Thermodynamics

The value of \(\log \mathrm{K}\) for the reaction \(\mathrm{A} \rightleftharpoons \mathrm{B}\) at \(298 \mathrm{~K}\) is ___________. (Nearest integer)

Given: \(\Delta \mathrm{H}^{\circ}=-54.07 \mathrm{~kJ} \mathrm{~mol}^{-1}\)

\(\Delta \mathrm{S}^{\circ}=10 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\)

(Take \(2.303 \times 8.314 \times 298=5705\) )