# Kinetic Theory of Gases Tutorial

## Key Concepts

- The kinetic theory, or the kinetic-molecular theory, of gases explains the properties of ideal gases.
- The kinetic theory of gases is based on the following four assumptions:
**1.**A gas is composed of a large number of tiny particles which are so small that their sizes are negligible compared to the average distances between them, that is, most of the volume of a gas is just empty space.**2.**Gas particles are in constant, random, straight-line motion, colliding with each other and the walls of the container.

All collisions are elastic, there is no net loss or gain of kinetic energy at each collision.**3.**Gas particles move independently of each other, there are no forces of attraction or repulsion between them.**4.**At any given instant there is a wide range of particle speeds and therefore a wide range of molecular kinetic energies, however, the average kinetic energy of all the gas particles is proportional to the absolute temperature (temperature in kelvin).The kinetic energy, E

_{k}or K.E, of a single gas particle is given by the equation below:E

_{k}= ½mv^{2}where m = mass of gas particle and v = speed of gas particle

- Gases will deviate from ideal gas behaviour if one or more of these assumptions does not apply