Asked by Karen

Benzene has a heat of vaporization of 30.72kJ/mol and a normal boiling point of 80.1 degrees C.

At what temperature does benzene boil when the external pressure is 405 torr?

how do i go about answering this question? i don't know where to start. am i supposed to use the clausius-clayperon equation?
Answered by DrBob222
Yes, use the Clausius-Clapeyron equation (capitals PLEASE). At the boiling point, the vapor pressure of benzene is 760 torr. The other set of points is 405 torr and x temperature. Solve for x temperature.
Answered by Anonymous
333K
There are no AI answers yet. The ability to request AI answers is coming soon!