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(B) For a reaction to be spontaneous,the Gibbs free energy change $\Delta G$ must be negative,where $\Delta G = \Delta H - T\Delta S$. For the reactio

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

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(B) For a reaction to be spontaneous,the Gibbs free energy change $\Delta G$ must be negative,where $\Delta G = \Delta H - T\Delta S$. For the reaction to be spontaneous at high temperature,the term $T\Delta S$ must be large and positive to make $\Delta G$ negative,even if $\Delta H$ is positive. This requires $\Delta S > 0$ and $\Delta H > 0$. Thus,when $\Delta H > 0$ and $\Delta S > 0$,the reaction becomes spontaneous at high temperatures where $T\Delta S > \Delta H$.

Which of the following set of thermodynamic conditions is true for the reaction to be spontaneous at high temperature?

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