Consider the following reversible reaction,A(g)+B(g)iffAB(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 reactionis 4 times that of the reverse reaction, the absolute value of DeltaG^(Theta) (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)

Consider the following reversible reaction,A(g)+B(g)iffAB(g)The activa

1.	Consider the following reversible reaction,A(g)+B(g)iffAB(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 reactionis 4 times that of the reverse reaction, the absolute value of DeltaG^(Theta) (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)
Answer» Solution :`A_((g))+B_((g))iffAB_((g))` `E_(ab)-E_(af)=2RT implies DeltaH=-2RT and (A_(f))/(A_(b))=4` `K_(EQ)=((K_(f))/(K_(b)))=(A_(f)e^(-E_(af)//RT))/(A_(b)e^(-E_(ab)//RT))=4(e^(2))` `DeltaG^(@)=-RTln K=-2500xxln(4xxe^(2))=-8500 J//mol` `THEREFORE` Absolute VALUE of `DeltaG^(@)=8500 J//mol`.