What is the relationship between average kinetic energy and temperature?

The relationship between average kinetic energy and temperature is a foundational principle in thermodynamics and kinetic molecular theory. According to these concepts, the average kinetic energy of gas molecules is directly proportional to the temperature of the gas measured in Kelvin.

As the temperature increases, the average kinetic energy of the gas molecules also increases because temperature is a measure of the thermal energy in a system. Since kinetic energy is tied to the motion of particles, higher temperatures mean that these particles are moving faster, leading to greater average kinetic energy. This is essential in explaining why gases expand when heated and why they exert more pressure when temperature rises, as their molecules collide with container walls more frequently and with greater force.

Thus, the correct choice highlights this direct correlation, illustrating that as kinetic energy rises, so does temperature, creating a clear connection that can be observed in countless physical and chemical processes.