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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.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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.
Transcribed Image Text: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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