Why gases are non ideal at low temperature and high pressure?

Gases behave non-ideally at low temperatures and high pressures due to increased intermolecular forces and reduced kinetic energy. At low temperatures, gas molecules move more slowly, allowing attractive forces to have a greater influence, leading to deviations from ideal behavior. Additionally, at high pressures, the volume of gas molecules becomes significant compared to the overall volume of the gas, causing assumptions of point-like particles in the ideal gas law to break down. These factors result in discrepancies from the ideal gas behavior described by the ideal gas law.