The standard Gibbs free energy change for the reaction is per mole of reaction as written

CHEMISTRY · Subjective · AP · Chemistry · Thermodynamics and Electrochemistry · Thermodynamics and Electrochemistry

Problem

The standard Gibbs free energy change for the reaction

\mathrm{Cu}^{2+}(\mathrm{aq}) + 2\,\mathrm{Cl}^{-}(\mathrm{aq}) \rightarrow \mathrm{Cu}(s) + \mathrm{Cl}_2(g)

\Delta G^\circ = +1.30 \times 10^2\,\text{kJ}

per mole of reaction as written. If

2\,\text{mol}\, e^{-}

are transferred, determine the minimum cell potential (in V) that must be applied at

298\,\text{K}

to make this reaction occur. (Faraday constant

F = 9.6485 \times 10^4\,\text{C mol}^{-1}\, e^{-}