Chapter 8, Problem 8.112GP

(a)

Interpretation Introduction

Interpretation:

The external pressure at a depth of $\text{25}\text{m}$ should be found out if the external pressure increases by $\text{1}\text{atm}$ for every $10\text{m}$ depth.

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.

(b)

Interpretation Introduction

Interpretation:

The partial pressures of oxygen and nitrogen in the diver’s lungs at the given depth 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.