Which two assumptions of the kinetic theory of gases fail for real gases at high pressure?

AMolecules are in random motion; collisions are elastic
BMolecular volume is negligible; there are no intermolecular forces
CAverage kinetic energy is proportional to temperature; collisions are elastic
DMolecules move in straight lines; pressure is due to collisions with walls

Answer: B

The ideal gas model treats molecules as point masses with no attractions. At high pressure the molecular volume is a significant fraction of the total and the molecules are close enough to attract each other, so both of these assumptions break down.

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