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

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Both $\Delta H$ and $\Delta S$ are $(+ve)$

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(A) For a reaction to be spontaneous,the Gibbs free energy change $\Delta G$ must be negative,where $\Delta G = \Delta H - T \Delta S$.Given that the reaction is endothermic,$\Delta H > 0$ (positive).At low temperature (freezing point of water,$273 \ K$),the reaction is non-spontaneous,meaning $\Delta G > 0$. This implies $\Delta H > T \Delta S$.At high temperature (boiling point of water,$373 \ K$),the reaction is spontaneous,meaning $\Delta G For $\Delta G$ to become negative as temperature $T$ increases,$\Delta S$ must be positive. Thus,both $\Delta H$ and $\Delta S$ are positive.

Let us consider an endothermic reaction which is non-spontaneous at the freezing point of water. However,the reaction is spontaneous at the boiling point of water. Choose the correct option.

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