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 2 RT (in J mol-1). If the pre-exponential factor of the forward  reaction is times that of the reverse reaction, the absolute value of G  ( in J mol-1) for the reaction at 300K is.................                     (Given; ln(2)=0.7 RT =2500J mol-1 at 300K and G is the Gibbs energy )


A) 7500 J/mol

B) 8500 J/mol

C) 6500 J/mol

D) 7000 J/mol

Answer:

Option B

Explanation:

 For the reaction,

 A(g)+B(g)AB(g)

 Given Eab=Eaf+2RT

EabEaf=2RT

 Further, Af=4Ab      or    AfAb=4

   Now, rate constant for forward reaction,

  kf=AfeEafRT

 Like wise, rate constant for backward reaction

 kb=AbeEabRT

At equillibrium,  Rate of forward reaction = Rate of backward reaction

 ie., kf=kb

or   kfkb=keq

 So,  keq=AfeEafRTAbeEabRT

  =   AfAbe(EafEab)RT

 After putting the given values,  keq=4e2

 (as   EabEaf=2RT  and       AfAb=4 )

  Now,

Δ G0 = -RT ln Keq

= -2500 ln(4 e2)

= -2500 (ln 4 +ln e2 )

= -2500 (1.4 +2)

= -2500 × 3.4

= -8500 J/mol

Absolute value = 8500 J/mol