   # Using the Clausius-Clapeyron equation : Calculate the enthalpy of vaporization of diethyl ether, (C 2 H 5 ) 2 O (Figure 11.12).This compound has vapor pressures of 57.0 mm Hg and 534 mm Hg at −22.8 °C and 25.0 ℃, respectively. (a) 29.0 kJ/mol (b) 112 kJ/mol (c) 2.44 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 11.6, Problem 2RC
Textbook Problem
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## Using the Clausius-Clapeyron equation: Calculate the enthalpy of vaporization of diethyl ether, (C2H5)2O (Figure 11.12).This compound has vapor pressures of 57.0 mm Hg and 534 mm Hg at −22.8 °C and 25.0 ℃, respectively. (a) 29.0 kJ/mol (b) 112 kJ/mol (c) 2.44 kJ/mol

Interpretation Introduction

Interpretation: It should be determined for the enthalpy of vaporization of diethyl ether compound.

Concept introduction:

Given

Vapor pressure

P2 = 534mm Hg at T2=298K

P1 = 57.0mm Hg at T1=250.2K

### Explanation of Solution

According to clausius clapeyron equation,

lnP2P1 = ΔHVAPR(1T1-1T2)

Here,P is vapour pressure at temperature T ,

ΔHVAP is enthalpy of vapourisation,

R is gas constant 8.314JK-1.

We have,

P2 = 534mm Hg at T2=298K

P1 = 57.0mm Hg at T1=250.2K

Substituting the above value in equation,

Calculating for ΔHVAP

ln(53457

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