Final answer:
The temperature of a gas is most accurately related to the average kinetic energy, not the average velocity, number of molecules, or internal potential energy of the molecules.
Step-by-step explanation:
In thermodynamics, the temperature of a gas is most accurately related to the average kinetic energy of the gas molecules. This is better explained by considering the kinetic theory of gasses. The theory states that, for an ideal gas, the average kinetic energy of the gas molecules is directly proportional to the absolute temperature of the gas. Kinetic energy is largely a function of velocity, so the average velocity of the gas molecules does have a relationship with temperature, but the number of molecules or the internal potential energy do not directly affect the temperature.
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