Question
A certain substance has a heat of vaporization of 62.08 kJ/mol. At what Kelvin temperature will the vapor pressure be 4.50 times higher than it was at 361 K?
I've gotten it to the point of:
ln(4.50)=7466.47423176378616 K (1/361 - 1/T2)
Solving for T2 but I don't know where to go from here!
I've gotten it to the point of:
ln(4.50)=7466.47423176378616 K (1/361 - 1/T2)
Solving for T2 but I don't know where to go from here!