Final answer:
If sample A has a higher average kinetic energy than sample B, then sample A has the higher temperature because temperature is directly proportional to the average kinetic energy of gas particles.
Step-by-step explanation:
The student is asking about the relationship between average kinetic energy and temperature in gases. If sample A has a higher average kinetic energy than sample B, then sample A has the higher temperature. This is because the temperature of a gas is directly proportional to the average kinetic energy of its particles. As the temperature increases, so does the average kinetic energy, which can result in a wider range of particle speeds and a "flattened" distribution curve for kinetic energy.
Additionally, it's worth noting that at a given temperature, all gases have the same average kinetic energy (KEavg) for their molecules. This means that a gas with lighter molecules will have a higher root mean square speed (Urms), while heavier molecules will have a lower Urms and a slower speed distribution. However, this does not affect the relationship between temperature and average kinetic energy. The significant takeaway here is that temperature is the driving factor for kinetic energy differences in the context of thermal physics.