The molecules of all ideal gases have the same average kinetic energies at the same *temperature*.

Here's why:

* Kinetic Energy and Temperature: The average kinetic energy of gas molecules is directly proportional to the absolute temperature (measured in Kelvin). The higher the temperature, the faster the molecules move, and the higher their average kinetic energy.

* Ideal Gas Law: The ideal gas law describes the behavior of ideal gases and relates pressure, volume, temperature, and the number of moles of gas. One of its key implications is that at a given temperature, the average kinetic energy of gas molecules is the same regardless of the type of gas.

Key Points:

* Ideal Gas: An ideal gas is a theoretical construct that assumes there are no intermolecular forces and that the volume of the gas molecules is negligible compared to the volume of the container. Real gases deviate from ideal behavior, especially at high pressures and low temperatures.

* Average Kinetic Energy: The average kinetic energy refers to the average of the kinetic energies of all the gas molecules in the sample. Not all molecules will have the same kinetic energy at a given instant, but the average will be the same for all ideal gases at the same temperature.

Let me know if you have any other questions!