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A
gas consists of very small microscopic particles called 'molecules'.
Depending upon the nature of gas each gas molecule may consists of
an atom or group of atoms. Molecules are in a state of continuous
motion.
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All
the molecules of a gas are in stable state and are considered
identical.
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Any
finite volume of a gas consists of very large number of molecules.
At S.T.P. there are 3 x 1025 molecules in a cubic
meter.
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The
molecules are wide separated from each other as compared to their
own dimensions.
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The
diameter of a molecule is about 3 x 10-10 meter.
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Gas
molecules move in straight line in all possible directions (random
movement) with various speeds.
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Gas
molecules collide with each other and with the walls of container.
There collisions are perfectly elastic in nature.
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Gas
molecules when collide with the walls of container, they transfer
their momentum which appears as pressure of gas.
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Molecules
of an ideal gas exert no force of attraction or repulsion on one
another except during collision.
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The
average kinetic energy of gas molecules is directly proportional to
absolute temperature.
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At
a given temperature, the molecules of all gases have the same
kinetic energy.
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Newtonian
mechanics is applicable to molecular motion.
