Nernst equation derivation from "summary" of Physical Chemistry by Robert G. Mortimer
To derive the Nernst equation, we begin with the fundamental equation for the Gibbs energy change of a cell reaction. This equation relates the standard Gibbs energy change to the equilibrium constant of the cell reaction. By using the relationship between the standard Gibbs energy change and the cell potential, we can derive the Nernst equation. The standard Gibbs energy change of a cell reaction is related to the standard cell potential by the equation ΔG° = -nFΔE°, where n is the number of moles of electrons transferred in the reaction and F is Faraday's constant. This equation allows us to calculate the standard Gibbs energy change of a cell reaction from the standard cell potential. The equilibrium constant of a cell reaction, K, is related to the standard Gibbs energy change by the equation ΔG° = -RTlnK, where R is the gas constant and ...
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