For a particular liquid,raising its temperature from 321 K to 352 K causes its vapor pressure to double.What is the enthalpy of vaporization of this liquid? (R = 8.314 J/K · mol)
A) 21.0 kJ/mol
B) 186 kJ/mol
C) 3.29 kJ/mol
D) 383 kJ/mol
E) 179 kJ/mol

Question

Quizplus · Accepted Answer

Using the Clausius-Clapeyron equation, the enthalpy of vaporization can be calculated. Doubling the vapor pressure over a temperature change from 321 K to 352 K gives an enthalpy of vaporization of approximately 21.0 kJ/mol.

For a Particular Liquid,raising Its Temperature from 321 K to 352