   # Calculate the entropy change, Δ r S °, for the vaporization of ethanol, C 2 H 5 OH, at its normal boiling point, 78.0 °C. The enthalpy of vaporization of ethanol is 39.3 kJ/mol. ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 18, Problem 43GQ
Textbook Problem
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## Calculate the entropy change, ΔrS°, for the vaporization of ethanol, C2H5OH, at its normal boiling point, 78.0 °C. The enthalpy of vaporization of ethanol is 39.3 kJ/mol.

Interpretation Introduction

Interpretation:

The ΔrS for a vaporization of ethanol should be calculated under given conditions.

Concept introduction:

The Gibbs free energy or the free energy change is a thermodynamic quantity represented by ΔrG. It is related to entropy and entropy by the following expression,

ΔrG=ΔrHTΔrS

Here, ΔrH is the change in enthalpy and ΔrS is the change in entropy.

The value of ΔrG is zero at the boiling point of the liquid. Thus the entropy change can be written as,

ΔrS=ΔrHT

### Explanation of Solution

The ΔrS for a vaporization of ethanol at its boiling point is calculated below.

The given reaction is,

C2H5OH(l)C2H5OH(g)

The boiling point is 78°C.

The enthalpy of vaporization of ethanol is 39.3 kJ/mol.

ΔrG=ΔrHTΔrS

At the boiling point the value of ΔrG is zero

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