🤓 Based on our data, we think this question is relevant for Professor Sadeghi's class at UTSA.
We’re being asked to determine the vapor pressure of water at 40°C. We’re given the heat of vaporization of water ΔHvap = 40.7 kJ/mol.
We can use the Clausius-Clapeyron Equation to solve for the vapor pressure of water.
P1 = vapor pressure at T1
P2 = vapor pressure at T2
ΔHvap = heat of vaporization (in J/mol)
R = gas constant (8.314 J/mol•K)
T1 and T2 = temperature (in K).
The molar enthalpy of vaporization (∆H) of water is 40.7 kJ/mol. What is the vapor pressure of water at 40.°C (R=8.314J/K mol)?
A) 11.5 torr
B) 311 torr
C) 3.58 torr
D) 38.6 torr
E) 61.4 torr