On top of one of the peaks in Rocky Mountain National Park the pressure of the atmosphere is 500. torr. Determine the boiling point of water at this location. The heat of vaporization of water is 40.7 kj/mol.
3 answers
Use the Clausius-Clapeyron equation. Remember that the boiling point is the temperature at which the vapor pressure of the liquid is equal to the atmospheric pressure.
but there aren't enough information to use Clausius-Clapeyron equation
Why do you think I gave you the hint when I responded? You're supposed to remember that vapor pressure of water at 1 atm (760 torr) is 760 torr when it boils at 100 C.
ln(P2/P1) = (DHvap/R)(1/T1 - 1/T2)
P1 = 760 torr; T1 = 100 C
p2 = 500 torr; T2 = ??
DHvap = given in problem.
R is 8.314 and don't forget T must be in kelvin.
Solve for T2.
ln(P2/P1) = (DHvap/R)(1/T1 - 1/T2)
P1 = 760 torr; T1 = 100 C
p2 = 500 torr; T2 = ??
DHvap = given in problem.
R is 8.314 and don't forget T must be in kelvin.
Solve for T2.