The kinetic molecular theory defines gas particles as those that are tiny and display random, straight line motion, according to the University of California. The particles demonstrate quick and continuous motion and collide with each other and the walls of their container.
The kinetic molecular theory is based on these assumptions:
1. The composition of gases entails many particles that have features of hard spherical objects.
2. The particles take a straight course until collision.
3. The particles are very tiny compared with the space between them. Thus, most of the space in a filled gas container is unoccupied.
4. Gas particles don’t attract each other. Also, there exists no force of attraction between the particles and their container’s walls.
5. Collisions taking place inside a gas container between the gas particles or between the gas particles and the container’s walls are 100 percent elastic. As such, the collisions result in no energy loss.
6. The temperature of the gas determines the average kinetic energy of all particles that make it up.
According to the University of California, higher temperatures increase the velocity of gas particles and their kinetic energy. The mass of the particles is also a consideration in the formula for calculating their kinetic energy.