What is the kinetic theory of gases and its postulates?

The kinetic theory of gases explains the behaviour of gases based on the motion of their particles.

According to the kinetic theory of gases, gases are made up of tiny particles (atoms or molecules) that are in constant random motion. The particles are assumed to be point masses with no volume, and they are separated by large distances relative to their size. The particles collide with each other and with the walls of their container, and these collisions are assumed to be perfectly elastic, meaning that no energy is lost during the collision.

The theory also assumes that the particles have negligible intermolecular forces, meaning that they do not attract or repel each other. The temperature of a gas is related to the average kinetic energy of its particles, with higher temperatures corresponding to higher average speeds of the particles.

The kinetic theory of gases can be used to explain many of the macroscopic properties of gases, such as their pressure, volume, and temperature. For example, the pressure of a gas is related to the frequency and force of the collisions of its particles with the walls of the container. The volume of a gas is related to the amount of space its particles occupy, and the temperature of a gas is related to the average kinetic energy of its particles.