   # Estimate the boiling point of water in Denver, Colorado (where the altitude is 1.60 km and the atmospheric pressure is 630 mm Hg or 0.840 bar). ### 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 52GQ
Textbook Problem
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## Estimate the boiling point of water in Denver, Colorado (where the altitude is 1.60 km and the atmospheric pressure is 630 mm Hg or 0.840 bar).

Interpretation Introduction

Interpretation:

The boiling point of water should be estimated in Denver, Colorado.

Concept introduction:

The vapor pressure of a substance is related to its enthalpy of vaporisation by the

expression,

ln(p2p1)=ΔHvapR(1T11T2)

Here, p1 and p2 are the vapour pressures at two different temperatures T1 and T2. This equation is known as Clausius-Clapeyron equation and is used to estimate the vapor pressure of a substance at a particular temperature.

### Explanation of Solution

The boiling point of water in Denver, Colorado is calculated below.

The Appendix L referred for the values of standard enthalpies of water to calculate the value of ΔHvap.

The given reaction is,

H2O(l)H2O(g)

The ΔHvap for the above reaction is,

ΔHvap=(241.83 kJ/mol)(285.83 kJ/mol)=44 kJ/mol=44000 J/mol

The normal boling point of water  is 100 °C under the standard condition of pressure (p2) which is 760 mmHg. The value of p1 is 630 mmHg

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