Which theory explains the behavior of gases?

The Kinetic Molecular Theory is the theoretical framework that underlies the behavior of gases. This theory posits that gas is composed of a large number of small particles (molecules or atoms) that are in constant, random motion. According to this theory, the temperature of a gas is directly proportional to the average kinetic energy of its particles.

As the temperature of a gas increases, the particles move faster, leading to more frequent and forceful collisions with each other and the walls of their container. This explains many observations related to gas behavior, such as how gases fill their containers, how they expand when heated, and how pressure varies with volume.

The other choices represent specific laws that describe certain behaviors of gases but do not encompass the overall behavior like the Kinetic Molecular Theory does. Charle's Law and Boyle's Law, for instance, govern relationships between temperature and volume, and pressure and volume, respectively, but they don't provide a comprehensive framework for understanding all aspects of gas behavior. Avogadro's Principle describes the relationship between the amount of gas and volume but is also more limited in scope compared to the Kinetic Molecular Theory.