For the reaction x + y rightarrow z,the proce | vedclass

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

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$\Delta H  0$

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(B) For a reaction to be spontaneous,the Gibbs free energy change $\Delta G$ must be negative,where $\Delta G = \Delta H - T \Delta S$. Since the forward reaction is spontaneous at room temperature,$\Delta H$ must be negative and $\Delta S$ must be positive for $\Delta G$ to be negative at low temperatures. Conversely,for the reverse reaction to be spontaneous at high temperatures,the conditions must favor the reverse process,confirming $\Delta H  0$.

For the reaction $x + y \rightarrow z$,the process is spontaneous at room temperature,and the reverse reaction is spontaneous at high temperature. Which of the following is true?

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