The activation energies for the forward and reverse elementary reactions in the system: A ⇌ B, are 10.303 and 8.000 kcal, respectively, at 500 K. Assuming the pre-exponential factor to be the same for

Question

The activation energies for the forward and reverse elementary reactions in the system: A ⇌ B, are 10.303 and 8.000 kcal, respectively, at 500 K. Assuming the pre-exponential factor to be the same for both the forward and reverse steps, the equilibrium constant of the reaction at 500 K is

Prashant Kotian · Accepted Answer

Correct answer: D. ΔH = E_a(forward) - E_a(reverse) = 10.303 - 8.000 = +2.303 kcal/mol. Since the pre-exponential factors are equal, K = e^(-ΔH / RT) = e^(-2303 cal / (2 cal/K·mol × 500 K)) = e^(-2303 / 1000) = e^(-2.303) = 10⁻¹ = 0.1. Therefore, correct answer is D.

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