According to Graham's Law, how does the rate of effusion relate to molar mass?

Graham's Law states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass. This means that as the molar mass of a gas increases, its rate of effusion decreases. Mathematically, this is often expressed with the equation:

[

\frac{Rate_1}{Rate_2} = \sqrt{\frac{Molar,Mass_2}{Molar,Mass_1}}

]

where (Rate_1) and (Rate_2) are the effusion rates of two gases, and (Molar,Mass_1) and (Molar,Mass_2) are their respective molar masses.

For example, if you have two gases with different molar masses, the gas with the lighter molar mass will effuse more quickly than the heavier gas. Hence, the heavier the gas, the slower its rate of effusion. This inverse relationship emphasizes that lighter gases escape through small openings faster than heavier gases, illustrating the significance of molar mass in the process of effusion.