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## Homework Statement

Consider air to be made up of only N2 (78 mole %), O2 (21%) and Ar (1%)

Estimate the mole fractions of each in both the liquid and gas phases if 1 mole of air at 300 K and 4 atm. total pressure were cooled to 65 K in the same volume

## Homework Equations

Raoult's law Pi = Pi* xi

## The Attempt at a Solution

So I know that the atmospheric pressure is 760 torr. So before they are cooled

vapor pressure of N2 would be (0.78)(760) torr

Vapor Pressure of O2 would be (0.21)(760) torr

Vapor Pressure of Ar would be (0.01)(760) Torr

I'm not sure how should I proceed. Maybe I should use the Clausius Clapeyron equation to find the final pressure after cooling it down? But what delta H value should I use?