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:
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:
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?
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Clausius-Clapeyron Equation concept. You can view video lessons to learn Clausius-Clapeyron Equation. Or if you need more Clausius-Clapeyron Equation practice, you can also practice Clausius-Clapeyron Equation practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Wingrave's class at UD.
What textbook is this problem found in?
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.