Chemistry – States of matter - Solids, liquids and gases | e-Consult

Kinetic Molecular Theory and Compressibility:

The Kinetic Molecular Theory states that gas particles are in constant, random motion. These particles are widely separated and have relatively low intermolecular forces. This means there is a significant amount of empty space between the particles. When pressure is applied, the gas particles are forced closer together, and the empty space is reduced. Because of the large spaces between the particles, gases can be easily compressed – a relatively small pressure change results in a significant volume change.

Liquids vs. Gases:

In liquids, the particles are much closer together than in gases. They are held together by stronger intermolecular forces. This means there is less empty space between the particles. When pressure is applied to a liquid, the particles are already relatively close together, so there is less space for them to move. Therefore, liquids are less compressible than gases. While liquids can be compressed to some extent, the compressibility is significantly less than that of gases.

Table summarizing compressibility: