JEE Advanced 2018 · Paper 2, Chemistry question 13

Consider the following reversible reaction,

$$\mathrm{A(g) + B(g) \rightleftharpoons AB(g)}.$$

The activation energy of the backward reaction exceeds that of the forward reaction by $2RT$ (in J mol$^{-1}$). If the pre-exponential factor of the forward reaction is 4 times that of the reverse reaction, the absolute value of $\Delta G^\ominus$ (in J mol$^{-1}$) for the reaction at 300 K is ____.

(Given; ln(2) = 0.7, $RT$ = 2500 J mol$^{-1}$ at 300 K and $G$ is the Gibbs energy)