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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 $\Delta S < 0$. $(B)$ Freezin

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Only $A, B, C$ and $D$

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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?
$(A)$ Freezing of water to ice at $0^{\circ} C$
$(B)$ Freezing of water to ice at $-10^{\circ} C$
$(C)$ $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$
$(D)$ Adsorption of $CO_{(g)}$ on a lead surface
$(E)$ Dissolution of $NaCl$ in water

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During which of the following processes does entropy decrease? $(A)$ Freezing of water to ice at $0^{\circ} C$ $(B)$ Freezing of water to ice at $-10^{\circ} C$ $(C)$ $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$ $(D)$ Adsorption of $CO_{(g)}$ on a lead surface $(E)$ Dissolution of $NaCl$ in water