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Which equation correctly expresses the relationship between standard Gibbs free energy change and the equilibrium constant?

1. Ecell = E° - RT/nF ln Q
2. At equilibrium, Ecell = 0 and Q = Kc
3. E° = RT/nF ln K
4. ΔG° = -nFE° = -RT ln K

Correct answer: ΔG° = -nFE° = -RT ln K

Solution

The correct relation between free energy change and equilibrium constant is ΔG° = -RT ln K, which is derived from thermodynamic principles and the Nernst equation.

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