Chemistry - Electrochemistry Question with Solution | TestHub

The standard Gibbs free energy change is related to the standard cell potential by the equation $\Delta {\mathrm{G}}^{\circ }=-\mathrm{nF}{\mathrm{E}}_{\text{cell}}^{\circ }$.

Rearranging this equation gives ${\mathrm{E}}_{\text{cell}}^{\circ }=-\frac{\Delta {\mathrm{G}}^{\circ }}{\mathrm{nF}}$.

The relation given in the option is missing the negative sign, making it false.

The other relations are correct standard formulas:
${\mathrm{E}}_{\text{cell}}^{\circ }={\mathrm{E}}_{\text{cathode}}^{\circ }-{\mathrm{E}}_{\text{anode}}^{\circ }$
${\mathrm{E}}_{\text{cell}}^{\circ }={\mathrm{E}}_{\text{right}}^{\circ }-{\mathrm{E}}_{\text{left}}^{\circ }$
${\mathrm{E}}_{\text{cell}}^{\circ }=\frac{0.0592}{\mathrm{n}}{\log }_{10}\mathrm{K}$ (at $298\text{ K}$)

Answer: ${\mathrm{E}}_{\text{cell }}^{\circ }=\frac{\Delta {\mathrm{G}}^{\circ }}{\mathrm{nF}}$