standard electromotive force

Quantity defined by $E ° = − Δ r G ° n F = R T n F ln K °$ , where $Δ r G °$ is the standard Gibbs energy of the cell reaction in the direction in which reduction occurs at the right-hand electrode in the diagram representing the cell ('reduction at right'), $K °$ is the standard equilibrium constant for this reaction, $n$ its charge number, $F$ the Faraday constant, $R$ the gas constant and $T$ the thermodynamic temperature.

Source:

Green Book, 2nd ed., p. 58

Interactive Link Maps
First Level	Second Level	Third Level

Cite as:
IUPAC. Compendium of Chemical Terminology, 2nd ed. (the "Gold Book"). Compiled by A. D. McNaught and A. Wilkinson. Blackwell Scientific Publications, Oxford (1997). XML on-line corrected version: http://goldbook.iupac.org (2006-) created by M. Nic, J. Jirat, B. Kosata; updates compiled by A. Jenkins. ISBN 0-9678550-9-8. https://doi.org/10.1351/goldbook.

Last update: 2014-02-24; version: 2.3.3.

DOI of this term: https://doi.org/10.1351/goldbook.S05913.

Original PDF version: http://www.iupac.org/goldbook/S05913.pdf. The PDF version is out of date and is provided for reference purposes only. For some entries, the PDF version may be unavailable.

Current PDF version | Version for print | History of this term

PREVIOUS	S05913	NEXT
standard electrode potential, $E °$		standard entropy of activation, $Δ ‡ S °$ , $Δ ‡ S$