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