Chapter 18, Problem 11PS

Interpretation Introduction

Interpretation:

The entropy change that occurs when $\text{0}\text{.50 mol}$ of ice gets converted to liquid water at $\text{0 }°\text{C}$ in a reversible process should be calculated.

Concept introduction:

The second law of thermodynamics relate the entropy of the system to the heat absorbed by the system. The change in entropy is related to the heat absorbed by the formula,

  $\Delta S=\frac{q_{\text{rev}}}{T}$

Here, $\Delta S$ is the change in entropy, $q_{\text{rev}}$ is the heat absorbed and $T$ is the temperature. The formula is applicable if the work done is reversible.