To solve this problem, you will need to use the Clausius-Clapeyron equation
ln(P1/P2) = (ΔHvap/R) * (1/T2 - 1/T1)
and this table of boiling points and heat of vaporization for liquids.
Liquid | Formula | Normal boiling temperature (°C) | Heat of vaporization (kJ/mol)
Mercury | Hg | 357.0 | 59.0
Water | H2O | 100.0 | 40.7
Ethanol | C2H5OH | 78.5 | 38.6
Methanol | CH3OH | 64.7 | 35.3
n-Octane | C8H18 | 125.7 | 35.0
Acetone | (CH3)2CO | 56.1 | 30.3
Chloroform | CHCl3 | 61.3 | 29.4
Diethyl ether | (C2H5)2O | 34.6 | 26.0
Ethane | C2H6 | -88.6 | 14.7
Methane | CH4 | -161.5 | 8.2
Question
What is the pressure of a system containing methanol at the temperature 34.2°C if the starting pressure and temperature are 1.04 atm and 23.9°C, respectively?