Chapter 13.5, Problem 3.3ACP

Interpretation Introduction

Interpretation: The total amount of nitrogen and oxygen in water and the mole fraction of oxygen in the given gas mixture should be determined.

Concept introduction:

• Mole fraction is one of the concentrations expressing term which is equal to the number of moles of a component divided by the total number of a solution. The mole fraction of all components of a solution, when added together will equal to $1$

  The mole fraction of component a can be determined by using the equation,

                      $\text{Mole}\text{fraction}\text{of}\text{a}{\text{(X}}_{\text{a}}\text{)}=\frac{\text{Mole}\text{of}\text{a}}{\text{Total}\text{moles}}$

• Raoult’s law: the vapor pressure of a solvent above a solution ($P_{solution}$)is equal to the vapor pressure of the pure solvent($P^0{}_{solvent}$ ) at the same temperature scaled by the mole fraction of the solvent ($X_{Solvent}$ )present.

            ${\text{P}}_{\text{solution}}\text{=}{\text{X}}_{\text{solvent}}\text{×}{\text{P}}^{\text{0}}{}_{\text{solvent}}$

• $Density=\frac{Mass}{Volume}$
• Henry’s law: The solubility of a gas in liquid is directly proportional to the gas pressure.

  $\begin{array}{l}{\text{S}}_{\text{g}}{\text{= k}}_{\text{H}}{\text{P}}_{\text{g}}\text{,}\\ \text{where,}{\text{S}}_{\text{g}}\text{is}\text{the}\text{gas}\text{solubility}\text{(in}\text{mol/kg)}\\ {\text{k}}_{\text{H}}\text{is Henry's constant }\\ {\text{P}}_{\text{g}}\text{ is the partial pressure of the gaseous solute}\text{.}\end{array}$

• $\text{Pressure}\text{in}\text{atm}\text{=}\text{pressure}\text{in}\text{pascal}\text{×}\frac{\text{1}\text{atm}}{\text{101325}\text{Pascal}}$