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The Nernst equation calculates the electrode potential of an electrochemical cell under non-standard conditions (non-unit concentrations). E = E° − (RT/nF) × ln(Q). At 25°C it simplifies to E = E° − (0.0592/n) × log(Q).

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1. 1E = E° − (0.0592/n) × log(Q) at 25°C
2. 2n = moles of electrons transferred
3. 3Q = reaction quotient (product of concentrations)
4. 4E > 0 means cell is spontaneous; E = 0 means equilibrium

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