Gas molecules move at very high velocities and have high kinetic energy. The ideal gas laws are elegant and profound in their meaning. Kinetic theory enables us to arrive at the same conditions by thinking about the nature of molecules as we do from performing well-chosen experiments.
- Gases are composed of particles. The particles are negligibly small compared to their container and to the distance between each other.
- The particles are in constant random motion colliding with the walls of the container. These collisions with the walls cause the pressure exerted by the gas. Pressure is constant in a container over time., molecular collisions are assumed to be perfectly elastic.
- The gas particles are assumed not to attract or to repel each other.
- The average kinetic energy of the molecules in a system is linearly proportional to the absolute Kelvin temperature.