JEE MAIN - Chemistry (2025 - 24th January Morning Shift - No. 14)
Let us consider an endothermic reaction which is non-spontaneous at the freezing point of water. However, the reaction is spontaneous at boiling point of water. Choose the correct option.
Both $\Delta \mathrm{H}$ and $\Delta \mathrm{S}$ are (-ve)
$\Delta \mathrm{H}$ is $(+\mathrm{ve})$ but $\Delta \mathrm{S}$ is (-ve)
$\Delta \mathrm{H}$ is $(-\mathrm{ve})$ but $\Delta \mathrm{S}$ is (+ve)
Both $\Delta \mathrm{H}$ and $\Delta \mathrm{S}$ are (+ve)
Explanation
Reaction is spontaneous at relatively high temperature and non-spontaneous at low temperature $\Delta \mathrm{G}=\Delta \mathrm{H}-\mathrm{T} \Delta \mathrm{S}$ It is only possible when $\Delta \mathrm{H}$ and $\Delta \mathrm{S}$ both are positive.
Option (1)
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