US3766026A - Electrolytic process for the recovery of nickel, cobalt and iron from their sulfides - Google Patents

Electrolytic process for the recovery of nickel, cobalt and iron from their sulfides Download PDF

Info

Publication number
US3766026A
US3766026A US00251940A US3766026DA US3766026A US 3766026 A US3766026 A US 3766026A US 00251940 A US00251940 A US 00251940A US 3766026D A US3766026D A US 3766026DA US 3766026 A US3766026 A US 3766026A
Authority
US
United States
Prior art keywords
metal
recovered
nickel
electrolyte
iron
Prior art date
Legal status (The legal status is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the status listed.)
Expired - Lifetime
Application number
US00251940A
Inventor
P Kruesi
Current Assignee (The listed assignees may be inaccurate. Google has not performed a legal analysis and makes no representation or warranty as to the accuracy of the list.)
Cyprus Mines Corp
Original Assignee
Cyprus Metallurgical Processes Corp
Priority date (The priority date is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the date listed.)
Filing date
Publication date
Application filed by Cyprus Metallurgical Processes Corp filed Critical Cyprus Metallurgical Processes Corp
Application granted granted Critical
Publication of US3766026A publication Critical patent/US3766026A/en
Assigned to CYPRUS MINES CORPORATION; A CORP OF DE reassignment CYPRUS MINES CORPORATION; A CORP OF DE ASSIGNMENT OF ASSIGNORS INTEREST. Assignors: CYPRUS METALLURGICAL PROCESSES CORPORATION
Anticipated expiration legal-status Critical
Expired - Lifetime legal-status Critical Current

Links

Classifications

    • CCHEMISTRY; METALLURGY
    • C25ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25CPROCESSES FOR THE ELECTROLYTIC PRODUCTION, RECOVERY OR REFINING OF METALS; APPARATUS THEREFOR
    • C25C1/00Electrolytic production, recovery or refining of metals by electrolysis of solutions
    • C25C1/06Electrolytic production, recovery or refining of metals by electrolysis of solutions or iron group metals, refractory metals or manganese

Definitions

  • ABSTRACT A pollution-free process for the electrolytic dissolution of sulfide concentrates of the metals of Group VIII of the Periodic Table in aqueous acidic media with the formation of metal ions and elemental sulfur followed by recovery of the metal ion from solution in the electrolyte media, the process characterized by certain critical process conditions, these being the use of:
  • an alkali metal and/or alkaline earth metal chloride electrolyte being above about 0.5N to saturation in chloride ion
  • US. Pat. No. 2,839,461 describes an electrolytic process for the recovery of nickel from nickel sulfide utilizing an acid sulfate-chloride electrolyte and which is dependent upon the anode current being passed through a nickel matte anode.
  • the process has the disadvantage of requiring concentrates suitable for the production of the required anode matte and is subject to the substantial expense of anode preparation and removal from the cells with subsequent treatment.
  • the process herein disclosed has the advantage over prior pyrometallurgical process of converting the sulfide sulfur to elemental sulfur rather than sulfur dioxide with its attendant air pollution and the advantage over the process disclosed in US. Pat. No. 2,839,461 of being adaptable to low grade and complex concentrates, and not requiring the production of a matte anode in the case of nickel and cobalt.
  • metal sulfide as contained herein is inclusive of the complex as well as the simple sulfide minerals which contain economically recoverable amounts of the specified metals.
  • the invention is a pollution-free process for recovery of metals of Group VIII of the Periodic Table from their sulfide and mixed sulfide ores in which the sulfide is electrochemically dissociated in an acid aqueous media into elemental sulfur and metal ions which are then recovered from solution in the electrolyte media by conventional techniques.
  • the electrolysis process is characterized by certain critical process conditions which render it economically feasible, these being the use of:
  • the process parameters which have been found to control the current requirement for the process are electrolyte composition, feed particle size, operating acidity, operating temperature, and anode current density. As the examples which follow show, these factors are mutually interacting and dependent as respects their effect on current requirements.
  • the electrolytic media for the process must be acidic as an alkaline electrolyte has proven unsatisfactory. Elemental sulfur is not stable in an alkaline environment because oxidation of the sulfur proceeds rapidly in this media through thiosulfate, hydrosulfite, sulfite to sulfate. The presence of sulfate ions is undesirable because at high sulfate concentrations oxygen is rapidly evolved at the anode resulting in a decrease in current efficiency.
  • the preferred electrolyte media is an aqueous acidic solution of alkali metal chloride or alkaline earth metal chloride or mixtures thereof.
  • the chlorides of sodium, potassium, barium and calcium or mixtures thereof, have been found suitable. Concentrations from 0.5N to saturation may be used. Voltage across the cell is lower at higher salt concentrations so that these are preferred except where low grade feeds are used and where salt losses would therefore become significant.
  • the particle size of the feed material is critical as it directly effects the conversion to elemental sulfur.
  • the sulfur produced is extremely fine.
  • the anode current attacks the metal sulfide preferentially to sulfur provided the sulfide has sufficient activity near the anode.
  • the activity of the sulfide is a function of its concentration and its exposed surface area. Therefore the presence of a high concentration of fine sulfide near the anode prevents the continuing oxidation of sulfur and results in higher efficiency and consequently lower current consumption.
  • An average grain size range for the feed sulfide smaller than about 60 mesh US. Standard is the operable range.
  • An acidity for the electrolyte media up to about 3.9 is critical. Current efficiency is reduced at a pH above 3.9.
  • the preferred acidity is about pH 0.5.
  • the reaction temperature of the electrolyte is critical and high process efficiency is not obtained at low temperature. At temperature below about 50 C, the reaction for the conversion of sulfide to sulfate rather than to sulfur is increasingly favored. A temperature range of about 50 to 105 C is the operable range. A temperature of about C is most preferred.
  • Anode current density is also critical as used with the other critical parameters with a preferred range being between 12 amperes/ft and 240 amperes/ft with the minimum being about 12 amperes/ft? While high efficiency may be maintained at relatively high current densities when ample fresh feed is present, it is necessary to decrease current density as the concentration of sulfur becomes high in proportion to that of the mineral being attacked.
  • the metal dissolved in the electrolyte can be finally recovered by conventional methods such as, electrolysis, precipitation, cementation, etc. Under certain conditions the metal can be plated out on the cathode during the dissociation process and recovered in this manner.
  • Elemental sulfur is readily recovered from the electrolyte media by the process disclosed in co-pending patent application Ser. No. 233,352 filed in the US Patent Office on Mar. 9, 1972, William G. Kazel, entitled Sulfur Recovery Process.
  • the feed concentrate for all of the examples was 60 mesh US. Standard. Current density is given in amperes per square foot. Current requirement is expressed in amperes per pound of metal or combined metal recovered.
  • Examples 1-4 400 grams of a nickel sulfide concentrate assaying 8.3 percent nickel, 5.2 percent copper, 37.8 percent iron were slurried in 2 liters of electrolyte and subjected to 60 ampere hours of current.
  • EXAMPLE 1 The following tests were performed to determine the approximate lower limit of the operable temperature range for recovering nickel and iron from nickel sulfide using a sodium chloride electrolyte and other parameters of the process.
  • EXAMPLE 2 The following tests were selected to show the effect of pH on the recovery of nickel and iron from nickel sulfide by the process.
  • EXAMPLE 5 The following test was selected to show the operativeness of the process for the recovery of cobalt, nickel and iron from their sulfides. 400 grams of nickel sulfide concentrate assaying 8.3 percent nickel, 5.2 percent copper, 37.8 percent iron and 0.337 percent cobalt were slurried in two liters of electrolyte and subjected to 90 ampere hours of current.
  • the process is effective for the recovery of cobalt as well as iron and nickel from their sulfides with good conversion of sulfur and satisfactory current requirements.
  • the power requirements set forth in the examples are well within commercial feasibility ranges for large scale production of nickel, iron and cobalt from their sulfide and mixed sulfide ores.
  • the cost of the recovery of the metals and sulfur from the electrolyte after electrolysis by conventional techniques is comparatively small.
  • the high percentage recovery of sulfur from the sulfides as elemental sulfur substantially reduces or eliminates the pollution problems associated with prior art processes. Accordingly, the invention provides a process for the recovery of nickel and cobalt from their sulfide and mixed sulfide ores which has the advantages of being commercially feasible and pollution free.
  • a process for the recovery of metals selected from the group consisting of iron, nickel and cobalt from their sulfides and mixed sulfides, and mixtures thereof, by electrolytic dissolution with the formation of elemental sulfur which process comprises:
  • an electrolyte in an electrolytic cell including at least an anode and a cathode, the electrolyte comprising an acidic aqueous solution of at least one chloride salt selected from the group consisting of alkali metal chlorides and alkaline earth metal chlorides, the solution having a concentration from about 0.5N to saturation;
  • alkali metal chlorides are sodium and potassium chlorides and the alkaline earth metal chlorides are calcium and magnesium chlorides.

Landscapes

  • Chemical & Material Sciences (AREA)
  • Engineering & Computer Science (AREA)
  • Chemical Kinetics & Catalysis (AREA)
  • Electrochemistry (AREA)
  • Materials Engineering (AREA)
  • Metallurgy (AREA)
  • Organic Chemistry (AREA)
  • Electrolytic Production Of Metals (AREA)
  • Manufacture And Refinement Of Metals (AREA)

Abstract

A pollution-free process for the electrolytic dissolution of sulfide concentrates of the metals of Group VIII of the Periodic Table in aqueous acidic media with the formation of metal ions and elemental sulfur followed by recovery of the metal ion from solution in the electrolyte media, the process characterized by certain critical process conditions, these being the use of: 1. AN ALKALI METAL AND/OR ALKALINE EARTH METAL CHLORIDE ELECTROLYTE BEING ABOVE ABOUT 0.5N to saturation in chloride ion, 2. A SULFIDE FEED OF AVERAGE PARTICLE SIZE SMALLER THAN 60 MESH U.S. Standard, 3. A PH range of about 0.01 - 3.9, 4. AN ELECTROLYTE TEMPERATURE OF ABOUT 50*C - 105* C, and 5. AN ANODE CURRENT DENSITY ABOVE ABOUT 12 AMPERES/FT2.

Description

nited States Patent [1 1 Kruesi [75] Inventor: Paul R. Kruesi, Golden, C010.
[73] Assignee: Cyprus Metallurgical Processes Corporation, Los Angeles, Calif.
[22] Filed: May 10, 1972 [21] Appl. No.: 251,940
[52] U.S. Cl. 204/113, 204/128 [51] Int. Cl...... C22d l/14, C22d 1/24, COlb 17/06 [58] Field of Search 204/113, 128
[56] References Cited UNITED STATES PATENTS 967,996 8/1910 Summers 204/130 840,511 l/l907 Packard 204/130 3,673,061 6/1972 Kruesi 204/105 R 3,464,904 9/1969 Brace 204/105 R FOREIGN PATENTS 0R APPLICATIONS 556,169 4/1958 Canada 204/128 Oct. 16, 1973 Primary Examiner-John H. Mack Assistant Examiner-R. L. Andrews Attorney-Sheridan, Ross & Fields [5 7] ABSTRACT A pollution-free process for the electrolytic dissolution of sulfide concentrates of the metals of Group VIII of the Periodic Table in aqueous acidic media with the formation of metal ions and elemental sulfur followed by recovery of the metal ion from solution in the electrolyte media, the process characterized by certain critical process conditions, these being the use of:
1. an alkali metal and/or alkaline earth metal chloride electrolyte being above about 0.5N to saturation in chloride ion,
2. a sulfide feed of average particle size smaller than 60 mesh U.S. Standard,
3. a pH range of about 0.01 3.9,
4. an electrolyte temperature of about 50C 105 C, and
5. an anode current density above about 12 amperes/ft 15 Claims, No Drawings ELECTROLYTIC PROCESS FOR THE RECOVERY OF NICKEL, COBALT AND IRON FROM THEIR SULFIDES BACKGROUND OF THE INVENTION Metals of Group VIII of the Periodic Table have been conventionally recovered from their sulfide concentrates by pyrometallurgical smelting techniques. This has required a high degree of concentration for economic processing particularly for nickel and cobalt and thus low grade concentrates or complex concentrates which were not amenable to physical separation are often considered valueless or of low value.
The pyrometallurgical processes in which sulfur contained in the ores is oxidized to sulfur dioxide of which a substantial proportion is released to the atmosphere with consequent damage to the environment are a cause of substantial concern. An electrolytic process requiring only economic quantities of power, in which substantially all of the sulfur in the above metal sulfides is converted to elemental sulfur is an answer to this air pollution problem.
US. Pat. No. 2,839,461 describes an electrolytic process for the recovery of nickel from nickel sulfide utilizing an acid sulfate-chloride electrolyte and which is dependent upon the anode current being passed through a nickel matte anode. The process has the disadvantage of requiring concentrates suitable for the production of the required anode matte and is subject to the substantial expense of anode preparation and removal from the cells with subsequent treatment.
The process herein disclosed has the advantage over prior pyrometallurgical process of converting the sulfide sulfur to elemental sulfur rather than sulfur dioxide with its attendant air pollution and the advantage over the process disclosed in US. Pat. No. 2,839,461 of being adaptable to low grade and complex concentrates, and not requiring the production of a matte anode in the case of nickel and cobalt.
STATEMENT OF THE INVENTION The term metal sulfide as contained herein is inclusive of the complex as well as the simple sulfide minerals which contain economically recoverable amounts of the specified metals.
The invention is a pollution-free process for recovery of metals of Group VIII of the Periodic Table from their sulfide and mixed sulfide ores in which the sulfide is electrochemically dissociated in an acid aqueous media into elemental sulfur and metal ions which are then recovered from solution in the electrolyte media by conventional techniques. The electrolysis process is characterized by certain critical process conditions which render it economically feasible, these being the use of:
1. an alkali or alkaline earth metal chloride electrolyte,
2. a sulfide feed particle size smaller than about 60 mesh U.S. Standard,
3. a pH range below about 3.9,
4. an electrolyte temperature range of about 50 105 C, and
5. an anode current density above about 12 ampereslft DETAILED DESCRIPTION OF THE INVENTION The economic feasibility of the process is dependent upon the current required to produce a given quantity of metal. It is expressed herein in terms of the ampere hours of current required to release a pound of metal. Because nickel ores frequently contain substantial quantities of iron and copper which may be coproducts, the efficiency here is expressed as the ampere hours necessary to release one pound of the combined metal.
The process parameters which have been found to control the current requirement for the process are electrolyte composition, feed particle size, operating acidity, operating temperature, and anode current density. As the examples which follow show, these factors are mutually interacting and dependent as respects their effect on current requirements.
The electrolytic media for the process must be acidic as an alkaline electrolyte has proven unsatisfactory. Elemental sulfur is not stable in an alkaline environment because oxidation of the sulfur proceeds rapidly in this media through thiosulfate, hydrosulfite, sulfite to sulfate. The presence of sulfate ions is undesirable because at high sulfate concentrations oxygen is rapidly evolved at the anode resulting in a decrease in current efficiency.
The preferred electrolyte media is an aqueous acidic solution of alkali metal chloride or alkaline earth metal chloride or mixtures thereof. The chlorides of sodium, potassium, barium and calcium or mixtures thereof, have been found suitable. Concentrations from 0.5N to saturation may be used. Voltage across the cell is lower at higher salt concentrations so that these are preferred except where low grade feeds are used and where salt losses would therefore become significant.
It is highly important that a high percentage of the sulfur in the metal sulfide be recovered as elemental sulfur both from the standpoint of pollution control and from the electrical efficiency of the process. Each mole of sulfur which is oxidized from elemental sulfur to sulfate rather than being converted to elemental sulfur requires six Faradays which is equivalent to 2,275 ampere hours per pound of sulfur. This renders oxidation of the sulfur to sulfate prohibitive for an economically acceptable process.
The particle size of the feed material is critical as it directly effects the conversion to elemental sulfur. The sulfur produced is extremely fine. The anode current attacks the metal sulfide preferentially to sulfur provided the sulfide has sufficient activity near the anode. The activity of the sulfide is a function of its concentration and its exposed surface area. Therefore the presence of a high concentration of fine sulfide near the anode prevents the continuing oxidation of sulfur and results in higher efficiency and consequently lower current consumption. An average grain size range for the feed sulfide smaller than about 60 mesh US. Standard is the operable range.
An acidity for the electrolyte media up to about 3.9 is critical. Current efficiency is reduced at a pH above 3.9. The preferred acidity is about pH 0.5.
The reaction temperature of the electrolyte is critical and high process efficiency is not obtained at low temperature. At temperature below about 50 C, the reaction for the conversion of sulfide to sulfate rather than to sulfur is increasingly favored. A temperature range of about 50 to 105 C is the operable range. A temperature of about C is most preferred.
Anode current density is also critical as used with the other critical parameters with a preferred range being between 12 amperes/ft and 240 amperes/ft with the minimum being about 12 amperes/ft? While high efficiency may be maintained at relatively high current densities when ample fresh feed is present, it is necessary to decrease current density as the concentration of sulfur becomes high in proportion to that of the mineral being attacked.
The metal dissolved in the electrolyte can be finally recovered by conventional methods such as, electrolysis, precipitation, cementation, etc. Under certain conditions the metal can be plated out on the cathode during the dissociation process and recovered in this manner.
Elemental sulfur is readily recovered from the electrolyte media by the process disclosed in co-pending patent application Ser. No. 233,352 filed in the US Patent Office on Mar. 9, 1972, William G. Kazel, entitled Sulfur Recovery Process.
The following examples are illustrative of the invention but not limiting thereof.
The examples were performed in apparatus well known in the art consisting of an anode section provided with means for agitation, a suitable anode, a cloth diaphragm and a suitable cathode in a cathode section. Conventional non-diaphragm cells may be used.
The feed concentrate for all of the examples was 60 mesh US. Standard. Current density is given in amperes per square foot. Current requirement is expressed in amperes per pound of metal or combined metal recovered.
1n Examples 1-4, 400 grams of a nickel sulfide concentrate assaying 8.3 percent nickel, 5.2 percent copper, 37.8 percent iron were slurried in 2 liters of electrolyte and subjected to 60 ampere hours of current.
EXAMPLE 1 The following tests were performed to determine the approximate lower limit of the operable temperature range for recovering nickel and iron from nickel sulfide using a sodium chloride electrolyte and other parameters of the process.
TEST NO. 1 2 3 4N 4N 4N Electrolyte NaCl NaCl NaCl Temperature 80C' 50C 30C pH 0.5 0.5 0.5 Anode Current Density (Amps/ft) 120 120 120 Metal and Sulfur Recovered (gm.)
Fe 69.5 27.7- 21.0 Ni 6.5 3.1 2.8 Cu 6.4 1.3 3.3 S 42.2 1 1.4 7.8 Amp. Hrs./lb. Combined Metals 330.5 848.5 1005.2 Recovered The tests show that reduction of the operating temperature below about 50 C results in excessive current requirements and drastic reduction in the conversion of sulfide sulfur to elemental sulfur.
EXAMPLE 2 The following tests were selected to show the effect of pH on the recovery of nickel and iron from nickel sulfide by the process.
TEST NO. 1 2 3 4 5 Electrolyte NaCl NaCl NaCl NaCl NuCl Temperature C 80C 80C 80C 80C pH 0.01(5%HC|) 0.5 1.5 2.0 4.0 Anode Current Density Amps/ft 120 120 120 120 Metal and Sulfur Recovered (gm) Fe 71.8 69.5 51.3 37.8 9.8 Ni 5.6 6.5 3.2 1.2 0.6 Cu 3.5 6.4 5.6 1.1 0.5 S 52.8 42.2 36.3 28.6 22.2 Amp. Hrs/1b. Combined Metals 336.9 330.5 453.1 679.2 2499.3 Recovered The increase in current requirement and decrease in conversion of sulfide sulfur to elemental sulfur above pH 1.5 as acidity decreases indicates the preferred pH. Above pH 3.9, the upper limit of pH range, 2,499.3 amperes/lb. of metal recovered were required and sulfur conversion was reduced to 22.2 grams.
EXAMPLE 3 The following tests were made to explore the preferred current density range for the process.
TEST NO. 1 2 3 4 4N 4N 4N 4N Electrolyte NaCl NaCl NaCl NaCl Temperature 80C 80C 80C 80C p 0.5 0.5 0.5 0.5 Anode Current Density(Amps/ft 480 240 120 60 Metal and Sulfur Recovered (gm.)
Fe 38.8 36.2 69.5 66.1 Ni 4.0 4.4 6.5 5.0 Cu 5.2 6.3 6.4 3.7 S 24.2 27.0 42.2 39.0 Amp. Hrs/lb. Combined Metals Recovered 567.5 580.7 330.5 364.1
The results indicate that current densities at or below about 120 amps/ft are preferable to those above this figure. The lower limit of the economically feasible current density range is about 12 amps/ft? EXAMPLE 4 The tests below were performed to explore the effectiveness of other electrolytes than NaCl and to determine the effect of the presence of sulfate ion in the electrolyte on the operativeness of the process for recovering nickel and iron from nickel sulfide concentrate.
The tests show that potassium chloride as well as the alkaline earth metal chlorides, calcium chloride and magnesium chloride, are effective electrolytes for the process. In Test No. 5 the sodium sulfate-sodium chloride electrolyte of U.S. Pat. No. 2,839,461 is shown to be less effective than the other electrolytes as indicated by the decrease in sulfur conversion.
EXAMPLE 5 The following test was selected to show the operativeness of the process for the recovery of cobalt, nickel and iron from their sulfides. 400 grams of nickel sulfide concentrate assaying 8.3 percent nickel, 5.2 percent copper, 37.8 percent iron and 0.337 percent cobalt were slurried in two liters of electrolyte and subjected to 90 ampere hours of current.
Electrolyte 4N NaCl Temperature 80C p 0.5 Anode Current Density(Amps/ft) 60 Metal and Sulfur of Feed Metal Recovered (gms.) Recovered Fe 88.7 61.8 Ni 16.6 54.1 Cu 9.35 49.1 Co 0.63 51.7 S 58.4 Amp.Hrs./lb.
Combined Metals Recovered 354.6
As the results indicate, the process is effective for the recovery of cobalt as well as iron and nickel from their sulfides with good conversion of sulfur and satisfactory current requirements.
EXAMPLE 6 Electrolyte 4N NaCl Temperature 80C p 0.01 5% HCl) Anode Current Density (Amps/ft) l20 Metal and Sulfur Recovered (gms) Co 0.5 Ni 0.2
S 19.9 Amps. HrsJlb. Combined Metals Recovered 472.2
The high conversion of sulfur and the relatively low current requirements with satisfactory recovery of cobalt show that the process can be used economically for the recovery of cobalt from low grade complex cobalt sulfide ores.
The power requirements set forth in the examples are well within commercial feasibility ranges for large scale production of nickel, iron and cobalt from their sulfide and mixed sulfide ores. The cost of the recovery of the metals and sulfur from the electrolyte after electrolysis by conventional techniques is comparatively small. The high percentage recovery of sulfur from the sulfides as elemental sulfur substantially reduces or eliminates the pollution problems associated with prior art processes. Accordingly, the invention provides a process for the recovery of nickel and cobalt from their sulfide and mixed sulfide ores which has the advantages of being commercially feasible and pollution free.
I claim:
1. A process for the recovery of metals selected from the group consisting of iron, nickel and cobalt from their sulfides and mixed sulfides, and mixtures thereof, by electrolytic dissolution with the formation of elemental sulfur, which process comprises:
a. providing an electrolyte in an electrolytic cell including at least an anode and a cathode, the electrolyte comprising an acidic aqueous solution of at least one chloride salt selected from the group consisting of alkali metal chlorides and alkaline earth metal chlorides, the solution having a concentration from about 0.5N to saturation;
b. mixing with the electrolyte a solid feed sulfide of the metal having an average particle size smaller than about 60 mesh U.S. Standard;
c. maintaining the temperature of the electrolyte media at about 50 to C, and the pH of the electrolyte media below about 3.9 while introducing electric current into the electrolytic cell to provide an anode current density above about 12 amperes per square foot to dissociate the metal sulfide into metal ions and elemental sulfur; and
d. recovering the metal from the electrolyte.
2. The process of claim l in which cobalt and nickel are recovered from the sulfides in the presence of iron sulfides.
3. The process of claim 1 including the final step of recovering the metal from solution in the electrolyte by electrode-position on the cathode.
4..The process of claim it including the step of recovering elemental sulfur from the electrolyte.
5. The process of claim 1 in which the metal recovered is nickel.
6. The process of claim 1 in which the metal recovered is cobalt.
7. The process of claim 1 in which the metal recovered is iron.
8. The process of claim l in which the alkali metal chlorides are sodium and potassium chlorides and the alkaline earth metal chlorides are calcium and magnesium chlorides.
9. The process of claim 8 in which the electrolyte is sodium chloride and the metal'recovered is a metal selected from the group consisting of iron, nickel and cobalt.
10. The process of claim 9 in which the metal recovered is nickel.
11. The process of claim 9 in which the metal recovered is cobalt.
12. The process of claim 9 in which the metal recovered is iron.
13. The process-of claim 8 in which the alkali metal chloride is potassium and the metals recovered are nickel and iron.
14. The process of claim 8 in which the alkaline earth metal chloride is calcium chloride and the metals recovered are nickel and iron.
15. The process of claim 8 in which the alkaline earth metal chloride is magnesium chloride and the metals recovered are nickel and iron.

Claims (19)

1. AND ALKALI METAL AND/OR ALKALINE EARTH METAL CHLORIDE ELECTROLYTE BEING ABOVE ABOUT 0.5N TO SATURATION IN CHLORIDE ION,
2. A SULFIDE FEED OF AVERAGE PARTICLE SIZE SMALLER THAN 60 MESH U.S. STANDARD,
2. The process of claim 1 in which cobalt and nickel are recovered from the sulfides in the presence of iron sulfides.
3. The process of claim 1 including the final step of recovering the metal from solution in the electrolyte by electrode-position on the cathode.
3. A PH RANGE OF ABOUT 0.01-3.9,
4. AND ELECTROLYTE TEMPERATURE OF ABOUT 50*C-105*C, AND
4. The process of claim 1 including the step of recovering elemental sulfur from the electrolyte.
5. The process of claim 1 in which the metal recovered is nickel.
5. AN ANODE CURRENT DENSITY ABOVE ABOUT 12 AMPERES-FT2.
6. The process of claim 1 in which the metal recovered is cobalt.
7. The process of claim 1 in which the metal recovered is iron.
8. The process of claim 1 in which the alkali metal chlorides are sodium and potassium chlorides and the alkaline earth metal chlorides are calcium and magnesium chlorides.
9. The process of claim 8 in which the electrolyte is sodium chloride and the metal recovered is a metal selected from the group consisting of iron, nickel and cobalt.
10. The process of claim 9 in which the metal recovered is nickel.
11. The process of claim 9 in which the metal recovered is cobalt.
12. The process of claim 9 in which the metal recovered is iron.
13. The process of claim 8 in which the alkali metal chloride is potassium and the metals recovered are nickel and iron.
14. The process of claim 8 in which the alkaline earth metal chloride is calcium chloride and the metals recovered are nickel and iron.
15. The process of claim 8 in which the alkaline earth metal chloride is magnesium chloride and the metals recovered are nickel and iron.
US00251940A 1972-05-10 1972-05-10 Electrolytic process for the recovery of nickel, cobalt and iron from their sulfides Expired - Lifetime US3766026A (en)

Applications Claiming Priority (1)

Application Number Priority Date Filing Date Title
US25194072A 1972-05-10 1972-05-10

Publications (1)

Publication Number Publication Date
US3766026A true US3766026A (en) 1973-10-16

Family

ID=22954020

Family Applications (1)

Application Number Title Priority Date Filing Date
US00251940A Expired - Lifetime US3766026A (en) 1972-05-10 1972-05-10 Electrolytic process for the recovery of nickel, cobalt and iron from their sulfides

Country Status (1)

Country Link
US (1) US3766026A (en)

Cited By (3)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US4060464A (en) * 1974-06-26 1977-11-29 Boliden Aktiebolag Method for extracting and recovering iron and nickel in metallic form
US20050266165A1 (en) * 2004-05-27 2005-12-01 Enthone Inc. Method for metallizing plastic surfaces
US11753732B2 (en) 2021-03-24 2023-09-12 Electrasteel, Inc. Ore dissolution and iron conversion system

Citations (5)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US840511A (en) * 1906-01-11 1907-01-08 Robert L Packard Extracting metals from sulfid ores.
US967996A (en) * 1909-04-08 1910-08-23 Leland L Summers Method of extracting or eliminating sulfur, phosphorus, and other impurities from coal, ore, &c.
CA556169A (en) * 1958-04-22 H. Dolloff Norman Polarization prevention in electrolysis of sulfide ores
US3464904A (en) * 1964-12-21 1969-09-02 Banner Mining Co Method for treating metallic sulfide compounds
US3673061A (en) * 1971-02-08 1972-06-27 Cyprus Metallurg Process Process for the recovery of metals from sulfide ores through electrolytic dissociation of the sulfides

Patent Citations (5)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
CA556169A (en) * 1958-04-22 H. Dolloff Norman Polarization prevention in electrolysis of sulfide ores
US840511A (en) * 1906-01-11 1907-01-08 Robert L Packard Extracting metals from sulfid ores.
US967996A (en) * 1909-04-08 1910-08-23 Leland L Summers Method of extracting or eliminating sulfur, phosphorus, and other impurities from coal, ore, &c.
US3464904A (en) * 1964-12-21 1969-09-02 Banner Mining Co Method for treating metallic sulfide compounds
US3673061A (en) * 1971-02-08 1972-06-27 Cyprus Metallurg Process Process for the recovery of metals from sulfide ores through electrolytic dissociation of the sulfides

Cited By (6)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US4060464A (en) * 1974-06-26 1977-11-29 Boliden Aktiebolag Method for extracting and recovering iron and nickel in metallic form
US20050266165A1 (en) * 2004-05-27 2005-12-01 Enthone Inc. Method for metallizing plastic surfaces
US11753732B2 (en) 2021-03-24 2023-09-12 Electrasteel, Inc. Ore dissolution and iron conversion system
US11767604B2 (en) 2021-03-24 2023-09-26 Electrasteel, Inc. 2-step iron conversion system
US12054837B2 (en) 2021-03-24 2024-08-06 Electrasteel, Inc. Ore dissolution and iron conversion system
US12065749B2 (en) 2021-03-24 2024-08-20 Electrasteel, Inc. 2-step iron conversion system

Similar Documents

Publication Publication Date Title
US3930969A (en) Process for oxidizing metal sulfides to elemental sulfur using activated carbon
US3673061A (en) Process for the recovery of metals from sulfide ores through electrolytic dissociation of the sulfides
US3736238A (en) Process for the recovery of metals from sulfide ores through electrolytic dissociation of the sulfides
GB1481663A (en) Electrowinning of metals
US3901776A (en) Process for the recovery of copper from its sulfide ores
KR960008617B1 (en) Process for recovering sulfuric acid
US3994789A (en) Galvanic cementation process
US4061552A (en) Electrolytic production of copper from ores and concentrates
US3853724A (en) Process for electrowinning of copper values from solid particles in a sulfuric acid electrolyte
US3766026A (en) Electrolytic process for the recovery of nickel, cobalt and iron from their sulfides
CA2593046A1 (en) Procedure and device to obtain metal powder, plates or cathodes from any metal-containing material
US4684450A (en) Production of zinc from ores and concentrates
US3755104A (en) Process for the recovery of molybdenum and rhenium from sulfides by electrolytic dissolution
JPS5844157B2 (en) Purification method of nickel electrolyte
US2766197A (en) Production of manganese
EP0026207B1 (en) Production of lead from ores and concentrates
Jiricny et al. Copper electrowinning using spouted-bed electrodes: Part II. Copper electrowinning with ferrous ion oxidation as the anodic reaction
RU2023758C1 (en) Method of electrochemically lixiviating copper from copper sulfide concentrate
USRE14436E (en) gidden
GB2025461A (en) Recovery of copper from sulphide ores
JPS5620186A (en) Treatment of dross contained copper and lead
Lemay The anodic oxidation of bivalent manganese to tetravalent manganese.
IE43392B1 (en) Extraction of copper from ores and concentrates
CS198967B1 (en) Process for electrolytic deposition of ferrous alloys
PL88404B1 (en)

Legal Events

Date Code Title Description
AS Assignment

Owner name: CYPRUS MINES CORPORATION; A CORP OF DE, COLORAD

Free format text: ASSIGNMENT OF ASSIGNORS INTEREST;ASSIGNOR:CYPRUS METALLURGICAL PROCESSES CORPORATION;REEL/FRAME:004020/0240

Effective date: 19820615

Owner name: CYPRUS MINES CORPORATION; 7000 SOUTH YOSEMITE ST.,

Free format text: ASSIGNMENT OF ASSIGNORS INTEREST.;ASSIGNOR:CYPRUS METALLURGICAL PROCESSES CORPORATION;REEL/FRAME:004020/0240

Effective date: 19820615