What does the kinetic theory of gases explain?

The kinetic theory of gases provides a comprehensive framework for understanding the behavior of gases by focusing on the motion of their constituent particles. It posits that gases are made up of numerous small particles (atoms or molecules) that are in constant, random motion. This theory explains several gas properties, such as pressure, temperature, and volume, by relating them to the speed and motion of these particles.

According to the kinetic theory, the pressure exerted by a gas results from collisions of the gas particles with the walls of their container. Higher temperatures correspond to increased kinetic energy, meaning particles move faster, which can increase pressure if the volume remains constant. Thus, the theory effectively connects macroscopic observations of gas behavior (like temperature and pressure) with microscopic phenomena (the motion and interactions of individual particles).

Understanding these principles helps explain why gases expand to fill their containers and exhibit behaviors like diffusion and effusion. This thorough relationship between particle motion and gas behavior makes the kinetic theory fundamental in chemistry.