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(C) The spontaneity of a reaction is determined by the Gibbs free energy change,given by the equation: $\Delta G = \Delta H - T\Delta S$. For a reacti

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$\Delta H  0$

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(C) The spontaneity of a reaction is determined by the Gibbs free energy change,given by the equation: $\Delta G = \Delta H - T\Delta S$. For a reaction to be spontaneous at all temperatures,$\Delta G$ must be negative $(\Delta G If $\Delta H  0$ (increase in entropy),then $\Delta G$ will always be negative regardless of the temperature $T$,because both terms ($\Delta H$ and $-T\Delta S$) will contribute to a negative value. Therefore,the correct condition is $\Delta H  0$.

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

Similar Questions

For vaporization of water at $1$ atmospheric pressure,the values of $\Delta H$ and $\Delta S$ are $40.63 \ kJ \ mol^{-1}$ and $108.8 \ J \ K^{-1} \ mol^{-1},$ respectively. The temperature when Gibb's energy change $(\Delta G)$ for this transformation will be zero,is ............ $K$. (in $.4$)

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