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Calculate standard electrode potentials, equilibrium constants, and cell EMF under non-standard conditions using the Nernst equation.
Electrochemistry links chemical potential to electrical work via $\Delta G^\circ = -nFE^\circ_{cell}$.
$E_{cell} = E^\circ_{cell} - \frac{0.0591}{n} \log_{10} Q$. The most common student error is misidentifying $n$ (number of moles of electrons transferred in the balanced redox equation).
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