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(A) For a reaction to be spontaneous,the Gibbs free energy change must be negative,i.e.,$\Delta G = \Delta H - T\Delta S < 0$. Given that the reaction

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

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(A) For a reaction to be spontaneous,the Gibbs free energy change must be negative,i.e.,$\Delta G = \Delta H - T\Delta S Given that the reaction is spontaneous below equilibrium temperature $(T If $\Delta H For $\Delta G  |T\Delta S|$,which implies $T Since both $\Delta H$ and $\Delta S$ are negative,the ratio $\frac{\Delta H}{\Delta S}$ is positive,representing the equilibrium temperature. Thus,the reaction is spontaneous when $T$ is less than this equilibrium temperature.

Identify from the following the correct set of thermodynamic conditions for the reaction to be spontaneous below equilibrium temperature.

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