What does an ideal gas assume about the molecular radius?

In the context of ideal gas behavior, it is assumed that the molecular radius of the gas particles is negligible compared to the distances between the molecules. This means that the size of individual gas molecules does not significantly affect the overall behavior of the gas, particularly in terms of pressure and temperature.

This assumption is crucial because it allows for a simplified model where gas molecules are treated as point particles that do not occupy any volume themselves. It enables the application of the ideal gas law and other calculations without having to consider the finite size of the gas particles, which would complicate the equations and concepts involved. In real gases, as pressure increases and temperatures decrease, the volume occupied by the gas molecules can no longer be neglected, but for an ideal gas, these effects are not considered. Hence, this assumption underlines the foundational principles of the kinetic molecular theory that describes the motion and energy of gas particles.