At what temperature do gases typically exhibit ideal behavior?

Gases typically exhibit ideal behavior at high temperatures, primarily due to the increased kinetic energy of the gas molecules. As the temperature rises, the average speed of the molecules increases, leading to more effective collisions that are less influenced by intermolecular forces. This means that gas molecules move far enough apart that attractions or repulsions between them become negligible, which is one of the assumptions of the ideal gas law.

At high temperatures, gases also have a tendency to expand. The vast distances between gas molecules reduce the effects of both intermolecular forces and the volume occupied by the gas molecules themselves relative to the total volume of the gas, allowing the gas to behave more ideally.

In contrast, at low temperatures and extremely low temperatures, gases can condense into liquids or exhibit strong intermolecular attractions that disrupt ideal behavior. Room temperature can vary but is generally above the threshold where gases tend to show significant deviations from ideal behavior, especially for gases that have substantial intermolecular forces at reduced temperatures.