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(D) The spontaneity of a reaction is determined by the Gibbs free energy equation: $\Delta G = \Delta H - T\Delta S$. For a reaction to be non-spontan

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

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(D) The spontaneity of a reaction is determined by the Gibbs free energy equation: $\Delta G = \Delta H - T\Delta S$. For a reaction to be non-spontaneous,$\Delta G$ must be greater than $0$ $(\Delta G > 0)$. If $\Delta H > 0$ (endothermic) and $\Delta S Since $T$ is always positive in Kelvin,$\Delta G$ will always be positive regardless of the temperature. Therefore,the reaction is non-spontaneous at all temperatures when $\Delta H > 0$ and $\Delta S < 0$.

Identify from the following the correct set of thermodynamic conditions for the reaction to be non-spontaneous at all temperatures.

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