Electrochemistry

At 300 K , the $E_{\text {cell }}^{\ominus}$ of

\(A(s)+B^{2+}(a q) \rightleftharpoons A^{2+}(a q)+B(s)\)

is 1.0 V . If $\Delta_r S^\theta$ of this reaction is $100 \mathrm{JK}^{-1}$. What is $\Delta_r H^{\ominus}$ (in $\mathrm{kJ} \mathrm{mol}^{-1}$ ) of this reaction?

\(\left(\mathrm{F}=96500 \mathrm{C} \mathrm{~mol}^{-1}\right)\)