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Chapter 53: Problem 4

Do you expect \(\Delta S\) to be positive or negative for the freezing of water? Explain your reasoning.

Short Answer

Expert verified
The entropy (\( \Delta S \)) for the freezing of water would be negative, indicating the system is becoming more ordered.

Step by step solution

01

Understand Changes in Entropy

Entropy (\( \Delta S \)) is a measure of the disorder of a system. A positive \( \Delta S \) means an increase in disorder, while a negative \( \Delta S \) means a decrease in disorder.
02

Understand the Context

The context here involves the change from liquid water to solid ice, which is a phase transition.
03

Apply Knowledge of Entropy and Phase Transitions

Generally, the solid phase of a substance (such as ice) is less disordered than its liquid phase (like water). Therefore, when water freezes and becomes ice, the system becomes more ordered.
04

Reach a Conclusion

Since the system goes from a more disordered state (liquid water) to a less disordered state (solid ice), the entropy (\( \Delta S \)) decreases. Thus, \( \Delta S \) should be negative.

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Most popular questions from this chapter

Under what conditions can an endothermic reaction occur naturally? Explain your reasoning.

Recall that \(\Delta H\) is positive for the melting of ice. In general, does \(\Delta \mathrm{H}>0\) tend to be the case for naturally occurring processes?

Do you expect \(\Delta S\) to be positive or negative for the melting of ice? Explain your reasoning.
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