At temperatures below 273 K, it is observed that liquid water spontaneously freezes to form solid ice. What must be true about the entropy changes of the system and surroundings for this process?

Question

Quizplus · Accepted Answer

The entropy of the system decreases when liquid water freezes and becomes solid ice. Therefore, ΔS_sys< 0. On the other hand, the surroundings become more disordered as they absorb the heat released by the freezing process, so the entropy of the surroundings increases. Thus, ΔS_surr> 0.

At Temperatures Below 273 K, It Is Observed That Liquid