Under what conditions does a real gas behave more like an ideal gas?

A real gas behaves more like an ideal gas under conditions where the molecules are far apart with weak attractions. This behavior aligns with the assumptions made about ideal gases, which include that gas molecules have negligible volume and do not exert forces on one another except during collisions.

When gas molecules are far apart, the interactions between them become minimal, and their individual properties dominate the behavior of the gas. Also, weak attractions ensure that the kinetic energy of the molecules, which is often substantial at higher temperatures and lower pressures, is not significantly offset by intermolecular forces. Under these conditions, the gas's behavior is more consistent with the ideal gas law, which operates most effectively when molecular interactions are negligible.

In scenarios where molecules are close together or have strong attractions, the behavior of the gas deviates from ideal behaviors due to significant intermolecular forces influencing the pressure and volume relationships described in the ideal gas law.