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Kinetic Theory of Gases (K.T.G) explains the behavior of gases based on the motion of their molecules. According to this theory, a gas consists of a large number of tiny particles that are continuously moving in random directions.

K.T.G is an important topic in Thermal Physics and provides the foundation for understanding gas laws and thermodynamics.

What is Kinetic Theory of Gases?

The kinetic theory describes gases in terms of molecular motion. The pressure exerted by a gas is a result of collisions between gas molecules and the walls of the container. The faster the molecules move, the greater the pressure and temperature of the gas.

Assumptions of K.T.G

  • Gas molecules are extremely small compared to the volume of the container.
  • Molecules are in continuous random motion.
  • Collisions between molecules are perfectly elastic.
  • The intermolecular forces are negligible except during collisions.
  • The duration of collisions is very small.
K.T.G
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Characteristics of Gases

  • Gases do not have a fixed shape or volume.
  • Gas molecules move freely in all directions.
  • Gases can be compressed easily.
  • They expand to fill the entire container.
  • Their behavior depends on temperature and pressure.

Applications of K.T.G

  • Understanding gas laws.
  • Studying thermodynamic processes.
  • Designing engines and refrigeration systems.
  • Atmospheric and weather studies.
  • Industrial gas storage and transport.

Importance for JEE Main

Kinetic Theory of Gases is a frequently tested topic in JEE Main Physics. Questions are commonly asked on molecular motion, gas properties, assumptions of K.T.G, and their relationship with temperature and pressure. A clear understanding of this topic helps students build a strong foundation in thermodynamics.

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