   # Calculate w and ∆ E when 1 mole of a liquid is vaporized at its boiling point (80.°C) and 1.00 atm pressure. ∆ H for the vaporization of the liquid is 30.7 kJ/mol at 80.°C. Assume the volume of 1 mole of liquid is negligible as compared to the volume of 1 mole of gas at 80.°C and 1.00 atm. ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 8, Problem 163CP
Textbook Problem
877 views

## Calculate w and ∆E when 1 mole of a liquid is vaporized at its boiling point (80.°C) and 1.00 atm pressure. ∆H for the vaporization of the liquid is 30.7 kJ/mol at 80.°C. Assume the volume of 1 mole of liquid is negligible as compared to the volume of 1 mole of gas at 80.°C and 1.00 atm.

Interpretation Introduction

Interpretation: the work done and ΔE for the vaporization of 1 mole of a liquid at its boiling point 80oC and 1atm should be determined, if the ΔH for the vaporization is 30.7kJ/mol .

Concept introduction:

• According to ideal gas law,

PV=nRT

• According to Ist-law of thermodynamics,

w=PΔV

ΔE=ΔH+w,atconstantpressure

### Explanation of Solution

Explanation

To determine: the work done for the vaporization of 1 mole of given liquid at its boiling point 80oC and 1atm .

The work done for the vaporization of 1 mole of given liquid is -2.94kJ .

The given 1 mole of liquid is vaporizing at its boiling point.

Therefore, the change in moles of gaseous molecules for the given vaporization process is 1.

The boiling point is 80oC=(80+273)K=353K

According to Ist-law of thermodynamics,

w=PΔV

According to ideal gas equation,

PV=nRT

Therefore,

At constant pressure and temperature,

PΔV=ΔnRT

Therefore,

The work done for the vaporization of 1 mole of given liquid is,

w=(1×8.3145J/Kmol×353K)=2.94kJ

Hence,

The work done for the vaporization of 1 mole of given liquid is -2

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