Chapter 13.6, Problem 13.9SC

Interpretation Introduction

Interpretation:

Partial pressure of oxygen and the moles of oxygen present in the mixture should be determined.

Concept introduction:

The problem can be solved using ideal gas law and Daltons gas law. The total number of moles (moles of nitrogen plus moles of oxygen) can be calculated using ideal gas law as follows

$\begin{array}{l}\text{PV=nRT}\\ \text{n=}\frac{\text{PV}}{\text{RT}}\end{array}$

Where, P is the total pressure of the mixture

V is the volume of the mixture

R is the gas constant

T is the absolute temperature and,

n is the total number of moles of nitrogen and oxygen gas

Now,

$\text{n}={\text{n}}_{{\text{N}}_2}+{\text{n}}_{{\text{O}}_2}$

${\text{n}}_{{\text{O}}_2}=\text{n}-{\text{n}}_{{\text{N}}_2}$

Once ${\text{n}}_{{\text{O}}_2}$ is calculated, one can use Dalton’s law to find out the partial pressure of oxygen gas in the mixture as follows

${\text{P}}_{{\text{O}}_{\text{2}}}{\text{= x}}_{{\text{O}}_{\text{2}}}\times \text{P}$

Where ${\text{P}}_{{\text{O}}_{\text{2}}}$ is the partial pressure of oxygen gas in the mixture.

${\text{x}}_{{\text{O}}_{\text{2}}}$ is the mole fraction of oxygen gas and,

P is the total pressure of the mixture.