What assumptions does the kinetic theory of gases make about molecules?

The kinetic theory of gases simplifies the behavior of a gas by modeling it as a large collection of particles. The theory relies on several key assumptions regarding these molecules:

• Random Motion: The gas consists of a large number of identical molecules in constant, random motion, obeying Newton’s laws of motion.12
• Negligible Volume: The individual volume of the molecules is considered negligibly small compared to the total volume occupied by the gas, and they are separated by distances large relative to their size.12
• Elastic Collisions: Molecules undergo perfectly elastic collisions with each other and the container walls, meaning there is no loss of energy during these impacts.1
• No Intermolecular Forces: Aside from the brief duration of collisions, there are no attractive or repulsive forces acting between the molecules.12

These assumptions define a perfect gas, providing a reasonable approximation for real gases under conditions of extreme dilution and high temperature.12