Chapter 15, Problem 10CR

Interpretation Introduction

Interpretation:

The meaning of partial pressure of an individual gas in a mixture is to be stated. The dependence of the total pressure of a gaseous mixture on the partial pressures of the individual gases in the mixture is to be stated. How Dalton’s law helps to realize that in an ideal gas sample, the volume of the individual molecules is significant compared with the bulk volume of the sample is to be stated.

Concept Introduction:

The partial pressure of a gas can be defined as the total pressure exerted by all the gases in the container multiplied by their mole fraction.

Suppose two gases A and B are in a container and the partial pressure of A can be calculated as,

${\text{P}}_{\text{a}}=\frac{{\text{n}}_{\text{a}}}{{\text{n}}_{\text{a}}+{\text{n}}_{\text{b}}}\times \text{P}$

Where

• ${\text{P}}_{\text{a}}$ is the partial pressure of gas A.
• ${\text{n}}_{\text{a}}$ is the number of moles of A.
• ${\text{n}}_{\text{b}}$ is the number of moles of B.
• $\text{P}$ is the total pressure in the container.