(C) For a reaction to be spontaneous, $\Delta G < 0$. Since $\Delta G = \Delta H - T\Delta S$, the condition for spontaneity is $\Delta H - T\Delta S

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(C) For a reaction to be spontaneous, $\Delta G Since $\Delta G = \Delta H - T\Delta S$, the condition for spontaneity is $\Delta H - T\Delta S Given: $\Delta H = -400 \text{ kJ mol}^{-1}$ and $\Delta S = -20 \text{ kJ mol}^{-1} \text{ K}^{-1}$. Substituting the values: $-400 - T(-20) $-400 + 20T $20T $T Therefore, the reaction is spontaneous below $20 \text{ K}$.

Class 11 Chemistry Thermodynamics Free energy and Work

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The values of $\Delta H$ and $\Delta S$ of a certain reaction are $-400 \text{ kJ mol}^{-1}$ and $-20 \text{ kJ mol}^{-1} \text{ K}^{-1}$ respectively. The temperature below which the reaction is spontaneous, is

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A
$100 \text{ K}$
B
$20^\circ \text{ C}$
C
$20 \text{ K}$
D
$120^\circ \text{ C}$

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The values of $\Delta H$ and $\Delta S$ of a certain reaction are $-400 \text{ kJ mol}^{-1}$ and $-20 \text{ kJ mol}^{-1} \text{ K}^{-1}$ respectively. The temperature below which the reaction is spontaneous, is

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