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

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

Given: \(\Delta H ^0=-54.07 \mathrm{~kJ mol ^{-1}}\)
\(\Delta S ^{\circ}=-10 \mathrm{~JK ^{-1} mol ^{-1}}\)
\((\) Take \(2.303 \times 8.314 \times 298=5705\))