The standard Gibbs energy for the given cell reaction in kJ mol^-1 at 298 K is: Zn ( s )+ Cu^2+( aq ) → Zn^2+( aq )+ Cu ( s ), E^°=2 V at 298 K…

The standard Gibbs energy for the given cell reaction in $\displaystyle \mathrm{kJ} \mathrm{mol}^{-1}$ at $\displaystyle 298$ K is : $$\begin{aligned} & \mathrm{Zn}(\mathrm{~s})+\mathrm{Cu}^{2+}(\mathrm{aq}) \rightarrow \mathrm{Zn}^{2+}(\mathrm{aq})+\mathrm{Cu}(\mathrm{~s}), \\ & \mathrm{E}^{\circ}=2 \mathrm{~V} \text { at } 298 \mathrm{~K} \end{aligned} $$ (Faraday's constant, $\displaystyle \mathrm{F}=96000 \mathrm{C} \mathrm{mol}^{-1}$ )