The standard electrode potential

The standard electrode potential $\mathrm{E}^{\ominus}$ and its

temeprature coefficient $\left(\frac{\mathrm{dE}^{\ominus}}{\mathrm{dT}}\right)$ for a cell are $2 \mathrm{~V}$

and $-5 \times 10^{-4} \mathrm{VK}^{-1}$ at $300 \mathrm{~K}$ 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 $\left(\Delta_{r} \mathrm{H}^{\ominus}\right)$ at 300

$\mathrm{K}$ in $\mathrm{kJ} \mathrm{mol}^{-1}$ is,

$\left[\right.$ Use $\mathrm{R}=8 \mathrm{jK}^{-1} \mathrm{~mol}^{-1}$ and $\left.\mathrm{F}=96,000 \mathrm{Cmol}^{-1}\right]$