Suppose the boiling point of pure water at high altitude is 85.00 °C. Use the Clausius-Clapeyron equation to determine the atmospheric pressure at this high altitude. The normal boiling point of water is 100.0 °C at 1 atm and its heat of vaporization is 40.7 kJ/mol.

Suppose the boiling point of pure water at high altitude is 85.00 °C. Use the Clausius-Clapeyron equation to determine the atmospheric pressure at this high altitude. The normal boiling point of water is 100.0 °C at 1 atm and its heat of vaporization is 40.7 kJ/mol.

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter15: Gases,liquids, And Solids

Section: Chapter Questions

Problem 51E

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Question

Suppose the boiling point of pure water at high altitude is 85.00 °C. Use the Clausius-Clapeyron equation to determine the
atmospheric pressure at this high altitude. The normal boiling point of water is 100.0 °C at 1 atm and its heat of vaporization is
40.7 kJ/mol.

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