys. Based on the potentials of the peaks, the known cathodic quantity of electricity, the phase diagram of the double layer, and stoichiometry, it can be suggested that peaks 1 and 3 relate to cobalt dissolution and peak 2 to the dissolution of a solid solution of the chemical compound СоМо in cobalt.

**Figure 15.** Anodic dissolution curves for pure cobalt (curve 1) and Co-Mo alloys (21.1 at.% Mo) deposited under the following conditions: 2—Co:Mo = 5:1, 50°C, 10 mA cm−2; 3—Co:Mo = 1:1, 25°C, 30 mA cm−2; 4—Co:Mo = 1:1, 50°С, 40 mА сm−2.

Thus, the alloy deposited from an electrolyte containing a small amount of molybdate contains a larger amount of cobalt bound into neither a chemical compound nor a solid solution; this can explain the 200 mV shift of the corrosion potential of this alloy to positive values, i.e., cobalt is a more electropositive metal than molybdenum, as well as the improvement of the magnetic properties of the alloy. The increase in peak 2 indicates an increase in the percentage of the molybdenum-rich phase, which results in the improvement of the corrosion properties of alloys.

Stripping analysis of alloys deposited from an electrolyte with [Co]/[Mo]=1/1 at different current densities is shown in **Figure 16**. It is seen from the figure that for the coatings obtained at lower deposition current densities 10–20 mА сm−2, three dissolution peaks are observed. For the alloys deposited at 30 and 40 mА сm−2, only two dissolution peaks are observed. The magnitude of peak 1 remains unchanged, and it can be assumed to correspond to the amount of cobalt that is directly on the electrode surface, i.e., dissolution of the less corrosion-resistant component than the alloy takes place, and since the electrode geometry does not change, the quantity of electricity for dissolution remains constant too. In the remaining alloy phase at different current densities, different redistribution of cobalt between the solid solution and the free α-phase takes place.

**5. Conclusions**

dissolution peaks.

the properties of exiting nickel cathodes.

the anodic dissolution peaks: 1—the first peak, and 2—the second peak.

Electrolytic alloys of molybdenum and tungsten with iron subgroup metals possess catalytic properties in the hydrogen evolution reaction and can be used as a coating which improves

**Figure 17.** (a) Anodic current-potential curves of the dissolution of Co-Mo alloys deposited from an electrolyte with [Co]/[Mo]=1/1 at 30 mA∙cm−2 and 50°C at different deposition time, s: 1—30, 2—60, 3—120, 4—210. (b) The magnitude of

**Figure 16.** (a) Anodic current-potential curves of the dissolution of Co-Mo alloys deposited from an electrolyte at [Co]/ [Mo] = 1/1 at 50°C at different current densities, mA cm−2: 1—10, 2—20, 3—30, 4—40 and (b) The magnitude of anodic

Electrocatalytic Properties of Molybdenum and Tungsten Alloys in the Hydrogen Evolution Reaction

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113

For each particular electrolyte and particular deposition conditions, the activity of the alloy and its corrosion stability increase with the amount of molybdenum, but the comparison of

The properties of alloys depend not only on their chemical composition but also on their phase composition. The alloy containing the same amount of molybdenum, but fabricated

data obtained by different authors does not give a clear correlation.

under different conditions, has different corrosion and magnetic properties.

To study the alloy formation process, anodic polarization curves have been obtained for Со-Мо alloys deposited from an electrolyte with [Co]/[Mo] = 1/1 under the conditions corresponding to the maximum current efficiency: a current density of 30 mА сm−2 and at temperature of 50°С [36]. The coatings were deposited during 30, 60, 120, and 210 s (**Figure 17**). All current-potential curves of the dissolution of Со-Мо alloys exhibit two peaks. As one would expect, the quantity of electricity for the dissolution of the solid solution increases linearly with deposition time. We failed, however, to determine the order of deposition of the components; using this method, it is impossible to either confirm or refute the hypothesis that cobalt deposits first, which catalyzes later the reduction of molybdenum. Under our experimental conditions, an alloy phase which grows uniformly with increasing deposition time is present in the alloy even within a deposition time of 30 s.

Electrocatalytic Properties of Molybdenum and Tungsten Alloys in the Hydrogen Evolution Reaction http://dx.doi.org/10.5772/intechopen.79058 113

**Figure 16.** (a) Anodic current-potential curves of the dissolution of Co-Mo alloys deposited from an electrolyte at [Co]/ [Mo] = 1/1 at 50°C at different current densities, mA cm−2: 1—10, 2—20, 3—30, 4—40 and (b) The magnitude of anodic dissolution peaks.

**Figure 17.** (a) Anodic current-potential curves of the dissolution of Co-Mo alloys deposited from an electrolyte with [Co]/[Mo]=1/1 at 30 mA∙cm−2 and 50°C at different deposition time, s: 1—30, 2—60, 3—120, 4—210. (b) The magnitude of the anodic dissolution peaks: 1—the first peak, and 2—the second peak.

### **5. Conclusions**

Thus, the alloy deposited from an electrolyte containing a small amount of molybdate contains a larger amount of cobalt bound into neither a chemical compound nor a solid solution; this can explain the 200 mV shift of the corrosion potential of this alloy to positive values, i.e., cobalt is a more electropositive metal than molybdenum, as well as the improvement of the magnetic properties of the alloy. The increase in peak 2 indicates an increase in the percentage of the molybdenum-rich phase, which results in the improvement of the corrosion properties of alloys. Stripping analysis of alloys deposited from an electrolyte with [Co]/[Mo]=1/1 at different current densities is shown in **Figure 16**. It is seen from the figure that for the coatings obtained at lower deposition current densities 10–20 mА сm−2, three dissolution peaks are observed. For the alloys deposited at 30 and 40 mА сm−2, only two dissolution peaks are observed. The magnitude of peak 1 remains unchanged, and it can be assumed to correspond to the amount of cobalt that is directly on the electrode surface, i.e., dissolution of the less corrosion-resistant component than the alloy takes place, and since the electrode geometry does not change, the quantity of electricity for dissolution remains constant too. In the remaining alloy phase at different current densities, different redistribution of cobalt between the solid solution and the free α-phase takes place. To study the alloy formation process, anodic polarization curves have been obtained for Со-Мо alloys deposited from an electrolyte with [Co]/[Mo] = 1/1 under the conditions corresponding to the maximum current efficiency: a current density of 30 mА сm−2 and at temperature of 50°С [36]. The coatings were deposited during 30, 60, 120, and 210 s (**Figure 17**). All current-potential curves of the dissolution of Со-Мо alloys exhibit two peaks. As one would expect, the quantity of electricity for the dissolution of the solid solution increases linearly with deposition time. We failed, however, to determine the order of deposition of the components; using this method, it is impossible to either confirm or refute the hypothesis that cobalt deposits first, which catalyzes later the reduction of molybdenum. Under our experimental conditions, an alloy phase which grows uniformly with increasing deposition time is present

**Figure 15.** Anodic dissolution curves for pure cobalt (curve 1) and Co-Mo alloys (21.1 at.% Mo) deposited under the following conditions: 2—Co:Mo = 5:1, 50°C, 10 mA cm−2; 3—Co:Mo = 1:1, 25°C, 30 mA cm−2; 4—Co:Mo = 1:1, 50°С, 40

in the alloy even within a deposition time of 30 s.

112 Electrocatalysts for Fuel Cells and Hydrogen Evolution - Theory to Design

mА сm−2.

Electrolytic alloys of molybdenum and tungsten with iron subgroup metals possess catalytic properties in the hydrogen evolution reaction and can be used as a coating which improves the properties of exiting nickel cathodes.

For each particular electrolyte and particular deposition conditions, the activity of the alloy and its corrosion stability increase with the amount of molybdenum, but the comparison of data obtained by different authors does not give a clear correlation.

The properties of alloys depend not only on their chemical composition but also on their phase composition. The alloy containing the same amount of molybdenum, but fabricated under different conditions, has different corrosion and magnetic properties.

The amorphous and nanocrystalline structure of electrolytic alloys makes hydrogen spillover possible, which greatly accelerates the hydrogen reduction process in alkaline electrolytes.

[9] Коrovin N. On the connection between the electrocatalytic activity of metals in the hydrogen evolution reaction with their properties. Elektrokhimiya. 1991;**27**(12):1629-1633 [10] Navarro-Flores E, Chong Z, Omanovic S. Characterization of Ni, NiMo, NiW and NiFe electroactive coatings as electrocatalysts for hydrogen evolution in an acidic medium. Journal of Molecular Catalysis A: Chemical. 2005;**226**:179-197. DOI: 10.1016/j.molcata.

Electrocatalytic Properties of Molybdenum and Tungsten Alloys in the Hydrogen Evolution Reaction

http://dx.doi.org/10.5772/intechopen.79058

115

[11] Highfield JG, Claude E, Oguro K. Electrocatalytic synergism in Ni/Mo cathodes for hydrogen evolution in acid medium: A new model. Electrochimica Acta. 1999;**44**:2805-2814.

[12] Martinez S, Metikoš-Huković M, Valek L. Electrocatalytic properties of electrodeposited Ni–15Mo cathodes for the HER in acid solutions: Synergistic electronic effect. Journal of Molecular Catalysis A: Chemical. 2006;**245**:114-121. DOI: 10.1016/j.molcata.2005.09.040

[13] Ved M, Sakhnenko N, Bairachnaya T, Tkachenko N. Structure and properties of electro-

[14] Subramania A, Sathiya Priya AR, Muralidharan VS. Electrocatalytic cobalt–molybdenum alloy deposits. International Journal of Hydrogen Energy. 2007;**32**:2843-2847. DOI:

[15] Arul Raj I. On the catalytic activity of Ni-Mo-Fe composite surface coatings for the hydrogen cathodes in the industrial electrochemical production of hydrogen. Applied

[16] Krstajic NV, Jovic VD, Gajic-Krstajic L, Jovic BM, Antozzi AL, Martelli GN. Electrodeposition of Ni–Mo alloy coatings and their characterization as cathodes for hydrogen evolution in sodium hydroxide solution. International Journal of Hydrogen Energy.

[17] Kuznetsov VV, Kalinkina AA, Pshenichkina TV, Balabaev VV. Electrocatalytic properties of cobalt-molybdenum alloy deposits in the hydrogen evolution reaction. Russian

Journal of Electrochemistry. 2008;**44**:1350-1358. DOI: 10.1134/S1023193508120070

[18] Rosanov VV, Krylov OV. Spillover of hydrogen in heterogeneous catalysis. Uspekhi

[19] Delmon B. A new hypothesis explaining synergy between two phases in heterogeneous catalysis the case of hydrodesulfurization catalysts. Bulletin des Societes Chimiques

[20] Santos Diogo MF, Sequeira César AC, Figueiredo José L. Hydrogen production by alkaline water electrolysis. Quimica Nova. 2013;**36**(8):1176-1193. DOI: 10.1590/S0100-

[21] Manazoglu M, Hapcı G, Orhan G. Effect of electrolysis parameters of Ni–Mo alloy on the electrocatalytic activity for hydrogen evaluation and their stability in alkali medium. Journal of Applied Electrochemistry. 2016;**46**:191-204. DOI: 10.1007/s10800-015-0908-y

lytic cobalt-tungsten alloy coatings. Functional Materials. 2008;**15**:613-617

Surface Science. 1992;**59**:245-252. DOI: 10.1016/0169-4332(92)90124-G

2008;**33**:3676-3687. DOI: 10.1016/j.ijhydene.2008.04.039

2004.10.029

DOI: 10.1016/S0013-4686(98)00403-4

10.1016/j.ijhydene.2006.12.027

Khimii. 1997;**66**(2):117-130

Belges. 1979;**88**:979-987

40422013000800017

Electrolytic coatings of refractory metals alloys have a wide range of physicochemical properties. Controlling the electrolysis modes allows precipitating and accurately controlling the chemical and phase composition of the coatings, and hence producing corrosion-resistant materials for soft magnetic materials, electrocatalysts, and wear-resistant coatings.

### **Author details**

Valeriy Kublanovsky\* and Yuliya Yapontseva

\*Address all correspondence to<EMAIL_ADDRESS>
V. I. Vernadskii Institute of General and Inorganic Chemistry of the Ukrainian NAS, Kyiv, Ukraine

### **References**

[9] Коrovin N. On the connection between the electrocatalytic activity of metals in the hydrogen evolution reaction with their properties. Elektrokhimiya. 1991;**27**(12):1629-1633

The amorphous and nanocrystalline structure of electrolytic alloys makes hydrogen spillover possible, which greatly accelerates the hydrogen reduction process in alkaline electrolytes.