Abstract
Redox reactions are usually described by a disguised form of equilibrium constant called the standard cell potential. It is directly proportional to the log of the K °eq . A system of hypothetical half-cell potentials is based on the standard hydrogen electrode. The Nernst equation relates cell potentials to the log of activities involved and to the K °eq . For a reaction to which a net change in oxidation states n applies,
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Notes
J. O. Bockris and A. K. N. Reddy, Modern Electrochemistry, Plenum Press, New York, 1970, Vol. II, pp. 1115–1120.
R. M. Garrels and C. L. Christ, Solutions, Minerals, and Equilibria, Harper and Row, New York, 1965, Chapters 7 and 11.
W. Stumm and J. J. Morgan, Aquatic Chemistry, Wiley-Interscience, New York, 1970, Chapters 7 and 10.
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© 1975 Plenum Press, New York
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Guenther, W.B. (1975). Oxidation—Reduction. In: Chemical Equilibrium. Springer, Boston, MA. https://doi.org/10.1007/978-1-4684-2163-7_12
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DOI: https://doi.org/10.1007/978-1-4684-2163-7_12
Publisher Name: Springer, Boston, MA
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