Chapter 10.8, Problem 3.2ACP

(a)

Interpretation Introduction

Interpretation:

The required mass of ${\text{NH}}_{\text{4}}{\text{NO}}_{\text{3}}$ has to be calculated.

Concept Introduction:

Different laws have been put forward to introduce properties of gases:

Boyle’s law:

At fixed temperature, the volume of a fixed amount of gas is inversely proportional to the pressure exerted by the gas.

  $\text{P}\propto \frac{\text{1}}{\text{V}}\left(\text{n}\text{,}\text{T}\text{will}\text{be}\text{constant}\right)$

Charles’s law: States that volume is directly proportional to temperature when the gas is held at constant pressure and number of molecules.

$\text{V}\propto \text{T}$

General Gas Law: Combining Charles’s law and Boyle’s law we get the General gas law or combined gas law.

  $\frac{{\text{P}}_{\text{1}}{\text{V}}_{\text{1}}}{{\text{T}}_{\text{1}}}\text{=}\frac{{\text{P}}_{\text{2}}{\text{V}}_{\text{2}}}{{\text{T}}_{\text{2}}}$

Avogadro’s hypothesis:

• To relate the amount of gas and the volume.
• $\text{V}\propto \text{n}\text{at}\text{constant}\text{T}\text{and}\text{P}$

Combining all these together ideal gas law is introduced:

  $\text{PV}\text{=}\text{nRT}$

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 ${\text{N}}_{\text{2}}\text{O}\text{and}{\text{H}}_{\text{2}}\text{O}$ in the airbag has to be calculated.

Concept Introduction:

Different laws have been put forward to introduce properties of gases:

Boyle’s law:

At fixed temperature, the volume of a fixed amount of gas is inversely proportional to the pressure exerted by the gas.

  $\text{P}\propto \frac{\text{1}}{\text{V}}\left(\text{n}\text{,}\text{T}\text{will}\text{be}\text{constant}\right)$

Charles’s law: States that volume is directly proportional to temperature when the gas is held at constant pressure and number of molecules.

General Gas Law: Combining Charles’s law and Boyle’s law we get the General gas law or combined gas law.

  $\frac{{\text{P}}_{\text{1}}{\text{V}}_{\text{1}}}{{\text{T}}_{\text{1}}}\text{=}\frac{{\text{P}}_{\text{2}}{\text{V}}_{\text{2}}}{{\text{T}}_{\text{2}}}$

Avogadro’s hypothesis:

• To relate the amount of gas and the volume.
• $\text{V}\propto \text{n}\text{at}\text{constant}\text{T}\text{and}\text{P}$

Combining all these together ideal gas law is introduced:

  $\text{PV}\text{=}\text{nRT}$

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