In which of the following conditions will a r | vedclass

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(D) For a reaction to be spontaneous,the Gibbs free energy change $\Delta G$ must be negative. The relationship is given by $\Delta G = \Delta H - T \

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$\Delta H = -ve, \Delta S = +ve$

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(D) For a reaction to be spontaneous,the Gibbs free energy change $\Delta G$ must be negative. The relationship is given by $\Delta G = \Delta H - T \cdot \Delta S$. If $\Delta H$ is negative (exothermic) and $\Delta S$ is positive (increase in entropy),then $\Delta G$ will be negative at all temperatures $T$ because both terms $\Delta H$ and $-T \cdot \Delta S$ will be negative.

In which of the following conditions will a reaction always be spontaneous at all temperatures?

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