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Oxidation—Reduction

  • William B. Guenther

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,
$$aA + bB + \cdots \rightleftharpoons xX + yY + \cdots E = {E^ \circ } - \frac{{0.05916}}{n}\log \frac{{{{(X)}^x}{{(Y)}^y} \cdots }}{{{{(A)}^a}{{(B)}^b} \cdots }}$$
(12-1)

Keywords

Cell Potential Nernst Equation Standard Hydrogen Electrode Ferric Chloride Solution Sulfur System 
These keywords were added by machine and not by the authors. This process is experimental and the keywords may be updated as the learning algorithm improves.

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Notes

  1. 1.
    J. O. Bockris and A. K. N. Reddy, Modern Electrochemistry, Plenum Press, New York, 1970, Vol. II, pp. 1115–1120.Google Scholar
  2. 2.
    R. M. Garrels and C. L. Christ, Solutions, Minerals, and Equilibria, Harper and Row, New York, 1965, Chapters 7 and 11.Google Scholar
  3. 3.
    W. Stumm and J. J. Morgan, Aquatic Chemistry, Wiley-Interscience, New York, 1970, Chapters 7 and 10.Google Scholar

Copyright information

© Plenum Press, New York 1975

Authors and Affiliations

  • William B. Guenther
    • 1
  1. 1.Department of ChemistryThe University of the SouthSewaneeUSA

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