For a particular liquid,raising its temperature from 339 K to 365 K causes its vapor pressure to double.What is the enthalpy of vaporization of this liquid? (R = 8.31 J/(K · mol))

Question

Quizplus · Accepted Answer

The Clausius-Clapeyron equation relates the change in vapor pressure with temperature to the enthalpy of vaporization. Using the equation ln(P2/P1) = -ΔHvap/R * (1/T2 - 1/T1), where P2/P1 = 2, T1 = 339 K, T2 = 365 K, and R = 8.31 J/(K·mol), solving for ΔHvap gives approximately 27,000 J/mol or 27 kJ/mol.

For a Particular Liquid,raising Its Temperature from 339 K to 365