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Under what conditions will a gas be most likely to exhibit the ideal gas properties predicted by the ideal gas law? High pressures and high temperature, because particles are forced closer together with higher kinetic energy, so intermolecular forces of attraction are weaker High pressure and low temperature, because particles are forced closer together and moving slower, so the volume of the particles is less significant Low pressure and high temperature, because particles are spread farther apart and moving faster, so the intermolecular forces of attraction are weaker Low pressure and low temperature, because particles are spread farther apart with lower kinetic energy, so the volume of the particles is less significant

Low pressure and high temperature, because particles are spread farther apart and moving faster, so the intermolecular forces of attraction are weaker

Explanation:

At low pressure and high temperature, gas molecules are separated and do not associate appreciably.

Recall that the the kinetic theory of gases holds that there is only a negligible intermolecular interaction between gases hence particles of a gas are relatively free and move about randomly at maximum velocities and kinetic energy.

This is only possible at low pressure and high temperature. At low pressure, gas particles are separated from each other and do not interact appreciably. High temperature imparts maximum kinetic energy to gas particles. Hence the answer.

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