Which of the following correctly describes why the behavior of a real gas deviates from an ideal behavior?

At high pressures the volume of gas particles becomes important, and at low temperatures the effect of intermolecular forces becomes significant.
At low pressures the volume of gas particles becomes important, and at high temperatures the effect of intermolecular forces becomes significant.
At high pressures the volume of gas particles becomes important, and at high temperatures the effect of intermolecular forces becomes significant.
At low pressures the volume of gas particles becomes important, and at low temperatures the effect of intermolecular forces becomes significant.

The correct answer is: At high pressures the volume of gas particles becomes important, and at low temperatures the effect of intermolecular forces becomes significant.

Explanation:

A gas can behave as an ideal gas at normal conditions of pressure and temperature. When the pressure is low, the volume occupied by the gas molecules is negligible in comparison with the total volume of the container. But at high pressures, the gas is compressed, the molecules occupies a significant volume and it becomes more important. The same occur with temperature. When the gas is at a low temperature, the molecules do not interact each other but when the temperature is high, there are more collisions between molecules and their interaction becomes more important.