Chapter 8, Problem 8.89AP

Interpretation Introduction

Interpretation:

The partial pressures of oxygen in a hyperbaric chamber which has $\text{21}\text{\%}{\text{O}}_{\text{2}}\text{and}\text{79\%}\text{He}$ at pressures up to $\text{120}\text{psi}$ should be determined.

Concept Introduction:

• Partial pressure: The pressure of each gas in a mixture of gases is the partial pressure.
• Dalton’s law of partial pressure: The total pressure of gases in a mixture of gases is the sum of the pressure of each gas in the mixture
• Mole fraction: Quantity which defines the number of moles of a substance in a mixture divided by the total number of moles of all substances present.

  ${\text{x}}_{\text{a}}\text{=}\frac{{\text{n}}_{\text{a}}}{{\text{n}}_{\text{total}}}$

• $\begin{array}{l}{\text{p}}_{\text{a}}\text{=}{\text{x}}_{\text{a}}\text{×}{\text{P}}_{\text{total}}\\ \end{array}$

  Partial pressure of a gas in the mixture of gases is the product of mole fraction of the gas and the total pressure.

General unit conversion:

$\begin{array}{c}\text{1}\text{atm}\text{=}\text{760}\text{mm}\text{Hg}\text{=}\text{14}\text{.7}\text{psi}\text{=}\text{101,325}\text{Pa}\\ \text{1}\text{inHg}\text{=}\text{25}\text{.4}\text{torr}\\ \text{1}\text{atm}\text{=}\text{760}\text{torr}\\ \text{1}\text{atm}\text{=}\text{760}\text{mm}\text{Hg}\text{=}\text{101}\text{.325}\text{kilopascals}\text{=}\text{1}\text{.01325}\text{bar}\end{array}$