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(A) . Freezing of water to ice at $0^{\circ} C$ involves a phase change from liquid to solid,which decreases disorder,so $\Delta S < 0$.$B$. Freezing

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$A, B, C$ and $D$ only

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(A) . Freezing of water to ice at $0^{\circ} C$ involves a phase change from liquid to solid,which decreases disorder,so $\Delta S $B$. Freezing of water to ice at $-10^{\circ} C$ is a spontaneous process where liquid water turns to solid ice,decreasing entropy,so $\Delta S $C$. In the reaction $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$,the number of moles of gas decreases from $4$ to $2$,leading to a decrease in entropy,so $\Delta S $D$. Adsorption of $CO_{(g)}$ on a lead surface restricts the movement of gas molecules,decreasing entropy,so $\Delta S $E$. Dissolution of $NaCl$ in water increases the disorder of the system as the crystal lattice breaks down into ions,so $\Delta S > 0$.Therefore,entropy decreases in processes $A, B, C,$ and $D$.

During which of the following processes does entropy decrease?

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