What happens to gas behavior when it is subjected to high pressure and low temperature according to gas laws?

Under conditions of high pressure and low temperature, gas behavior deviates significantly from that predicted by the ideal gas laws. When pressure is increased, the gas molecules are forced closer together, and as the temperature decreases, the kinetic energy of the molecules decreases, causing them to move slower.

At this point, intermolecular forces begin to dominate the behavior of the gas. If the conditions are right, the gas can lose enough energy that the attractive forces between the molecules cause them to condense into a liquid. This transformation occurs because the molecules no longer have sufficient energy to overcome the attractions that pull them together.

This process is well described by the phase diagrams of substances, which indicate the regions of gas, liquid, and solid phases based on temperature and pressure. In summary, at high pressure and low temperature, gases tend to condense into a liquid due to the influence of intermolecular forces becoming significant at these conditions.