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Nernst equation
In electrochemistry, the Nernst equation gives the electrode potential (E), relative to the standard electrode potential, (E0), of the electrode couple or, equivalently, of the half cells of a battery
At room temperature the following is true
![E = E^0 - \frac{0.0591}{n} \log\frac{[\mbox{red}]}{[\mbox{ox}]}](a/../upload/math/a85ea4fc8a5f28c317a15d72586fd77f.png)
- R is the universal gas constant, equal to 8.314570 J K-1 mol-1
- T the temperature in kelvins
- a the chemical activities on the reduced and oxidized side, respectively
- F is the Faraday constant, equal to 96,485 C mol-1
- n is the number of electrons transferred in the half-reaction.
- [red] is the concentration of oxidizing agent (the reduced species).
- [ox] is the concentration of reducing agent (the oxidized species).
History
The Nernst equation is named after the German physical chemist Walther Nernst who first formulated it.
See also
- Electrodiffusion .
10-26-2009 08:16:03
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The contents of this article is licensed from www.wikipedia.org under the GNU Free Documentation License. Click here to see the transparent copy and copyright details