Final answer:
The rates of diffusion and effusion of gases increase with absolute temperature because higher temperatures lead to greater kinetic energy, thus faster movement of gas particles. Graham's law and Charles's law explain these relationships and the effect of molar mass and temperature on these rates.
Step-by-step explanation:
Relation between Absolute Temperature, and Rates of Diffusion and Effusion of Gases
The rates of diffusion and effusion are processes that depend on the kinetic energy of gas particles. Graham's law shows that the rate of effusion or diffusion of a gas is inversely proportional to the square root of the gas's molar mass. Meaning, gases with lighter molar masses diffuse or effuse faster than those with heavier molar masses at the same temperature.
Furthermore, according to Charles's law, at constant pressure, the volume of a fixed amount of gas is directly proportional to its absolute temperature (measured in Kelvin). Since temperature is a measure of kinetic energy, higher temperatures increase the speeds of gas particles, which in turn can increase the rates of diffusion and effusion.
This is because as the kinetic energy increases with temperature, gas particles move more rapidly, leading to more frequent and forceful collisions that can either increase diffusion rates across a concentration gradient or increase the rate at which gas particles pass through a small orifice (effusion).