Question

The normal boiling point of water under 1.00 atm pressure is 100.00 °C, or 373.15 K. The enthalpy of vaporization of water at this temperature is 40.68 kJ/mol. Use the Clausius-Clapeyron equation to predict the boiling point of water on the top of a mountain where the air pressure is 0.72 atm. Express your answer in °C

Name: The normal boiling point of water under 1.00 atm pressure is 100.00 °C, or 373.15 K. The enthalpy of vaporization of water at this temperature is 40.68 kJ/mol. Use the Clausius-Clapeyron equation to predict the boiling point of water on the top of a mountain where the air pressure is 0.72 atm. Express your answer in °C
Uploaded: 2023-03-09T12:45:12-08:00
Duration: 3 min 23 s
Channel: Madhur L
Description: The normal boiling point of water under 1.00 atm pressure is 100.00 °C, or 373.15 K. The enthalpy of vaporization of water at this temperature is 40.68 kJ/mol. Use the Clausius-Clapeyron equation to predict the boiling point of water on the top of a mountain where the air pressure is 0.72 atm. Express your answer in °C

          The normal boiling point of water under 1.00 atm pressure is 100.00 °C, or 373.15 K. The enthalpy of vaporization of water at this temperature is 40.68 kJ/mol. Use the Clausius-Clapeyron equation to predict the boiling point of water on the top of a mountain where the air pressure is 0.72 atm. Express your answer in °C

The normal boiling point of water under 1.00 atm pressure is 100.00 °C, or 373.15 K. The enthalpy of vaporization of water at this temperature is 40.68 kJ/mol. Use the Clausius-Clapeyron equation to predict the boiling point of water on the top of a mountain where the air pressure is 0.72 atm. Express your answer in °C

Added by Tammy H.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Madhur L

03/09/2023

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We are given the normal boiling point of water (373.15 K) and the enthalpy of vaporization (40.68 kJ/mol). Show more…

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The normal boiling point of water under 1.00 atm pressure is 100.00 °C, or 373.15 K. The enthalpy of vaporization of water at this temperature is 40.68 kJ/mol. Use the Clausius-Clapeyron equation to predict the boiling point of water on the top of a mountain where the air pressure is 0.72 atm. Express your answer in °C.