One of the assumptions of kinetic theory of gases is that there is no force of attraction between the molecules of a gas. State and explain the evidence that shows that assumption is not applicable for real gas.

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Solution

The assumption of kinetic theory of gases that there is no force of attraction between the molecules of a gas is not applicable for real gas because gases can be liquefied by cooling and compression of the gas. This proves that forces of attraction exist among the molecules.

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One of the assumptions of kinetic theory of gases states that "there is no force of attraction between the molecules of a gas." How far is this statement correct? Is it possible to liquefy an ideal gas? Explain.

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Q. One of the assumptions of the kinetic theory of gases is that there is no force of attraction between the molecules of a gas.

State and explain the evidence that shows that the assumption is not applicable for real gases.

Q. One of the assumptions of kinetic theory of gases is that there is no force of attraction between the
molecules of a gas.

Q. The main reason for deviation of gases from ideal behaviour is few assumptions of kinetic theory. These are
(i) there is no force of attraction between the molecules of a gas
(ii) volume of the molecules of a gas is negligibly small in comparison to the volume of the gas
(iii) Particles of a gas are always in constant random motion.

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