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   mol - 1 ). If the pre-exponential factor of the forward reaction is 4 times that of the reverse reaction,…

Question

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

{mol}^{- 1}

). If the pre-exponential factor of the forward reaction is

4

times that of the reverse reaction, the absolute value of

∆ G^{⊝} (in J {mol}^{- 1})

for the reaction at

300 K

is ____.
(Given;

\ln (2) = 0 .7, = 2500 J {mol}^{- 1} at 300 K

and

G

is the Gibbs energy)

Aicharya · Accepted Answer

A &#160; g + B &#160; g &#8652; AB &#160; g E ab - E ef = 2 RT &#160; &#8658; &#8710; H = - 2 RT &#160; and A f A b = 4 K eq = K f K b = A f &#160; e - E af / RT A b e - E ab / RT = 4 e 2 &#8710; G o = - RTln &#8289; K = - 2500 &#215; ln &#8289; 4 &#215; e 2 = - 8500 J / mol &#8756; &#160; &#160; Absolute value of &#8710; G o - 8500 &#160; J / mol

Consider the following reversible reaction: A   g + B   g ⇌ AB   g The activation…

Solution

Consider the following reversible reaction: A &#160; g + B &#160; g &#8652; AB &#160; g The activation…

Solution

Consider the following reversible reaction: A g + B g ⇌ AB g The activation…