The value of the equilibrium constant for the following reaction at 300 K and constant pressure:
A(g) ⇌ B(g) + 2C(g); Δ E^° = -20.4 kcal and Δ S^° = -60 cal/K

Question

The value of the equilibrium constant for the following reaction at 300 K and constant pressure: A(g) ⇌ B(g) + 2C(g); Δ E ° = -20.4 kcal and Δ S ° = -60 cal/K

TestHub · Accepted Answer

Δ n g = 3 - 1 = 2 and take R = 2 cal/mol/K so RT = 600 cal/mol Δ H ° = Δ E ° + Δ n g RT = -20400 + 1200 = -19200 cal Δ G ° = Δ H ° - TΔ S ° = -19200 - 300(-60) = -1200 cal Δ G ° = -RTln K gives ln K = 1200/600 = 2 K = e 2 This is option (b).

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