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(A) The reaction $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$ involves the dissociation of one mole of gas into two moles of gas,which leads

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$\Delta H > 0$ and $\Delta S > 0$

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(A) The reaction $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$ involves the dissociation of one mole of gas into two moles of gas,which leads to an increase in entropy,so $\Delta S > 0$.Since bond breaking is an endothermic process,the enthalpy change is positive,so $\Delta H > 0$.For a reaction to be spontaneous,the Gibbs free energy change $\Delta G = \Delta H - T\Delta S$ must be negative.At high temperatures,the term $T\Delta S$ becomes large and positive,making $\Delta G$ negative when $\Delta H > 0$ and $\Delta S > 0$.

For the reaction occurring in the gaseous phase: $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$,which of the following conditions is correct for the reaction to be spontaneous at high temperatures?

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