Consider the following reversible reaction. A(g)+B(g)→AB(g) The activation energy of the backward reaction exceeds that of the forward reaction by 2RT (Jmol−1). If the pre-exponential factor of the forward reaction is 4 times that of the reverse reaction, the absolute value of ΔGo (Jmol−1) for the reaction at 300 K is . (Given: ln2=0.7; RT=2500 Jmol−1 at 300 K; G is Gibbs energy)

Consider the following reversible reaction. A(g)+B(g)→AB(g) The acti

1.	Consider the following reversible reaction. A(g)+B(g)→AB(g) The activation energy of the backward reaction exceeds that of the forward reaction by 2RT (Jmol−1). If the pre-exponential factor of the forward reaction is 4 times that of the reverse reaction, the absolute value of ΔGo (Jmol−1) for the reaction at 300 K is . (Given: ln2=0.7; RT=2500 Jmol−1 at 300 K; G is Gibbs energy)
Answer» Consider the following reversible reaction. $A (g) + B (g) \to A B (g)$ The activation energy of the backward reaction exceeds that of the forward reaction by $2 R T (J m o l^{- 1})$ . If the pre-exponential factor of the forward reaction is 4 times that of the reverse reaction, the absolute value of $Δ G^{o} (J m o l^{- 1})$ for the reaction at $300 K$ is . $(G i v e n : l n 2 = 0.7; R T = 2500 J m o l^{- 1} at 300 K; G is Gibbs energy)$