A certain substance has a heat of vaporization of 56.91 kJ/mol. At what Kelvin temperature will the vapor pressure be 4.00 times higher than it was at 295 K?
+37097 Here is a good video on YouTube which is almost exactly this problem.....
https://www.youtube.com/watch?v=OGAxPWUB8H8
ln (p2/p1) = - hvap/r (1/T2 - 1/T1) r = gas constant = 8.314 hvap = 569100 j/mol p2 is 4 x p1
ln(4) = - 56910/8.314(1/T2 - 1/295) solve for T2
1.386294 = - 56910/8.314 (1/T2 - 1/295)
T2 = 313.74 K for a vapor pressure 4 times higher than at 295K
No guarantee about this answer....but I am reasonably sure it is correct !
