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What are Kinetic theory of gases

by Joy_Chemistry

Kinetic theory of gases is a theoretical model which details the molecular composition of the gas in terms of a huge number of sub microscopic particles that contain both atoms and molecules. Moreover, the theory explains that gas pressure arises due to particles colliding with one another and also the walls of the container.

The theory also defines properties such as viscosity, temperature and thermal conductivity

The kinetic theory of gases relates all these properties to the microscopic phenomenon.

The importance of the theory is that it provides a developing correlation between the macroscopic and microscopic phenomenon.,

In simple words the action of molecules highlights the kinetic theory of gases, the molecules of gases are always in motion.

The action of molecules, tend to collision with each other and also the walls of the container.

  Kinetic theory of gases assumes that the atoms and molecules of a gas are at constant moving point masses, with a large interparticle distance

The atoms and molecules of a gas also undergoes elastic collisions perfectly.

Kinetic Theory of Gases Postulates

The kinetic theory of gas postulates gives a more wider approach to understand the macroscopic properties from the microscopic properties.

• The gases containing large number of tiny particles known as atoms and molecules. Compared to the distance between the particles, they are extremely small. However, the individual particle size is negligible and the volume occupied by the gas is mostly empty space.

• These molecules are in constant random motion and results in collisions the collisions occur within each other and also the walls of the container

• The collisions between the molecules and with the walls are perfectly elastic. During collision of molecules kinetic energy is never lost.

During the process of collisions, the molecules do not slow down and are at the same speed.

• The average kinetic energy of the gas particles changes with temperature. The higher the temperature, the higher the average kinetic energy of the gas.

• During collisions , the molecules do not show any exertion of  any force of attraction or repulsion on one another.

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