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| Kinetic Theory of Gases |
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| The word 'Kinetic' means due to motion. The Kinetic Theory of Gases is based on the idea that gases consist of atoms and molecules moving ceaselessly and randomly with all possible velocities in all directions. Each of these gas particles has certain amount of kinetic energy that depends upon its temperature. Lighter particles move faster than heavier ones at all temperatures. Careful observations show that smaller the particles, more rapid is their motion at a given temperature. |
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| Kinetic theory of gases makes the following basic assumptions: |
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 Molecules are in a state of perfect chaos, moving with all possible velocities in all directions, colliding with each other and with the walls of the container. |
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Collisions between the gas molecules are considered to be perfectly elastic. This means that no kinetic energy is lost when two gas molecules collide against each other. |
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The attraction between the molecules of a gas is assumed to be almost zero. |
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The volume of the individual molecules is assumed to be negligible compared to the volume of the whole gas. |
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The time taken for a collision to occur is reckoned to be negligible compared to the time that a molecule spends between two collisions. |
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| The molecules of a gas collide against each other as well as against the walls of the container with a particular force. The strength of this force depends upon its kinetic energy. You must have realized that it is this force that is responsible for the pressure exerted by the gas upon the walls of the container. |
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