🤓 Based on our data, we think this question is relevant for Professor Wingrave's class at UD.
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?