POSTULATES OF KINETIC THEORY OF GASES

The kinetic theory of gases is a theory that explains the behavior of gases by motion and collisions of their constituent particles. There are several postulates, or assumptions, that form the basis of this theory. These include:

• Gases are made up of many small particles (such as atoms and molecules) that are in constant motion.
• These particles have very little volume and do not interact except when they collide.
• Collisions between particles are elastic. That is, there is no loss of kinetic energy. 
• The average kinetic energy of the particles is proportional to the absolute temperature of the gas, according to the equation E = (3/2) kT, where E is the average kinetic energy, k is the Boltzmann constant, and T is the temperature of the gas.
• The pressure of a gas is a result of the collisions of its particles with the walls of the container.
• The gas particles move in random directions and at a wide range of velocities.
• A molecule moves in a straight line with uniform velocity between two collisions. 

Many of the known gas laws are derived from these assumptions, such as the ideal gas law and the laws of thermodynamics.

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