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Q.

The equilibrium concentrations of the species in the $A + B ⇌ C + D$ are 2,3,10 and 6molL^-1 , respectively at 300 K . $∆$ G₀ for the reaction is (R = 2cal/mol K)

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a

-137.26 cal

b

-13.73 cal

c

-1381.80 cal

d

1372.60 cal

answer is D.

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Detailed Solution

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$\begin{array}{l} Δ G = - 2.303 R T \log k_{eq} \\ Δ G = - 2.303 R T \log \frac{[C] [D]}{[A] [B]} \\ Δ G = - 2.303 \times 2 \times 300 \times \log \frac{10 \times 6}{2 \times 3} \\ Δ G = - 1381.80 cal \end{array}$

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The equilibrium concentrations of the species in the A+B⇌C+D are 2,3,10 and 6molL-1 , respectively at 300 K . ∆G0 for the reaction is (R = 2cal/mol K)