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For the electrochemical cell reaction Cu2+(C1, aq) + Zn(s) → Zn2+(C2, aq) + Cu(s), the Gibbs free energy change, ΔG, at a fixed temperature depends on

1. ln(C1)
2. ln(C2/C1)
3. ln(C2)
4. ln(C1 + C2)

Correct answer: ln(C2/C1)

Solution

The Gibbs free energy change, ΔG, for an electrochemical reaction is related to the concentrations of the reactants and products through the Nernst equation, which shows that ΔG depends on the ratio of the concentrations of the products to the reactants, specifically ln(C2/C1) in this case.

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