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A mixed surface reaction kinetic model for the reductive leaching of manganese dioxide with acidic sulfur dioxide
Journal article   Peer reviewed

A mixed surface reaction kinetic model for the reductive leaching of manganese dioxide with acidic sulfur dioxide

G. Senanayake
Hydrometallurgy, Vol.73(3-4), pp.215-224
2004
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Abstract

Previous researchers have rationalised the kinetics of dissolution of manganese dioxide in acidic sulfur dioxide solutions on the basis of either the adsorption of reactants followed by reactions with HSO3- and SO2 or a two-electron surface electrochemical reaction with H+ and HSO3-, the species involved in the equilibrium: SO2(aq)+H2O=H++HSO 3-. This paper revisits the reported rate data for the dissolution of MnO2 in the form of plates [Herring and Ravitz, Trans. SME/AIME 231 (1965) 191] or particles [Miller and Wan, Hydrometallurgy 10 (1983) 219] to show that the rate of dissolution can be rationalised on the basis of a fast redox reaction: (i) MnO2(s)+SO2(aq)+H 2O=MnOOH(s)+HSO3(aq) followed by one of the two rate determining redox reactions: (ii) MnOOH(s)+HSO3(aq) = MnSO 40(aq)+H2O or Mn(OH)HSO4(s), (iii) MnOOH(s)+SO2(aq) = MnO(s)+HSO3(aq) depending on the pH of the medium. Whilst the rate equation for (iii) agrees with the electrochemical kinetic model reported previously, the dissolution of the solid Mn(OH)HSO 4 or the direct reaction: (iv) MnO2(s)+SO2(aq) = MnSO40(aq) also appear to be rate controlling. The two rate constants k1 and k2 based on a shrinking sphere kinetic model: 1-(1-X)1/3 = k1K0.5[SO 2]0.5(t/rρ)+k2[SO2](t/rρ), for the leaching of monosized pyrolusite and electrolytically prepared MnO 2 particles, are in reasonable agreement with k1 and k2 based on the dissolution kinetics of MnO2 plates.

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Citation topics
7 Engineering & Materials Science
7.229 Mineral & Metal Processing
7.229.774 Bioleaching
Web Of Science research areas
Metallurgy & Metallurgical Engineering
ESI research areas
Materials Science
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