   Chapter 18, Problem 11PS

Chapter
Section
Textbook Problem

Calculate the entropy change that occurs when 0.50 mol of ice is converted to liquid water at 0 °C in a reversible process. (qfus = 333 J/g)

Interpretation Introduction

Interpretation:

The entropy change that occurs when 0.50 mol of ice gets converted to liquid water at °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,

ΔS=qrevT

Here, ΔS is the change in entropy, qrev is the heat absorbed and T is the temperature. The formula is applicable if the work done is reversible.

Explanation

Given:

The given reaction is,

H2O(s)H2O(l)

qfus= 333 J/g

Number of moles of ice is 0.50 mol

The entropy change that occurs when 0.50 mol of ice is converted to liquid water at °C in a reversible process is calculated as follows,

The molar mass is 18.015 g/mol. The given fusion value is positive which then the conversion of ice to liquid should be negative of that value.

qrev(-333 J/g)(18

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