Which postulate of the kinetic molecular theory breaks down under conditions of high pressure? Explain.

Key Concepts

Kinetic Molecular Theory

The Kinetic Molecular Theory (KMT) describes the behavior of gases in terms of particles in constant motion. It posits that gas particles are small, have negligible volume, and experience elastic collisions. This theory helps explain gas properties such as pressure, temperature, and volume, providing a framework for understanding gas behavior under various conditions.

Ideal Gas Behavior

Ideal gas behavior refers to the assumption that gas particles do not interact with each other and occupy no volume. This behavior is described by the Ideal Gas Law (PV=nRT), which holds true under low pressure and high temperature. However, deviations from ideal behavior occur at high pressures, where particle volume and intermolecular forces become significant.

High Pressure Effects

Under high pressure, the assumptions of the Kinetic Molecular Theory begin to break down because gas particles are forced closer together, leading to significant intermolecular forces and a noticeable volume of the particles themselves. This results in deviations from the Ideal Gas Law, as real gases do not behave ideally under such conditions, affecting their pressure, volume, and temperature relationships.