In the Kinetic Molecular Theory, how is the average kinetic energy of gas molecules related to temperature?

The average kinetic energy of gas molecules is indeed directly proportional to the temperature of the gas. This relationship is a fundamental aspect of the Kinetic Molecular Theory, which describes the behavior of gas particles.

As the temperature of a gas increases, the average kinetic energy of its molecules also increases. This is because temperature is a measure of the average energy of the molecules in a substance. Specifically, in the context of ideal gases, the equation that relates temperature (in Kelvin) to average kinetic energy can be expressed as:

KE = (3/2)kT

Here, KE is the average kinetic energy, k is the Boltzmann constant, and T is the absolute temperature in Kelvin. As temperature increases, this equation shows that the average kinetic energy increases proportionally.

This understanding is crucial in many areas of chemistry and physics, as it explains phenomena such as gas expansion and the relationship between temperature and pressure in gas laws. The direct proportionality explains not only why gases behave the way they do under varying temperatures but also lays the groundwork for understanding reaction kinetics and thermodynamics in various chemical processes.