Consider the following reaction :2A (g) + B ( | vedclass

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(A) For the reaction $2A(g) + B(g) \rightarrow 2D(g)$, the change in the number of gaseous moles is $\Delta n_g = 2 - (2 + 1) = -1$.We know the relati

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$+ 0.636 	ext{ kJ mol}^{-1}$, non-spontaneous

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(A) For the reaction $2A(g) + B(g) ightarrow 2D(g)$, the change in the number of gaseous moles is $\Delta n_g = 2 - (2 + 1) = -1$.We know the relation $\Delta H^{\circ} = \Delta U^{\circ} + \Delta n_g RT$.Substituting the values: $\Delta H^{\circ} = -10 	imes 10^3 	ext{ J mol}^{-1} + (-1) 	imes 8.31 	ext{ J K}^{-1} 	ext{ mol}^{-1} 	imes 298 	ext{ K} = -10000 - 2476.38 = -12476.38 	ext{ J mol}^{-1} = -12.476 	ext{ kJ mol}^{-1}$.Now, we use the Gibbs free energy equation: $\Delta G^{\circ} = \Delta H^{\circ} - T\Delta S^{\circ}$.$\Delta G^{\circ} = -12.476 	ext{ kJ mol}^{-1} - 298 	ext{ K} 	imes (-44 	imes 10^{-3} 	ext{ kJ K}^{-1} 	ext{ mol}^{-1}) = -12.476 + 13.112 = +0.636 	ext{ kJ mol}^{-1}$.Since $\Delta G^{\circ} > 0$, the reaction is non-spontaneous.

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