The standard electrode potential $E^{\circ}$ and its temperature coefficient $\left(\frac{d E^{\circ}}{d T}\right)$ for a cell are $2 V$ and $-5 \times 10^{-4} V K^{-1}$ at 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 ( $\Delta_{\mathrm{r}} \mathrm{H}^{\circ}$ ) at $300 \mathrm{~K} \mathrm{in} \mathrm{kJ} \mathrm{mol}^{-1}$ is, $\left[\right.$ Use $\mathrm{R}=8 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}$ and $\left.\mathrm{F}=96,000 \mathrm{C} \mathrm{mol}^{-1}\right]$