The value of log K for the reaction A ⇌ B at 298 K is ____. (Nearest integer) Given: Δ H^°=-54.07 kJ mol^-1 Δ S^°=10 JK^-1 mol^-1 ( Take 2.303 ×…

The value of $\displaystyle \log \mathrm{K}$ for the reaction $\displaystyle \mathrm{A} \rightleftharpoons \mathrm{B}$ at $\displaystyle 298$ K is $\displaystyle \_\_\_\_$. (Nearest integer) Given: $\displaystyle \Delta \mathrm{H}^{\circ}=-54.07 \mathrm{~kJ} \mathrm{~mol}^{-1}$ $$\Delta \mathrm{S}^{\circ}=10 \mathrm{JK}^{-1} \mathrm{~mol}^{-1} $$ $\displaystyle ($ Take $\displaystyle 2.303 \times 8.314 \times 298=5705)$