What does kinetic gas theory state about gas pressure?

Kinetic gas theory states that gas pressure is the result of collisions between gas molecules and the walls of their container. As gas molecules move rapidly and randomly, they exert force on the walls when they collide with them. This force per unit area is what we measure as pressure. The more frequent and forceful the collisions, the greater the pressure in the container.

This concept hinges on the understanding that gas molecules are in constant motion and that their kinetic energy contributes to the pressure exerted. Factors such as the number of collisions and the intensity of these collisions depend on variables like temperature and volume. Therefore, the relationship outlined in kinetic gas theory provides a clear explanation of how gas pressure arises from molecular behavior. Understanding these principles is essential in physical science as they apply to various real-world scenarios involving gases.