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?

15 years ago

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.

15 years ago

Answered by Anonymous

333K

14 years ago

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