Chapter 1, Problem 1.9NP

Consider a 31.0 L sample of moist air at $\text{6}0.°\text{C}$ and one atm in which the partial pressure of water vapor is 0.131 atm. Assume that dry air has the composition 78.0 mole percent ${\text{N}}_{\text{2}}$, 21.0 mole percent ${\text{O}}_{\text{2}}$, and 1.00 mole percent Ar.

1. What are the mole percentages of each of the gases in the sample?
2. The percent relative humidity is defined as $\%\text{RH}={\text{P}}_{\text{H},\text{O}}/{\text{P}}_{H_{2}O}^{*}$ where ${\text{P}}_{\text{H},\text{O}}$ is the partial pressure of water in the sample and $\text{P}=0.\text{197 atm}$ is the equilibrium vapor pressure of water at $\text{6}0.°\text{C}$. The gas is compressed at $\text{6}0.°\text{C}$ until the relative humidity is 100.%. What volume does the mixture contain now?
3. What fraction of the water will be condensed if the total pressure of the mixture is isothermally increased to 81.0 atm?