Cupric Chloride Leaching of Chalcopyrite
Abstract In a strong chloride solution the predominant cuprous, cupric, ferrous, and ferric chloride complexes are $ CuCl_{3} $−2, $ CuCl^{+} $, $ CuCl_{2} $, $ FeCl_{2} $, and $ FeCl_{2} $+ respectively. The probable dissolution reaction for chalcopyrite in cupric chloride solution is $ CuFeS_{2} $...
Ausführliche Beschreibung
Gespeichert in:
| Autor*in: |
Wilson, J. P. [verfasserIn] |
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| Format: |
E-Artikel |
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| Sprache: |
Englisch |
| Erschienen: |
1981 |
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| Schlagwörter: |
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| Anmerkung: |
© The Minerals, Metals & Materials Society 1981 |
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| Übergeordnetes Werk: |
Enthalten in: JOM - New York, NY : Springer Science + Business Media, 1989, 33(1981), 2 vom: Feb., Seite 52-57 |
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| Übergeordnetes Werk: |
volume:33 ; year:1981 ; number:2 ; month:02 ; pages:52-57 |
| Links: |
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| DOI / URN: |
10.1007/BF03354527 |
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SPR022666222 |
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| 245 | 1 | 0 | |a Cupric Chloride Leaching of Chalcopyrite |
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| 520 | |a Abstract In a strong chloride solution the predominant cuprous, cupric, ferrous, and ferric chloride complexes are $ CuCl_{3} $−2, $ CuCl^{+} $, $ CuCl_{2} $, $ FeCl_{2} $, and $ FeCl_{2} $+ respectively. The probable dissolution reaction for chalcopyrite in cupric chloride solution is $ CuFeS_{2} $ + $ 3CuCl^{+} $ + $ 11Cl^{−2} $ = $ 4CuCl_{3} $−2 + $ FeCl_{2} $ + 2S The standard free energy change for this reaction at 25°C and unit activities is +43.84 kJ, indicating that the reaction is not thermodynamically feasible. The reaction becomes thermodynamically feasible at high chloride concentration when the ratio of cuprous to cupric copper in solution is less than about 1.9. When the cuprous to cupric ratio becomes larger than a critical value (dependent upon the operating conditions) the dissolution ceases because it is no longer thermodynamically feasible. Over the range 0.79–1.46 M $ Cu^{+2} $ and 2.82–6.21 M $ Cl^{−} $ at 90°C, neither cupric nor chloride ion concentration influences the rate of chalcopyrite dissolution, which is directly proportional to mineral surface area. The activation energy for the reaction is 134.7 kJ/mole, and the rate controlling process is probably a step in the anodic reaction. | ||
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10.1007/BF03354527 doi (DE-627)SPR022666222 (SPR)BF03354527-e DE-627 ger DE-627 rakwb eng Wilson, J. P. verfasserin aut Cupric Chloride Leaching of Chalcopyrite 1981 Text txt rdacontent Computermedien c rdamedia Online-Ressource cr rdacarrier © The Minerals, Metals & Materials Society 1981 Abstract In a strong chloride solution the predominant cuprous, cupric, ferrous, and ferric chloride complexes are $ CuCl_{3} $−2, $ CuCl^{+} $, $ CuCl_{2} $, $ FeCl_{2} $, and $ FeCl_{2} $+ respectively. The probable dissolution reaction for chalcopyrite in cupric chloride solution is $ CuFeS_{2} $ + $ 3CuCl^{+} $ + $ 11Cl^{−2} $ = $ 4CuCl_{3} $−2 + $ FeCl_{2} $ + 2S The standard free energy change for this reaction at 25°C and unit activities is +43.84 kJ, indicating that the reaction is not thermodynamically feasible. The reaction becomes thermodynamically feasible at high chloride concentration when the ratio of cuprous to cupric copper in solution is less than about 1.9. When the cuprous to cupric ratio becomes larger than a critical value (dependent upon the operating conditions) the dissolution ceases because it is no longer thermodynamically feasible. Over the range 0.79–1.46 M $ Cu^{+2} $ and 2.82–6.21 M $ Cl^{−} $ at 90°C, neither cupric nor chloride ion concentration influences the rate of chalcopyrite dissolution, which is directly proportional to mineral surface area. The activation energy for the reaction is 134.7 kJ/mole, and the rate controlling process is probably a step in the anodic reaction. Chalcopyrite (dpeaa)DE-He213 CuCl (dpeaa)DE-He213 Free Energy Change (dpeaa)DE-He213 Extractive Metallurgy (dpeaa)DE-He213 Standard Free Energy Change (dpeaa)DE-He213 Fisher, W. W. aut Enthalten in JOM New York, NY : Springer Science + Business Media, 1989 33(1981), 2 vom: Feb., Seite 52-57 (DE-627)31368197X (DE-600)2002726-6 1543-1851 nnns volume:33 year:1981 number:2 month:02 pages:52-57 https://dx.doi.org/10.1007/BF03354527 lizenzpflichtig Volltext GBV_USEFLAG_A SYSFLAG_A GBV_SPRINGER AR 33 1981 2 02 52-57 |
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10.1007/BF03354527 doi (DE-627)SPR022666222 (SPR)BF03354527-e DE-627 ger DE-627 rakwb eng Wilson, J. P. verfasserin aut Cupric Chloride Leaching of Chalcopyrite 1981 Text txt rdacontent Computermedien c rdamedia Online-Ressource cr rdacarrier © The Minerals, Metals & Materials Society 1981 Abstract In a strong chloride solution the predominant cuprous, cupric, ferrous, and ferric chloride complexes are $ CuCl_{3} $−2, $ CuCl^{+} $, $ CuCl_{2} $, $ FeCl_{2} $, and $ FeCl_{2} $+ respectively. The probable dissolution reaction for chalcopyrite in cupric chloride solution is $ CuFeS_{2} $ + $ 3CuCl^{+} $ + $ 11Cl^{−2} $ = $ 4CuCl_{3} $−2 + $ FeCl_{2} $ + 2S The standard free energy change for this reaction at 25°C and unit activities is +43.84 kJ, indicating that the reaction is not thermodynamically feasible. The reaction becomes thermodynamically feasible at high chloride concentration when the ratio of cuprous to cupric copper in solution is less than about 1.9. When the cuprous to cupric ratio becomes larger than a critical value (dependent upon the operating conditions) the dissolution ceases because it is no longer thermodynamically feasible. Over the range 0.79–1.46 M $ Cu^{+2} $ and 2.82–6.21 M $ Cl^{−} $ at 90°C, neither cupric nor chloride ion concentration influences the rate of chalcopyrite dissolution, which is directly proportional to mineral surface area. The activation energy for the reaction is 134.7 kJ/mole, and the rate controlling process is probably a step in the anodic reaction. Chalcopyrite (dpeaa)DE-He213 CuCl (dpeaa)DE-He213 Free Energy Change (dpeaa)DE-He213 Extractive Metallurgy (dpeaa)DE-He213 Standard Free Energy Change (dpeaa)DE-He213 Fisher, W. W. aut Enthalten in JOM New York, NY : Springer Science + Business Media, 1989 33(1981), 2 vom: Feb., Seite 52-57 (DE-627)31368197X (DE-600)2002726-6 1543-1851 nnns volume:33 year:1981 number:2 month:02 pages:52-57 https://dx.doi.org/10.1007/BF03354527 lizenzpflichtig Volltext GBV_USEFLAG_A SYSFLAG_A GBV_SPRINGER AR 33 1981 2 02 52-57 |
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10.1007/BF03354527 doi (DE-627)SPR022666222 (SPR)BF03354527-e DE-627 ger DE-627 rakwb eng Wilson, J. P. verfasserin aut Cupric Chloride Leaching of Chalcopyrite 1981 Text txt rdacontent Computermedien c rdamedia Online-Ressource cr rdacarrier © The Minerals, Metals & Materials Society 1981 Abstract In a strong chloride solution the predominant cuprous, cupric, ferrous, and ferric chloride complexes are $ CuCl_{3} $−2, $ CuCl^{+} $, $ CuCl_{2} $, $ FeCl_{2} $, and $ FeCl_{2} $+ respectively. The probable dissolution reaction for chalcopyrite in cupric chloride solution is $ CuFeS_{2} $ + $ 3CuCl^{+} $ + $ 11Cl^{−2} $ = $ 4CuCl_{3} $−2 + $ FeCl_{2} $ + 2S The standard free energy change for this reaction at 25°C and unit activities is +43.84 kJ, indicating that the reaction is not thermodynamically feasible. The reaction becomes thermodynamically feasible at high chloride concentration when the ratio of cuprous to cupric copper in solution is less than about 1.9. When the cuprous to cupric ratio becomes larger than a critical value (dependent upon the operating conditions) the dissolution ceases because it is no longer thermodynamically feasible. Over the range 0.79–1.46 M $ Cu^{+2} $ and 2.82–6.21 M $ Cl^{−} $ at 90°C, neither cupric nor chloride ion concentration influences the rate of chalcopyrite dissolution, which is directly proportional to mineral surface area. The activation energy for the reaction is 134.7 kJ/mole, and the rate controlling process is probably a step in the anodic reaction. Chalcopyrite (dpeaa)DE-He213 CuCl (dpeaa)DE-He213 Free Energy Change (dpeaa)DE-He213 Extractive Metallurgy (dpeaa)DE-He213 Standard Free Energy Change (dpeaa)DE-He213 Fisher, W. W. aut Enthalten in JOM New York, NY : Springer Science + Business Media, 1989 33(1981), 2 vom: Feb., Seite 52-57 (DE-627)31368197X (DE-600)2002726-6 1543-1851 nnns volume:33 year:1981 number:2 month:02 pages:52-57 https://dx.doi.org/10.1007/BF03354527 lizenzpflichtig Volltext GBV_USEFLAG_A SYSFLAG_A GBV_SPRINGER AR 33 1981 2 02 52-57 |
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10.1007/BF03354527 doi (DE-627)SPR022666222 (SPR)BF03354527-e DE-627 ger DE-627 rakwb eng Wilson, J. P. verfasserin aut Cupric Chloride Leaching of Chalcopyrite 1981 Text txt rdacontent Computermedien c rdamedia Online-Ressource cr rdacarrier © The Minerals, Metals & Materials Society 1981 Abstract In a strong chloride solution the predominant cuprous, cupric, ferrous, and ferric chloride complexes are $ CuCl_{3} $−2, $ CuCl^{+} $, $ CuCl_{2} $, $ FeCl_{2} $, and $ FeCl_{2} $+ respectively. The probable dissolution reaction for chalcopyrite in cupric chloride solution is $ CuFeS_{2} $ + $ 3CuCl^{+} $ + $ 11Cl^{−2} $ = $ 4CuCl_{3} $−2 + $ FeCl_{2} $ + 2S The standard free energy change for this reaction at 25°C and unit activities is +43.84 kJ, indicating that the reaction is not thermodynamically feasible. The reaction becomes thermodynamically feasible at high chloride concentration when the ratio of cuprous to cupric copper in solution is less than about 1.9. When the cuprous to cupric ratio becomes larger than a critical value (dependent upon the operating conditions) the dissolution ceases because it is no longer thermodynamically feasible. Over the range 0.79–1.46 M $ Cu^{+2} $ and 2.82–6.21 M $ Cl^{−} $ at 90°C, neither cupric nor chloride ion concentration influences the rate of chalcopyrite dissolution, which is directly proportional to mineral surface area. The activation energy for the reaction is 134.7 kJ/mole, and the rate controlling process is probably a step in the anodic reaction. Chalcopyrite (dpeaa)DE-He213 CuCl (dpeaa)DE-He213 Free Energy Change (dpeaa)DE-He213 Extractive Metallurgy (dpeaa)DE-He213 Standard Free Energy Change (dpeaa)DE-He213 Fisher, W. W. aut Enthalten in JOM New York, NY : Springer Science + Business Media, 1989 33(1981), 2 vom: Feb., Seite 52-57 (DE-627)31368197X (DE-600)2002726-6 1543-1851 nnns volume:33 year:1981 number:2 month:02 pages:52-57 https://dx.doi.org/10.1007/BF03354527 lizenzpflichtig Volltext GBV_USEFLAG_A SYSFLAG_A GBV_SPRINGER AR 33 1981 2 02 52-57 |
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10.1007/BF03354527 doi (DE-627)SPR022666222 (SPR)BF03354527-e DE-627 ger DE-627 rakwb eng Wilson, J. P. verfasserin aut Cupric Chloride Leaching of Chalcopyrite 1981 Text txt rdacontent Computermedien c rdamedia Online-Ressource cr rdacarrier © The Minerals, Metals & Materials Society 1981 Abstract In a strong chloride solution the predominant cuprous, cupric, ferrous, and ferric chloride complexes are $ CuCl_{3} $−2, $ CuCl^{+} $, $ CuCl_{2} $, $ FeCl_{2} $, and $ FeCl_{2} $+ respectively. The probable dissolution reaction for chalcopyrite in cupric chloride solution is $ CuFeS_{2} $ + $ 3CuCl^{+} $ + $ 11Cl^{−2} $ = $ 4CuCl_{3} $−2 + $ FeCl_{2} $ + 2S The standard free energy change for this reaction at 25°C and unit activities is +43.84 kJ, indicating that the reaction is not thermodynamically feasible. The reaction becomes thermodynamically feasible at high chloride concentration when the ratio of cuprous to cupric copper in solution is less than about 1.9. When the cuprous to cupric ratio becomes larger than a critical value (dependent upon the operating conditions) the dissolution ceases because it is no longer thermodynamically feasible. Over the range 0.79–1.46 M $ Cu^{+2} $ and 2.82–6.21 M $ Cl^{−} $ at 90°C, neither cupric nor chloride ion concentration influences the rate of chalcopyrite dissolution, which is directly proportional to mineral surface area. The activation energy for the reaction is 134.7 kJ/mole, and the rate controlling process is probably a step in the anodic reaction. Chalcopyrite (dpeaa)DE-He213 CuCl (dpeaa)DE-He213 Free Energy Change (dpeaa)DE-He213 Extractive Metallurgy (dpeaa)DE-He213 Standard Free Energy Change (dpeaa)DE-He213 Fisher, W. W. aut Enthalten in JOM New York, NY : Springer Science + Business Media, 1989 33(1981), 2 vom: Feb., Seite 52-57 (DE-627)31368197X (DE-600)2002726-6 1543-1851 nnns volume:33 year:1981 number:2 month:02 pages:52-57 https://dx.doi.org/10.1007/BF03354527 lizenzpflichtig Volltext GBV_USEFLAG_A SYSFLAG_A GBV_SPRINGER AR 33 1981 2 02 52-57 |
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Cupric Chloride Leaching of Chalcopyrite |
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Abstract In a strong chloride solution the predominant cuprous, cupric, ferrous, and ferric chloride complexes are $ CuCl_{3} $−2, $ CuCl^{+} $, $ CuCl_{2} $, $ FeCl_{2} $, and $ FeCl_{2} $+ respectively. The probable dissolution reaction for chalcopyrite in cupric chloride solution is $ CuFeS_{2} $ + $ 3CuCl^{+} $ + $ 11Cl^{−2} $ = $ 4CuCl_{3} $−2 + $ FeCl_{2} $ + 2S The standard free energy change for this reaction at 25°C and unit activities is +43.84 kJ, indicating that the reaction is not thermodynamically feasible. The reaction becomes thermodynamically feasible at high chloride concentration when the ratio of cuprous to cupric copper in solution is less than about 1.9. When the cuprous to cupric ratio becomes larger than a critical value (dependent upon the operating conditions) the dissolution ceases because it is no longer thermodynamically feasible. Over the range 0.79–1.46 M $ Cu^{+2} $ and 2.82–6.21 M $ Cl^{−} $ at 90°C, neither cupric nor chloride ion concentration influences the rate of chalcopyrite dissolution, which is directly proportional to mineral surface area. The activation energy for the reaction is 134.7 kJ/mole, and the rate controlling process is probably a step in the anodic reaction. © The Minerals, Metals & Materials Society 1981 |
| abstractGer |
Abstract In a strong chloride solution the predominant cuprous, cupric, ferrous, and ferric chloride complexes are $ CuCl_{3} $−2, $ CuCl^{+} $, $ CuCl_{2} $, $ FeCl_{2} $, and $ FeCl_{2} $+ respectively. The probable dissolution reaction for chalcopyrite in cupric chloride solution is $ CuFeS_{2} $ + $ 3CuCl^{+} $ + $ 11Cl^{−2} $ = $ 4CuCl_{3} $−2 + $ FeCl_{2} $ + 2S The standard free energy change for this reaction at 25°C and unit activities is +43.84 kJ, indicating that the reaction is not thermodynamically feasible. The reaction becomes thermodynamically feasible at high chloride concentration when the ratio of cuprous to cupric copper in solution is less than about 1.9. When the cuprous to cupric ratio becomes larger than a critical value (dependent upon the operating conditions) the dissolution ceases because it is no longer thermodynamically feasible. Over the range 0.79–1.46 M $ Cu^{+2} $ and 2.82–6.21 M $ Cl^{−} $ at 90°C, neither cupric nor chloride ion concentration influences the rate of chalcopyrite dissolution, which is directly proportional to mineral surface area. The activation energy for the reaction is 134.7 kJ/mole, and the rate controlling process is probably a step in the anodic reaction. © The Minerals, Metals & Materials Society 1981 |
| abstract_unstemmed |
Abstract In a strong chloride solution the predominant cuprous, cupric, ferrous, and ferric chloride complexes are $ CuCl_{3} $−2, $ CuCl^{+} $, $ CuCl_{2} $, $ FeCl_{2} $, and $ FeCl_{2} $+ respectively. The probable dissolution reaction for chalcopyrite in cupric chloride solution is $ CuFeS_{2} $ + $ 3CuCl^{+} $ + $ 11Cl^{−2} $ = $ 4CuCl_{3} $−2 + $ FeCl_{2} $ + 2S The standard free energy change for this reaction at 25°C and unit activities is +43.84 kJ, indicating that the reaction is not thermodynamically feasible. The reaction becomes thermodynamically feasible at high chloride concentration when the ratio of cuprous to cupric copper in solution is less than about 1.9. When the cuprous to cupric ratio becomes larger than a critical value (dependent upon the operating conditions) the dissolution ceases because it is no longer thermodynamically feasible. Over the range 0.79–1.46 M $ Cu^{+2} $ and 2.82–6.21 M $ Cl^{−} $ at 90°C, neither cupric nor chloride ion concentration influences the rate of chalcopyrite dissolution, which is directly proportional to mineral surface area. The activation energy for the reaction is 134.7 kJ/mole, and the rate controlling process is probably a step in the anodic reaction. © The Minerals, Metals & Materials Society 1981 |
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Cupric Chloride Leaching of Chalcopyrite |
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