Gaseous State | Kinetic Theory of Gases#
Postulates of Kinetic Theory of Gases#
- A gas consists of a large number of very small tiny particles, which are identified as molecules. The molecules of a given gas are completely identical in size, shape and mass.
- The volume occupied by the molecules is negligible in comparison to the volume of the gas.
- The molecules are in rapid motion, which is completely random. During their motion, they collide with the sides of the vessel. The collisions are perfectly elastic in nature.
- The laws of classical mechanics are applicable to the molecules in motion.
- There is no force of attraction or repulsion amongst the molecules, i.e., they are moving independent of each other.
- At any given instant, a molecule can have energy ranging from a small value to a large value, but the average kinetic energy is proportional to the absolute temperature of the gas.
\[(K.E.)_{avg.} ∝ T\]
This also means that at fixed temperature, average kinetic energy of gas molecule is fixed.
Note
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Kinetic Theory of gases is applicable only for ideal gases.
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All the gas laws can be derived from Kinetic Theory of gases.