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Q.

Consider the following reversible reaction A (g)+B (g) $⇌$ AB (g). The activation Energy of backward reaction exceeds than that of forward reaction by 2RT (in joule $m o l e^{- 1}$ ). If the Pre exponential factor of forward reaction is 4 times than that of reverse reaction and the value of $Δ G^{0}$ for the reaction at 300 K is approx. - $0.85 \times 10^{x}$ joule. Find out the value of x?

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Detailed Solution

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$A (g) + B (g) ⇌ A B (g) E a (b) - E a (f) = 2 R T \frac{A f}{A b} = 4 Δ G^{o} = - R T \ln K_{e q} . \frac{K_{f}}{K_{b}} = K_{e q} . k e q = \frac{A_{f}}{A_{b}} . e^{2} = 4 e^{2} Δ G^{o} = - R T \ln K_{e q} = - R T l m (4 e^{2}) - 8500 J o u l e - 0.85 \times 10^{4} J o u l e$

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