The pressure exerted by a gas is due to the collisions of the gas particles with the walls of the container. The ideal gas law describes the behavior of gases under ideal conditions, which means that the gas particles are assumed to be point particles with no interactions between them.
In reality, gas particles do interact with each other, and these interactions can affect the pressure exerted by the gas. For example, at high pressures, the gas particles are more likely to collide with each other, which can cause the pressure to increase.
The ideal gas law is a good approximation for the behavior of gases at low pressures and high temperatures, but it does not accurately describe the behavior of gases at high pressures or low temperatures.
