   Chapter 11, Problem 64SCQ

Chapter
Section
Textbook Problem

Vapor pressures of NH3(ℓ) at several temperatures are given in the table below. Use this information to calculate the enthalpy of vaporization of ammonia. Interpretation Introduction

Interpretation:

The molar enthalpy of vaporization of ammonia has to be determined.

Concept Introduction:

Clausius-Clapeyron equation:

lnP=(ΔvapH0RT)+C

From this relationship we can calculate the molar enthalpy of vaporization by knowing the corresponding temperature and pressure values.

If we have pressures at two different temperatures, then enthalpy of vaporization can be calculated by

lnP2p1=-ΔvapH0R[1T2-1T1]

Boiling point of a liquid: The temperature at which external pressure and vapour pressure of the liquid become same.

Normal boiling point: When the external pressure is 760mmHg we can call it as normal boiling point.

Explanation

Given:

Temperature(°C) Vapor Pressure(mmHg)68.40.13245.40.52633.61.00018.72.004.75.0025.710.0050.120.00

Temperatures and corresponding pressures are given. We can calculate the molar enthalpy of vaporization by using the Clausius-Clapeyron equation

lnP2p1=-ΔvapH0R[1T2-1T1]

P1=0.132mmHg,P2=0.526mmHgT1=68

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