Problem: The enthalpy of vaporization for acetone is 32.0 kJ/mol. The normal boiling point for acetone is 56.5 ˚C. What is the vapor pressure of acetone at 23.5 ˚C?

FREE Expert Solution

We need an equation that relates vapor pressure, temperature and enthalpy of vaporization. We're going to use the Clausius-Clapeyron Equation to solve this problem:

Given: 

Normal boiling point of acetone (T1) = 56.5°C + 273.15 = 329.65 K
Normal pressure (P1) = 1 atm
T2 = 23.5°C + 273.15 = 296.65 K
 vapor pressure (P2) = ?
ΔHvap = 32.0 kJ/mol

Substitute values and calculate for P2:

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Problem Details

The enthalpy of vaporization for acetone is 32.0 kJ/mol. The normal boiling point for acetone is 56.5 ˚C. What is the vapor pressure of acetone at 23.5 ˚C?

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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.