Chapter 8, Problem 8.77AP

Interpretation Introduction

Interpretation:

The difference between ideal gas law and combined gas law should be explained.

Concept Introduction:

Ideal gas Equation:

Any gas is described by using four terms namely pressure, volume, temperature and the amount of gas. Thus combining three laws namely Boyle’s, Charles’s Law and Avogadro’s Hypothesis the following equation could be obtained. It is referred as ideal gas equation.

$\text{PV}\text{=}\text{nRT}$

Where,

$\begin{array}{l}\text{n = moles}\text{of}\text{gas}\\ \text{P = pressure}\\ \text{T = temperature}\\ \text{R = gas }\text{constant}\end{array}$

Combined gas law:

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 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.

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