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.
The statement is correct. Assumption true only at low pressure and high temperature of gaseous molecule. At low pressure, system volume increases but volume of real gas become negligible, molecules occupy no volume relative to system. At high temperature gas molecules movement become fastersuch that there is no intermolecular attraction. Under this condition gas behave as ideal gas.It is impossible to liquefy an ideal gas since ideal gas have no force of attraction between the gaseous molecules.
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