The dissolution of low-iron sphalerite, (Zn,Fe)S containing 0.08% Fe, in ferric sulphate-sulphuric acid media was investigated using closely sized fractions of crushed sphalerite crystals and sintered disks made from the crushed crystals. Linear kinetics are observed, and the predominant reaction products are ZnSO_4, FeSO_4 and elemental sulphur. The leaching rate increases systematically with increasing temperature, and the calculated apparent activation energy is 56 kJ/mol for the sized sphalerite and 54 kJ/mol for the sintered disks. The relatively high apparent activation energy suggests that the rate is chemically controlled, a conclusion supported by the insensitivity of the rate to the disk rotation speed. The rate increases as the 0.22 power of the Fe(SO_4)_(1.5) concentration, and as the 0.22 power of the H_2SO_4 concentration. However, in the absence of ferric ions, the rate increases more significantly with increasing H_2SO_4 concentrations, and relatively rapid rates are observed in solutions containing >0.5 M H_2SO_4. In 0.1 M Fe(SO_4)_(1.5)-0.3 M H_2SO_4 media, the measured rate decreases with increasing sulphate concentrations, added as Li_2SO_4. The rate of dissolution of low-iron sphalerite is promoted by dissolved copper concentrations as high as 800 mg/L. In contrast, dissolved silver, even in the 0-2 mg/L concentration range, significantly retards the dissolution of the low-iron sphalerite.
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