the prior art diaphragm cell shown in fig1 for water electrolysis consists of the cell 1 , the anode electrode 2 and the cathode electrode 3 connected to the dc power source 7 . the anode and cathode electrodes are separated by a diaphragm 4 . in operation , the hydroxyl ions are converted to oxygen 10 and water . the excess of hydrogen ions is the driving force for the hydrogen ions to diffuse through the diaphragm 4 through the catholyte 5 to the cathode electrode 3 where the hydrogen ions are reduced to hydrogen gas 9 . the electronic circuit is from the dc power source to the cathode electrode through the catholyte through the diaphragm through the anolyte to the anode electrode and to the dc power source . the ionic circuit is normally from the anode through the anolyte through the diaphragm through the catholyte to the cathode electrode . this slow diffusion process can be by - passed by mechanically transferring the anolyte to the cathode cell . the reduced catholyte is returned 8 a to the anode cell . water 8 is added to the anode cell to replenish the water used in the reaction . fig2 : principle of the electrolytic cell of the present invention in water electrolysis the electrolytic cell consists of the anode cell 11 and the cathode cell 12 . the diaphragm is replaced by a solution electrode 17 adjacent to the anode electrode 13 and solution electrode 18 adjacent to the cathode electrode 14 and externally connected by a conductor 19 . in operation and using a potassium hydroxide solution 21 , electrons are removed from the anolyte 15 in contact with the anode electrode 13 resulting in the following reaction : with the production of oxygen . the anolyte 20 containing the hydrogen ion is transferred to the cathode cell where electrons are added to the catholyte resulting in the following reaction : the electronic circuit is from the dc power source 22 to the cathode electrode 14 through the catholyte 16 to the solution electrode 18 through the external conductor 19 to the solution electrode 17 at the anode cell 11 to through the anolyte 15 to the anode electrode 13 then to the dc power source 22 . the ionic circuit consists of transferring the anolyte 15 via line 20 to the cathode cell 12 and returning the reduced catholyte 16 via line 21 to the anode cell 11 . water 25 is added to the anode cell 11 to make up for the water consumed in the reaction . fig3 is a schematic presentation of a commercial plant using diaphragm - less electrolytic cell to produce hydrogen from water using either an acid electrolyte or a basic electrolyte . the pressurized anode cell 31 containing the anode electrode 33 and the solution electrode 37 receives reduced catholyte 64 continuously and discharges the anolyte 39 continuously to a turbine pump 40 . electrons are continuously removed from the anolyte by the anode electrode 33 connected to the dc power source 53 . the following reactions occur : the anolyte containing oxygen and the hydrogen ion is fed into a hydrocyclone 41 or centrifugal separator to remove as much oxygen in the electrolyte to the overflow 42 . the separator 44 separates the liquid from the hydrocyclone overflow to produce the main oxygen stream 45 and electrolyte 46 that joins the hydrocyclone underflow 43 and directed into the cathode pump box 47 . the oxygen may either be released to the atmosphere 48 to maintain the oxygen balance or collected and used as oxidant in fuel cell installations . the anolyte 49 with out oxygen and containing the hydrogen ions is transferred under pressure by turbine pump 51 where the following reactions occur : the turbine pumps 31 and 51 are used to reduce power consumption in the commercial process . the catholyte 50 containing the hydrogen gas is passed through the turbine pump 51 to the hydrocyclone 55 where the hydrogen gas is separated into the overflow 56 that is directed to separator 58 . the catholyte liquids 57 and 60 are collected into the anode pump box 61 before being pumped by turbine pump 31 to the anode cell 31 . water 63 is added to the anode pump box 61 to replenish the water used in the reaction . in either acid or basic electrolytes , appropriate metal or compound ions may be used to further reduce the voltage of the cell . the example given in fig3 is the ferrous - ferric ion and the reaction at the anode with an acid electrolyte is projected as follows : at the anode with acid electrolyte : 2fe +++ + h 2 o → 2fe ++ + ½o 2 + 2h + the ferrous ion is oxidized to ferric : 2fe ++ − 2e − → 2fe +++ the objective of this commercial process is to produce the quantities of hydrogen shown on table 1 . fig4 is an embodiment of the diaphragm - less electrolytic cell of the present invention in a unipolar mode where there are separate anode and cathode circuits . there is a separate electrolyte passing the anode cell and a separate electrolyte passing the cathode cell . these electrolytes are connected electrically to the dc power source and through the solution electrodes . electrons are removed from the anode electrolyte while electrons are added to the electrolyte passing the cathode cell . water 73 is fed into the anode cell 70 containing the anode electrode 71 and the solution electrode 78 . the oxidized electrolyte is discharged from the anode cell 70 as anolyte 75 . gas 74 may be produced . electrons are removed from the anode electrolyte by the dc power source 76 and delivered to the cathode electrode 81 at the cathode cell 80 . water 83 is fed into the cathode cell 80 and is discharged as catholyte 84 after being reduced . there hydrogen gas 85 is generated . the electronic circuit is from the dc power source 76 to the cathode electrode 81 through the catholyte 82 to the solution electrode 79 to the external conductor 77 to the solution electrode 78 through the anolyte 72 to the anode electrode 71 and to the dc power source 76 . the concept shown on fig5 to reduce energy consumption in water electrolysis was developed from tests carried out in our laboratory . the concept has the objective of reducing the energy consumption in the electrolysis of water by reducing the voltage required and utilizing the energy imparted to the electrolytes in the primary cells to produce more hydrogen . the alkaline circuit consists of a storage tank 90 where electrolyte 92 and water 91 are withdrawn by pump 93 and fed to primary anode cell 94 that is connected to dc power source 95 . the primary anode cells solution electrodes are connected by external conductor 97 to the primary cathode solution electrodes . oxygen is produced at a theoretical voltage of 0 . 401 volts . the oxidized electrolyte 98 rich in hydrogen ion is passed to an oxygen collector 99 before passing through the secondary cathode cells 100 where the oxidized electrolyte is reduced . theoretically , a voltage of 0 . 828 is required to produce hydrogen . several secondary cathode cells may be connected in series to achieve the required voltage to produce hydrogen . the reduced electrolyte 102 is passed to hydrogen collector 103 before the electrolyte 96 is returned to the alkaline storage tank 90 . the acid circuit consists of a storage tank 104 where electrolyte 105 and water 91 are withdrawn by pump 106 and fed to primary cathode cells 107 that is connected to dc power source 95 . the primary cathode cells solution electrodes are connected by external conductor 97 to the primary anode solution electrodes . hydrogen is produced at a theoretical voltage of 0 . 000 volts . the reduced electrolyte 108 rich in hydroxyl ion is passed to a hydrogen collector 109 before passing through the secondary anode cells 110 where the reduced electrolyte is oxidized . theoretically , a voltage of 1 . 229 volts is required to produce oxygen . several secondary anode cells may be connected in series to achieve the required voltage to produce oxygen . the oxidized electrolyte 111 is passed to an oxygen collector 112 before the electrolyte 113 is returned to the acid storage tank 104 . the secondary cathode cell solution electrodes are connected by external conductor 101 to the secondary anode solution electrodes and the secondary cathodes are connected by external conductor 101 a to the secondary anodes . fig6 is a diagram of a commercial process to produce hydrogen by unipolar activation using potassium hydroxide electrolyte in one circuit and phosphoric acid in the other circuit . the potassium hydroxide circuit consists of a storage tank 145 provided with heat 152 and make up water 147 controlled by a float valve . electrolyte 148 is withdrawn by pump 150 and the electrolyte 148 is delivered to the primary anode cells 120 containing the anode electrodes 121 connected to the dc power source 125 and the solution electrodes 122 connected to the external conductor 129 . oxygen 123 is produced by the reaction : the oxidized electrolyte 124 exiting the primary anode cell 120 is rich in potassium ions and is passed to the secondary cathode cells 132 containing the secondary cathode electrodes 133 connected by external conductor 136 to the secondary anode electrodes 140 and containing the secondary cathode solution electrodes 134 connected by external conductor 135 to the secondary anode solution electrodes 137 . the theoretical voltage to produce hydrogen is 0 . 828 volts from the following reaction : it may require several secondary cathode cells connected in series to generate the hydrogen . the electrolyte 143 is returned to the storage tank 145 . the phosphoric acid circuit consists of a storage tank 146 provided with heat 152 and make up water 147 controlled by a float valve . electrolyte 149 is withdrawn by pump 151 and the electrolyte 149 is delivered to the primary cathode cells 126 containing the cathode electrodes 127 connected to the dc power source 125 and the solution electrodes 128 connected to the external conductor 129 . hydrogen 130 is produced by the reaction : the reduced electrolyte 131 exiting the primary cathode cell 126 is rich in phosphoric ions and is passed to the secondary anode cells 139 containing the secondary anode electrodes 140 connected by external conductor 136 to the secondary cathode electrodes 133 and containing the secondary anode solution electrodes 137 connected by external conductor 135 to the secondary cathode solution electrodes 134 . the theoretical voltage to produce oxygen is 1 . 229 volts from the following reaction : 2po − 4 + 6h + + 6oh − − 6e − → h 3 po 4 + 3h 2 o + 3 / 2o 2 it may require several secondary anode cells connected in series to generate the oxygen . the electrolyte 144 is returned to the storage tank 146 .