Chapter 8.3, Problem 8.6CE

Interpretation Introduction

Interpretation:

Reason for why volume is increased when pressure is constant and the way in which constant volume is maintained when temperature is raised should be explained.

Concept Introduction:

Kinetic-molecular theory of gases:

Properties of gases are different from solids and liquids.  When pressure is applied to gases, they are easily compressed to smaller volume and they have low densities.  These properties can be explained by a theory called kinetic-molecular theory.

The four assumptions of this theory are given below:

• Gases are made up of particles like atoms or molecules which randomly move and there will be no attractive forces between them.
• Comparing the space occupied by the gas particles and the space between particles, the former is much smaller than the latter.
• The average kinetic energy of gas particles and the Kelvin temperature is proportional.
• There is an elastic collision between gas particles or with the wall of their container and thus no energy is lost during collision and total kinetic energy of the particles is constant.

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

  $\begin{array}{l}\text{V}\propto \text{T}\\ \text{V}\text{=}\text{Constant}\text{×}\text{T}\\ \frac{{\text{V}}_{\text{1}}}{{\text{T}}_{\text{1}}}\text{=}\frac{{\text{V}}_{\text{2}}}{{\text{T}}_{\text{2}}}\end{array}$