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Thermodynamics of the zinc-sulfur dioxide-water system

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Abstract

The known thermodynamic data for the aqueous zinc and sulfur dioxide systems have been gathered, evaluated, and presented in the form of potential -pH diagrams. Empirical relationships describing the entropy of ions at 298 K combined with the extrapolation method of Criss and Cobble[6] have been used in the absence of high-temperature free-energy data. The free energy of formation of zinc sulfite (ZnSO3 · 2.5H2O) has been experimentally determined to be −1256 ± 4 kJ mol−1 and has been incorporated into the diagrams along with the various metastable polythionate species of sulfur.

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Abbreviations

(i):

activity of speciesi

C o p :

standard molal heat capacity

C o p :

standard mean molal heat capacity

Eh :

potential of electrode referred to SHE

F:

the Faraday

ΔG o p :

standard free energy of formation of species

ΔG o :

standard free energy change of reaction

K :

equilibrium constant or solubility product

n :

number of electrons involved in reaction

R:

gas constant

S o 298 :

molal entropy of species in standard state at 298.15 K

SHE:

standard hydrogen electrode

T :

absolute temperature

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Author information

Authors and Affiliations

  1. Asamera Minerals U.S. Inc., 98807, Wentachee, WA

    D. M. Larsen (Chief Metallurgist)

  2. Department of Chemical Engineering, The University of Sydney, 2006, Sydney, New South Wales, Australia

    P. B. Linkson (Professor)

Authors
  1. D. M. Larsen
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  2. P. B. Linkson
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Larsen, D.M., Linkson, P.B. Thermodynamics of the zinc-sulfur dioxide-water system. Metall Trans B 24, 409–417 (1993). https://doi.org/10.1007/BF02666423

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