Chapter 6, Problem 6.80QE

Interpretation Introduction

Interpretation:

The partial pressure of oxygen in a container that holds $3.22\text{ mol}$ of oxygen and $4.53\text{ mol}$ of nitrogen has to be calculated.

Concept Introduction:

The net pressure of a mixture of gases is equal to the sum of the partial pressures of its constituent gases. This is known as Dalton’s law of partial pressure.

The total pressure for a mixture of two gases A and B is calculated as follows:

  $P_{\text{T}}=P_{\text{A}}+P_{\text{B}}$

In terms of mole fraction the partial pressure is calculated as follows:

  $P_{\text{A}}={\text{χ}}_{\text{A}}{P}_{\text{T}}$

Here,

$P_{\text{T}}$ denotes the total pressure exerted by the mixture of gases.

${\text{χ}}_{\text{A}}$ denotes the mole fraction of component gas A.

$P_{\text{A}}$ denotes the pressure exerted by the gaseous component A.

$P_{\text{B}}$ denotes the pressure exerted by the gaseous component B.