For the cell reaction Cu^{2+}_{(C_1, aq)} + Z | vedclass

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(D) The Nernst equation for the given cell reaction is $E_{cell} = E^o_{cell} - \frac{RT}{nF} \ln \frac{[Zn^{2+}]}{[Cu^{2+}]} = E^o_{cell} - \frac{RT}

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ln $(C_2 / C_1)$

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(D) The Nernst equation for the given cell reaction is $E_{cell} = E^o_{cell} - \frac{RT}{nF} \ln \frac{[Zn^{2+}]}{[Cu^{2+}]} = E^o_{cell} - \frac{RT}{nF} \ln \frac{C_2}{C_1}$.The relationship between Gibbs free energy change and cell potential is given by $\Delta G = -nF E_{cell}$.Substituting the expression for $E_{cell}$,we get $\Delta G = -nF \left( E^o_{cell} - \frac{RT}{nF} \ln \frac{C_2}{C_1} \right) = -nF E^o_{cell} + RT \ln \frac{C_2}{C_1}$.Thus,the change in free energy $\Delta G$ is a function of $\ln \left( \frac{C_2}{C_1} \right)$.

For the cell reaction $Cu^{2+}_{(C_1, aq)} + Zn_{(s)} \rightarrow Zn^{2+}_{(C_2, aq)} + Cu_{(s)}$ of an electrochemical cell,the change in free energy at a given temperature is a function of

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