A two-electron cell has $E^{\circ }=0.100\mathrm{V}$ at 298 K and ${\left(\frac{\partial E^{\circ }}{\partial T}\right)}_P=+4.0\times 10^{-4}\mathrm{V}{\mathrm{K}}^{-1}$. Taking $F=96500\mathrm{C}\mathrm{mo}{\mathrm{l}}^{-1}$, ${\Delta }_r{H}^{\circ }$ at 298 K and the nature of the cell reaction are

1. A$+3.71\mathrm{kJ}\mathrm{mo}{\mathrm{l}}^{-1}$; the reaction is endothermic but spontaneous because it is entropy-driven
2. B$-3.71\mathrm{kJ}\mathrm{mo}{\mathrm{l}}^{-1}$; the reaction is weakly exothermic
3. C$-42.31\mathrm{kJ}\mathrm{mo}{\mathrm{l}}^{-1}$; the reaction is strongly exothermic
4. D$-19.30\mathrm{kJ}\mathrm{mo}{\mathrm{l}}^{-1}$; the enthalpy equals the Gibbs energy for a galvanic cell