Which factor can lead to deviations from ideal gas behavior?

Deviations from ideal gas behavior occur when real gases do not conform to the assumptions of the ideal gas law, which are based on the ideal conditions of high temperature and low pressure. When a gas is subjected to low temperatures, the kinetic energy of the gas molecules decreases, causing them to come closer together and experience intermolecular forces. At the same time, high pressure forces these gas molecules into a smaller volume, enhancing the effects of intermolecular attractions and repulsions.

Under these conditions, the ideal gas law fails because it assumes no interactions and that the volume of the gas particles is negligible. However, in reality, at low temperatures and high pressures, the volume occupied by gas molecules becomes significant compared to the volume of the container, and attractive forces become more pronounced. This leads to deviations from the ideal gas assumptions, making it essential to consider real gas behavior and corrections like the Van der Waals equation when analyzing such situations.