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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Solution

This statement is correct only for ideal gases. It is not possible to liquefy an ideal gas because there are no intermolecular forces of attractions between the molecules of an ideal gas.

It is true at low pressure and a high temperature only. If the statement is true under all conditions of temperature and pressure, it will not be possible to liquefy an ideal gas.

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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 the assumption is not applicable for real gases.

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