referring to fig1 , the feed ( 1 ) used can be ore or an ore concentrate obtained from an appropriate mineral processing technology . in examples presented below , on the feed used is from a massive chromite layer obtained from the menarik deposit ( james bay , quebec ). the average mineralogy of 29 massive chromite layers of the menarik complex is : chromite 45 %, chlorite 32 %, serpentine 13 %, magnetite 3 %, talc 1 %, hornblende 4 %, and traces of sulfides . the sample was hand picked from the chromite mineralized zone cr - 3 and subsequently ground to 125 μm . the chemical composition of this starting material , identified as feed ( 1 ) in fig1 , is reported in table 2 as starting ore for examples 1 and 2 , and in table 3 as starting ore for examples 3 to 6 . nacl ( 3 ) was added to the ground ore as a solution in order to obtain a concentration ( w / w ) of salt in the feed varying between 0 . 8 % and 15 % according to examples 1 to 6 below . the nacl salt addition provides one of the components for the formation of an eutectic point which the fecl 3 produces via the carbochlorination of the chromite feed ( reactions are reported under the carbochlorination heading below ). the phase diagram for the system fecl 3 — nacl is illustrated at fig2 . for temperatures over the first eutectic temperature , 157 ° c ., liquid nafecl 4 is formed from the reaction of fecl 3 with nacl . in examples presented below , the chlorination temperature varies from 250 ° to 720 ° c . according to the phase diagram of fig2 , nafecl 4 is present as a liquid phase in the feed at all chlorination temperatures used . in the present invention , the salt addition is performed in order to produce a thin film of a melt around each grain of the feed . this interstitial melt contains the chlorination agent in a chemical form such as nafecl 4 . the thin film acts as a chlorination solvent increasing chlorine diffusion in the chromite . the chlorine gaseous atmosphere enclosed in the reactor regenerates the effective chlorination agent contained in the melt . it is understood from the person of ordinary skill in the art that other types of salts such as kcl and mgcl 2 can be used to produce a catalytic system for the carbochlorination of chromites . the drying step ensures a complete removal of water resulting from the salt addition and can be carried out at different temperatures and time periods . in examples presented below , the mixture was dried at 180 ° c . for 30 minutes . after cooling , the charge was transferred in the chlorination reactor and pre - heated at the selected reaction temperature . feo . cr 2 o 3 + 1 . 5cl 2 ( g )+ co ( g ) cr 2 o 3 + fecl 3 ( g )+ co 2 ( g ) 4 . the δg ° t versus temperature of this reaction was calculated using the hsc ™ software of outokumpu . they are presented at fig3 . for the rangef of temperatures considered , the δg ° o t values were inferior to − 150 kjoules . this demonstrates the thermodynamic feasibility of the reaction . according to reaction 4 , the iron contained in the chromite reacts with cl 2 to form fecl 3 . at the temperature range described examples presented below , 250 ° to 673 ° c ., fecl 3 is in a vapour state . because of the continuous flow of gas passing through the reactor , fecl 3 is carried outside the reactor , where it is condensed . an acceptor such as co ( g ) for the oxygen liberated during the chlorination reaction may be added to maintain reducing conditions . the addition of co ( g ) limits the probability that the reaction 2fecl 3 + 3 / 2o 2 = fe 2 o 3 + 3cl 2 will occur . thereby , no detectable precipitation of unwanted solid hematite takes place in the reactor . another significant reaction occurring according to the process of the present invention is the formation of ferrous chloride fecl 2 during the carbochlorination phase . ferrous chloride ( fecl 2 ) having a high melting point of 670 ° c ., hence a temperature higher than that used during the carbochlorination according to certain embodiments of the present invention , a rapid chlorination of fecl 2 into ferric chloride ( fecl 3 ) according to the reaction 2fecl 2 + cl 2 2fecl 3 ( g ) may be desirable in these specific embodiments in order to avoid the production of a diffusion barrier by the formed solid ferrous chloride . this barrier may decrease the chlorine access to the reaction sites . rhee and shon ( 1990 , metallurgical transactions b , 21b , pp . 321 - 330 ) reported data on the carbochlorination of ilmenite ( feo . tio 2 ), a product presenting similarities to chromites when chlorinated . they showed that the kinetics follow a pore - blocking rate law . zhao , tian and duan ( 1990 , metallurgical transactions b , 21b , 131 - 133 ) studied the equilibrium between ferrous and ferric chloride in molten chloride salts . they concluded on the catalytic effect of the combination of salt and iron chloride and also on the volatilization of iron from the salt melt . their data indicated that volatilization of iron as fecl 3 is maximized when the nacl content is high . none of these conditions were tested before on chromites . hence , in the present invention , carbochlorination is performed with a salt such as nacl , kcl and mgcl 2 to produce a catalytic melt when nacl combines with fecl 2 and / or fecl 3 so as to increase the volatilization ( the removal ) of iron as gaseous fecl 3 from the carbochlorination reactor . when the carbochlorination temperature was reached in the chlorination reactor ( 5 ) a mixture of cl 2 and co and , in specific embodiments , n 2 ( not shown ) was introduced in the reactor so as to induce carbochlorination . after a few minutes , fecl 3 ( g ) ( 5 ) was expelled from the reactor . according to specific embodiments described examples below , the temperature was varied from 250 ° to 720 ° c . however because of thermodynamics rules , it is expected that this temperature may be increased at least up to 750 ° c . without loosing the selectivity of the chlorination towards iron . in specific embodiments , chlorine and carbon monoxide were used on a 1 / 1 basis . the flow rate was maintained at 1 ml per second . in other embodiments , a mixture of cl 2 , co , and n 2 was employed , n 2 acting as a carrier gas . n 2 is not believe to play a role in any reaction involved in the method and may accordingly be dispensed of . in cases where cl 2 , co , and n 2 were used , the flow rates of the different gases were varied as well as the weight % of salt additives . results ( not shown ) have shown that the optimal cl 2 / co flow rate ratio is between about 0 . 5 and about 1 . 5 . interesting results are nevertheless obtained outside this range but the cr / fe obtained progressively decreases with ratios below 0 . 5 or above 1 . 5 ( results not shown ). the chlorination reactions were conducted in a simple horizontal static furnace . usually , at industrial scale , chlorination is realized in fluidized bed reactors constructed of acid resistant bricks enclosed in a metal shell . since the salt addition results in the formation of a thin liquid film layer around the chromite grains , which increases their adherence properties , it may be desirable to avoid fluidized reactor in order to avoid problems associated with grains agglomeration and bed sedimentation . alternatives to fluidized bed reactor include a vertical static reactor and a horizontal rotating reactor . other embodiments of the present invention may include the use of solid reducing agents like coal or coke instead of co which may be onerous for industrial scale methods . when coal and coke are used , they react with oxygen to form co so that the end result is similar to that obtained when co is directly introduced in the chlorination reactor . pelletizing - sintering procedures , similar to the ones employed in the ferrochromium industry , can be performed before the chlorination step . after the chlorination reaction , the solid upgraded chromites minerals ( 6 ) contained in the reactor were dumped . depending on the duration of the reaction , the gas flow rate , the salt additives , the cl 2 / co ratio , the chlorinated solid residue showed an increase in its chrome to iron ratios . the ratios varied from 1 . 5 in the starting ore before chlorination up to 17 after chlorination . these results are presented in tables 2 - 5 below . gaseous fecl 3 ( 10 ) exits continuously the reactor during the reaction and the abrupt temperature drop outside the reactor causes its fast condensation in the top section of the condenser . the condenser is placed at an adequate distance from the furnace so as to keep its temperature below 50 ° c . so as to ensure fecl 3 &# 39 ; s condensation . fecl 3 is highly soluble in water . a small volume of water is added to the condenser apparatus to wash the solid fecl 3 . the fecl 3 rich aqueous solution accumulates at the base of the condenser and is directed into a reservoir for subsequent neutralization . the other gases leaving the reactor are essentially cl 2 , co , co 2 ( 12 ) and n 2 ( not shown ). these gases are apparently not affected by the presence of the condenser ( 8 ) and flow through it without experiencing any detectable change in their compositions or states and exit the condenser . cl 2 , co , co 2 and n 2 exiting the chlorination reactor ( 5 ) are routed toward a washing tower ( 14 ). scraps of metallic iron ( 16 ) in the millimetre range are placed in the tower ( 14 ) and sprayed with a small quantity of water ( 18 ) in order to keep wet the iron metallic surfaces . this arrangement favors the reaction fe ( s )+ 3 / 2cl 2 fecl 3 ( aq ) which consume the unreacted cl 2 . after the reaction , fecl 3 is present as a solute ( 20 ) in h 2 o . co and co 2 ( 22 ) percolate up and exit the washing tower near the top . co is burned as co 2 ( 24 ) in an after burner ( 26 ) unit . if necessary , by environmental regulations , the scrubbing of co 2 can be achieved by an existing complementary technology ( not shown ). the aqueous fecl 3 solution flows out at the base of the washing tower to be routed toward the neutralization reservoir . the aqueous fecl 3 solutions ( 10 ) and ( 20 ) coming from the condenser ( 8 ) and the washing tower are pumped in a neutralization reservoir ( 28 ). a solution of naoh ( not shown ) is added to the reservoir . the ferric chloride reacts with naoh to produce fe ( oh ) 3 ( 30 ) according to the reaction : after completion of the reaction , the solid amorphous iron oxides are isolated from the liquid phase by an appropriate solid - liquid separation such as centrifugation or press filtration ( 31 ). the filtration cake is discharged to the tailings . the aqueous nacl solution ( 32 ) is directed to an electrolysis cell ( 34 ). the nacl solution ( 32 ), obtained from the neutralization step of the process , is electrolyzed by a chlor - alkali membrane cell process . the reaction involved is : the gaseous cl 2 and aqueous naoh generated by the reaction are recycled in the process . the cl 2 is returned ( 36 ) to the carbochlorination reactor ( 5 ) and the aqueous naoh is directed ( 31 ) in the neutralization reservoir ( 28 ). the h 2 ( g ) produced ( not shown ) by this reaction can be employed as the main energy source or an additional energy source for the carbochlorination reactor ( 5 ). external supplies of nacl can be used if needed . any means for routing , transporting and transferring solid , gas , liquid and pulp are within the scope of these inventions . the present invention is described in further details by the following non - limiting examples . the implementation and results of examples provided herein are summarized in tables 2 - 5 . table 2 presents results according to the first set of experiments for which the cl 2 / co ratio flow rates , reaction time , and type and quantity of salt addition were kept constant during the experiments , while the temperature was varied . examples 1 and 2 are derived from this first set of experiences . tables 3 and 4 contain data for the second set of embodiments for which , temperature , reaction time and quantity of salt addition were varied . this second set of experiments is represented in examples 3 to 6 . the carbochlorination experiments where carried out in a 65 cm long horizontal cylindrical furnace equipped with a type k pyrometer linked to a thermostat controller . usually , a 10 grams sample was placed in a ceramic beaker and inserted in a silica fused tube . the beaker - tube assembly was then introduced in the furnace . the major and trace elements were analyzed by inductively couple plasma atomic emission spectroscopy , icp - aes , after a fusion procedure specifically applicable to chromite . sulfur was determined with a cns analyzer . this example comprises a set of 4 experiments . the results are presented in table 2 . this example demonstrates the selectivity of the iron removal by carbochlorination versus chromium according to the method of the present invention . the other major elements are reported in table 2 for indicative purposes only . the range of temperature tested varied from 250 to 550 ° c . the chlorinated sample were mixed with a nacl brine and dried at 180 ° c . for 30 minutes . the salt content of the chlorinated samples was 5 % ( w / w ). a 10 g sample of chromite ore was placed in a 10 ml porcelain beaker . the beaker was positioned in the center of 60 cm in length silica tube , with an internal diameter of 6 cm . the assembly beaker - silica tube was placed in the furnace and the temperature was raised at the chosen carbochlorination temperature . when the temperature was reached and stable , a cl 2 , co gas mixture was introduced in the furnace on a one to one ratio basis . the carbochlorination step was conducted for 60 minutes . a red brown chlorine vapor formed five minutes after the beginning of introducing the gases in the furnace . this vapor was expelled outside the reactor through the gases flow , where it condensed on the inside wall of the silica tube . at the end of the experiment , the furnace - heating device and the gases flow were stopped . after a cooling period , the solid residue left in the porcelain beaker was analyzed for major and selected trace elements . the results presented in table 2 show that the concentration of fe 2 o 3t increased and that of cr 2 o 3 decreased in tests - 01 - 04 . these results clearly show the selective removal of iron . the original content of iron decreased gradually with corresponding increases of the carbochlorination temperature from 25 . 31 % in the starting ore to 17 . 12 % in the test - 04 run at 550 ° c . the chromium content of the samples tested increased from 45 . 33 % in the starting ore to 52 . 07 % in the test - 04 sample performed at 550 ° c . this chrome enrichment was correlated with the weights losses of the samples and therefore reflected the removal of iron from the samples . as expected , the chrome to iron ratios show a positive correlation with the temperature ( fig4 ). the chrome to iron ratio increases from 1 . 76 in the starting ore up to 2 . 98 in the test - 04 sample . the red brown condensate formed on the inside wall of the silica tube ( in experiment described in example 1 ) was washed out from the tube with water , in which this compound dissolved readily . this solution was analyzed by icp - aes for major elements and by uv spectroscopy for the oxidation state of iron . analyzis of the solution established the presence of iron as the only major element . other elements were present at the trace level . iron oxidation state was determined as fe + 3 by uv . these observations further demonstrated that iron was removed as gaseous fecl 3 during the carbochlorination of the chromite ore . effect of the salt addition on the selective removal of iron versus chromium the effect of the nacl salt addition on the carbochlorination was tested by adding incremental quantity of nacl to samples t - 2 - 1 to t - 2 - 5 . the experimental conditions for these five samples are summarized in table 3 . carbochlorination temperature was set at 600 ° c ., the reaction time at 2 hours , and the quantity of nacl salt addition varied from 0 to 15 . 0 % ( w / w ). results presented in table 3 show a direct increase in the chrome to iron ratio in relation with the quantity of salt added to the feed . in sample t - 2 - 1 , with no salt addition , the chrome to iron ratio reached a value of 3 . 16 after the chlorination step , an increase of 1 . 75 compared to the original ore . in sample t - 2 - 5 to which was added 15 % nacl ( w / w ), the chrome to iron ratio was 4 . 52 at the end of the chlorination experiment . this corresponds to a 47 % increase in the cr / fe when compared to sample t - 2 - 1 . this strong increase of the carbochlorination efficiency is attributed to the catalyst effect of the mixture nacl and fecl 3 as explained before . effect of increasing the reaction time on the selective removal of iron versus chromium the effect of increasing the reaction time on the selective removal of iron was tested by 0 . 5 hour time increments . total reaction time varied from 0 . 5 hour to 2 . 0 hours . samples were tested as follows , 0 . 5 hour for t - 2 - 8 , 1 . 0 hour for t - 2 - 7 , 1 . 5 hours for t - 2 - 6 and 2 . 0 hours for t - 2 - 3 . experimental conditions used for these samples are reported in table 3 . the chrome to iron ratios increased from 1 . 88 for the starting ore , to 3 . 63 for t - 2 - 3 after a reaction time of 2 hours . the chrome to iron ratios increase is positively correlated to the reaction time ( fig5 ). effect of using a temperature higher than the melting point of fecl 2 on the selective removal of iron versus chromium the temperature of 673 ° c . was selected as slightly superior to the melting point of fecl 2 ( 670 ° c .). the total reaction time varied from 0 . 5 hour to 2 . 0 hours with a time increment of a half hour for each of samples were t - 2 - 9 to t - 2 - 12 as in example 4 . the experimental conditions and the results for these experiments are reported in table 3 . it is postulated that fecl 2 is formed at some point during the chlorination and subsequently transformed in fecl 3 according to the reaction fecl 2 + 1 / 2cl 2 fecl 3 ( g ). at temperature below the melting point of fecl 2 , the presence of this compound as a solid can act as a blocking agent between the chlorination agent and the chromites reaction sites . when melted , fecl 2 can actively promote fe extraction in the chlorination catalytic system earlier described herein . the results presented in table 2 indicated that bringing the chlorination temperature to 673 ° c . has a very decisive impact on the selective removal of iron versus chromium , with the production of a chrome to iron ratio up to 10 for a two hours chlorination time . the relation between the chrome to iron ratio versus chlorination time is presented in fig6 . a comparison between results for t = 550 ° c . and t = 600 ° c . with results for t = 673 ° c . is also presented in fig6 . carbochlorinations conducted at 673 ° c . showed a significant increase in the chrome to iron ratios when compared to those conducted at lower temperatures . moreover , the chrome to iron ratios between experiments conducted at 550 ° c . and 600 ° c . show a relatively small increase , namely from 2 . 98 to 3 . 27 for a temperature difference of 50 ° c . while that obtained for experiments conducted at 673 ° c . is much larger for a temperature difference of 73 ° c ., namely 2 . 98 to 6 . 00 . without being limited to such hypothesis , it is proposed that the important increase in the chrome to iron ratios for the experiments conducted at 673 ° c . are attributed to the melting of fecl 2 and volatilization of fecl 3 . this melting allowed fecl 2 to play a role in the catalytic system comprising nacl , fecl 2 and fecl 3 . effect of the carbochlorination for selectively removing iron without altering the major chemical components of the chromite in the second set of experiments , the major elements concentrations and the weight losses were measured and presented at tables 3 and 4 . when correcting for the weight losses due to the losses of iron ( under the heading “ weight losses ” in table 3 ), no apparent removal of other major elements was noticed by comparison to the starting composition . although , the cr 2 o 3 contents of samples t - 24 and t - 2 - 5 show small losses , they are attributed to a dilution effect caused by nacl . in these two samples , the concentration of salt was especially high , 10 and 15 %, respectively . mno and cao also showed slight decreases in their concentrations . these two components are however generally present at concentrations lower than 1 % in chromites and their partial removal is not detrimental to the present invention . chromium to iron ratio increase versus temperature and duration of the reaction experiments were conducted at 720 ° c . to further investigate the chromium to iron ratio increase at higher temperatures . the experimental conditions were the following : nacl addition 5 %, cl 2 and co flow rate = 220 ml / min , n 2 flow rate = 110 ml / min , the reaction time was varied from 0 to 2 hours . the results are presented in table 5 above and fig7 . an increase of the time of reaction correlated with an increase of chromium to iron ratios . after two yours , the cr / fe reaches 16 . 9 for a starting value of 1 . 8 in the feed . the cr 2 o 3 content of the material showed no sign of chromium removal during the experiment and increased from 4 to 55 %, as shown in above table 5 . although the invention has been described above with respect to a few representative examples and drawings , it will be evident in the person skilled in the art that it may be modified and refined in various ways . it is therefore wished to have it understood that the present invention should not be limited in scope , except by the terms of the following claims :