At the same temperature, what can be said about the average kinetic energy of two gases, such as H2 and O2?

The average kinetic energy of gas molecules is directly related to the temperature of the gas. The kinetic molecular theory states that at a given temperature, all gases have the same average kinetic energy, regardless of their molecular weights or types. Therefore, if both hydrogen (H2) and oxygen (O2) are at the same temperature, they will possess the same average kinetic energy. This equivalence holds true due to the relationship ( KE = \frac{3}{2} kT ), where ( KE ) is the average kinetic energy, ( k ) is the Boltzmann constant, and ( T ) is absolute temperature measured in Kelvin.

In this scenario, H2 and O2, while having different masses and speeds at the same temperature, will still be measured to have identical average kinetic energy. This fundamental principle of gas behavior ensures that temperature is the critical factor in determining average kinetic energy, not the specific characteristics of the gas molecules themselves.