A reaction at 300 K with ΔGo = −1743 J consists of 3 moles of A(g), 6 moles of B(g) and 3 moles of C

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A reaction at 300 K with ΔGo = −1743 J consists of 3 moles of A(g), 6 moles of B(g) and 3 moles of C(g). If A, B and C are in equilibrium in one liter vessel, then the reaction should be (ln 2 = 0.7, R = 8.3 J/K-mol)

Accepted Answer

$\Delta G^{o} = - RT.\ln K_{eq}$$\Rightarrow - 1743 = - 8.3t300 	imes \ln K_{eq} $$${	herefore K_{eq} = 2 }{	ext{Now, }(a)K_{eq} = \frac{3}{3 	imes 6}(b)K_{eq} = \frac{6 	imes 3^{2}}{3} }{(c)K_{eq} = \frac{6 	imes 3}{3^{2}}(d)K_{eq} = \frac{3^{2}}{3 	imes 6}}$$

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