Gases tend to deviate from the ideal gas law at

a. high pressures

b. low pressures

c. high temperature

d. low pressures and high temperatures

a. High pressures.

Explanation:

Hello,

In this case, when we recall the ideal gas model, we must take into account the following assumptions:

- All gas particles are in constant motion and collisions between the gas molecules and the walls of the container cause the pressure of the gas.

- The particles are so small that their volume is negligible compared with the volume occupied by the gas.

- The particles don't interact. There are no attractive or repulsive forces between them.

- The average kinetic energy of the gas particles is proportional to temperature.

Thus, such assumptions are only true at low pressures as the particles behave as described. Nonetheless, the pressure is increased, the particles are able to move faster to collisions and interactions start showing off, that is why at high pressures, the gases deviate from the ideal gas law.

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(a.) high pressures

Explanation:

Deviations from Ideal Gas Law Behavior:

At low temperatures or high pressures, real gases deviate significantly from ideal gas behavior.