Explanation:
In real gases, there exists force of attraction between the molecules at low temperature and high pressure. This is because at low temperature there occurs a decrease in kinetic energy of gas molecules and high pressure causes the molecules to come closer to each other.
As a result, forces of attraction increases as molecules come closer to each other and therefore, gases deviate from an ideal gas behavior.
And, at low pressure and high temperature there exists no force of attraction or repulsion between the molecules of a gas. Hence gases behave ideally at these conditions.
Therefore, we can conclude that as the space between molecules in a gas sample decreases, the tendency for the behavior of this gas increases to deviate from the ideal gas laws.
