The standard electrode potential E^ and its temperature coefficient ((dE^)/dT) for a cell are 2 V and -5 × 10^-4 VK^-1 at 300 K respectively. The…

The standard electrode potential $\displaystyle \mathrm{E}^{\ominus}$ and its temperature coefficient $\displaystyle \left(\frac{\mathrm{dE}^{\ominus}}{\mathrm{dT}}\right)$ for a cell are $\displaystyle 2$ V and $\displaystyle -5 \times 10^{-4} \mathrm{VK}^{-1}$ at $\displaystyle 300$ K respectively. The cell reaction is $$\mathrm{Zn}(\mathrm{~s})+\mathrm{Cu}^{2+}(\mathrm{aq}) \rightarrow \mathrm{Zn}^{2+}(\mathrm{aq})+\mathrm{Cu}(\mathrm{~s}) $$ The standard reaction enthalpy $\displaystyle \left(\Delta_{\mathrm{r}} \mathrm{H}^{\ominus}\right)$ at $\displaystyle 300 \mathrm{~K}$ in $\displaystyle \mathrm{kJ} \mathrm{~mol}^{-1}$ is, [Use $\displaystyle \mathrm{R}=8 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}$ and $\displaystyle \mathrm{F}=96,000 \mathrm{Cmol}^{-1}$ ]