The value of ${\log }_{10}\mathrm{K}$ for a reaction $A\rightleftharpoons B$ is :

{Given : ${\mathrm{\Delta }}_{\mathrm{r}}{\mathrm{H}}_{298\mathrm{K}}^{\circ }=-54.07\mathrm{kJ} {\mathrm{mol}}^{-1}, {\mathrm{\Delta }}_{\mathrm{r}}{\mathrm{S}}_{298\mathrm{K}}^{\circ }=10 {\mathrm{JK}}^{-1}{\mathrm{mol}}^{-1}$ and $\mathrm{R}=8.314{\mathrm{JK}}^{-1}{\mathrm{mol}}^{-1}; 2.303\times 8.314\times 298=5705\text{ ) }$