The equilibrium vapor pressure of a single component liquid at 300 K was found to be 0.2 bar. The heat of vaporization of the liquid is 40 kJ/mol. Assume the vapor to be an ideal gas, its density to be much less than that of the liquid. Estimate the temperature at which the equilibrium vapor

Question

The equilibrium vapor pressure of a single component liquid at 300 K was found to be 0.2 bar. The heat of vaporization of the liquid is 40 kJ/mol. Assume the vapor to be an ideal gas, its density to be much less than that of the liquid. Estimate the temperature at which the equilibrium vapor pressure is doubled.

Accepted Answer

The logarithmic form of (7.45) – the solution of the Clausius– Clapeyron equation – can be used in the following form:

[latex]P_{2}=P_{1} e^{-\frac{\Delta_{ ext {vap }} h}{R}\left(\frac{1}{T_{2}}-\frac{1}{T_{1}} ight)} .[/latex] (7.45)

[latex]\ln \frac{P_{1} }{P_{2} }=\frac{\Delta _{vap} h}{R}(\frac{1}{T_{2} }-\frac{1}{T_{1} } )[/latex]

Solution of the equation inserting [latex]P_{1}/P_{2}[/latex] = 2 yields 313.55 K at which the vapor pressure is doubled.

Question 7.1: The equilibrium vapor pressure of a single component liquid ...

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