Under what conditions will a gas be least likely to exhibit the ideal gas properties predicted by the ideal gas law?

High pressure and low temperature, because particles are forced close together and moving slower, so intermolceular forces of attraction increase.

Explanation:

The properties of an ideal gas are explained by the kinetic-molecular theory. An ideal gas assumes there is no intermolecular attraction between the molecules. High pressure would make the particles closer together and interact more, going against the kinetic molecular theory that states there are large spaces between particles and no interactions between particles. Low temperature would make the particles slow which prevents them from overcoming the intermolecular attraction between particles.