Thermodynamic modeling of phase formation conditions in the system CuO–CO2–H2O–NH3

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Аннотация

Phase formation in the CuO–CO2–H2O–NH3 system has been studied using thermodynamic modelling in the temperature range of 20–100°C, рo = 0.1 MPa and ammonia concentrations of 0, 0.01 and 2.0 mol/kg. The stability fields of tenorite [CuO], malachite [Cu2CO3(OH)2], azurite [Cu3(CO3)2(OH)2] were determined and the compositions of the solutions in equilibrium with the solid phases were calculated. The effect of temperature and ammonia concentration on the change in phase relations in the system was shown. It was found that during the interaction of tenorite, malachite and azurite with ammonia solutions 1.0–3.0 mol/kg, the copper content in the solution increased with increasing ammonia concentration and decreased with increasing temperature. The results presented provide a basis for understanding the mechanism of mineral formation in aqueous copper-carbonate systems, as well as for solving a number of environmental problems and developing technological processes for ammonia leaching.

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Авторлар туралы

T. Bublikova

Korzhinskii Institute of Experimental Mineralogy of the Russian Academy of Sciences

Хат алмасуға жауапты Автор.
Email: tmb@iem.ac.ru
Ресей, Chernogolovka, 142432

T. Setkova

Korzhinskii Institute of Experimental Mineralogy of the Russian Academy of Sciences

Email: tmb@iem.ac.ru
Ресей, Chernogolovka, 142432

V. Balitsky

Korzhinskii Institute of Experimental Mineralogy of the Russian Academy of Sciences

Email: tmb@iem.ac.ru
Ресей, Chernogolovka, 142432

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3. Fig. 1. Solubility isothermal diagrams of compounds in the CuO–CO2–H2O system: t = 25, 50, 75, 100°C; p = 0.1 MPa; Tnr – tenorite, Mlc – malachite, Azu – azurite; 1 – partial pressure of CO2 under atmospheric conditions; 2 – CO2 content in rainwater [1].

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4. Fig. 2. Concentration of copper particles in a solution in equilibrium with solid phases of the CuO–CO2–H2O system, depending on pH; t = 25 (a), 100°C (b); p = 0.1 MPa.

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5. Fig. 3. Solubility isothermal diagrams of compounds in the CuO–CO2–H2O–NH3 system: CNH3 = 0.01 mol/kg; t = 25 (a), 100°C (b); p = 0.1 MPa.

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6. Fig. 4. Concentration of aqueous particles and copper complexes in a solution in equilibrium with solid phases of the CuO–CO2–H2O–NH3 system, depending on pH. CNH3 = 0.01 mol/kg; t = 25 (a), 100°C (b); p = 0.1 MPa.

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7. Fig. 5. Dependence of copper concentration in solution on temperature during dissolution of tenorite (Tnr) and malachite (Mlc) in a 0.01 m NH3 solution.

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8. Fig. 6. Ratio of solid phases in the process of incongruent dissolution of malachite (Mlc) in a 0.01 m NH3 solution.

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9. Fig. 7. Solubility isothermal diagrams of compounds in the CuO–CO2–H2O–NH3 system. СNH3 = 2.0 mol/kg; t = 25 (a), 100°С (b); р = 0.1 MPa.

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10. Fig. 8. Concentration of aqueous particles and copper complexes in a solution in equilibrium with solid phases of the CuO–CO2–H2O–NH3 system depending on pH. СNH3 = 2.0 mol/kg; t = 25 (a), 100°С (b); р = 0.1 MPa.

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11. Fig. 9. Dependence of copper concentration in solution on temperature during dissolution: a – tenorite, b – malachite, c – azurite in solutions of 1.0 (1), 2.0 (2), 3.0 m NH3 (3). Black triangles in Fig. 9b are experimental data from [9].

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12. Fig. 10. Ratio of solid phases in the process of incongruent dissolution: a – malachite (Mlc); b – azurite (Azu) in solutions of 1.0 (1), 2.0 (2), 3.0 m NH3 (3).

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