Vapor Pressure of Water

[deteam]

1. The problem statement, all variables and given/known data
The vapor pressure of water at 25.0 C is 23.8 torr, and the heat of vaporization is 43.9 kJ/mol. What is the vapor pressure (atm) of water at 59.8C?


2. Relevant equations
Clausius-Clapeyron equation.
ln(P2/P1)=(ΔH/R)((1/T1)-(1/T2))


3. The attempt at a solution

P2=?
P1=23.8 torr = .031315789 atm
ΔH=43.9 KJ/mol=43900 J/mol
R= 8.31 (J)/(mol∙K)
T1=25.0°C=298 K
T2=59.8°C=332.8 K

plugged into the equation and keep getting the wrong answer.

Can someone please help.

ln(p2) - ln(.031315789) = -(439005)/(8.31) * [(1/332.8) - (1/298)]

HELP idk what i did wrong

[flatmaster]

Atm is not KMS units

[PhaseShifter]

Atm is not KMS units
That shouldn't matter as long as P1 and P2 have the same units.

The setup looks good, but it does look like the calculations have a typo in the heat of vaporization though.