In terms of kinetic energy, what can we conclude about gas molecules at higher temperatures?

At higher temperatures, the average kinetic energy of gas molecules increases. This relationship is a direct consequence of temperature being a measure of the average kinetic energy of the particles in a substance. According to kinetic molecular theory, as the temperature of a gas rises, the energy of its molecules also rises, leading to more vigorous motion. This increased kinetic energy results in higher speeds for the molecules, which translates to greater energy within the system.

The average kinetic energy is defined mathematically as proportional to the temperature measured in Kelvin. This means that as one measures the temperature increase, one also expects to see an increase in the average kinetic energy of the gas molecules. Thus, at higher temperatures, gas particles collide with more force and frequency, leading to an overall rise in their energy.

In contrast, other options suggest scenarios that do not align with this fundamental principle. An average kinetic energy decrease or constancy at elevated temperatures contradicts the laws of thermodynamics, specifically that energy transfers and states change in correspondence with temperature variations. Lastly, the idea that average kinetic energy fluctuates does not hold for a system at thermal equilibrium, where temperature and corresponding kinetic energy are consistently averaged over time. Thus, the conclusion that average kinetic energy increases with temperature is consistent with established physical principles