According to kinetic theory, what is the relationship between average kinetic energy of gas molecules and temperature?

The relationship between the average kinetic energy of gas molecules and temperature, as described by kinetic theory, is directly proportional. This means that as the temperature of a gas increases, the average kinetic energy of its molecules also increases.

Kinetic theory posits that temperature is a measure of the thermal energy of the gas particles. When the temperature rises, the molecules gain more energy and move faster, leading to an increase in their average kinetic energy. This relationship is critical because it helps explain many gas laws and behaviors, such as those governing pressure and volume changes in gases during heating or cooling processes.

Understanding this direct proportionality is essential for grasping the fundamental principles of thermodynamics and the behavior of gases in various physical situations.