Which gas law relates the rates of diffusion of two gases to their molar masses?

Graham's Law is the correct choice because it specifically describes the relationship between the rates of diffusion of two gases and their molar masses. According to this law, the rate of diffusion of a gas is inversely proportional to the square root of its molar mass. This means that lighter gases diffuse more rapidly than heavier gases. Mathematically, this is expressed as:

[ \frac{r_1}{r_2} = \sqrt{\frac{M_2}{M_1}} ]

where ( r_1 ) and ( r_2 ) are the rates of diffusion of gases 1 and 2, respectively, and ( M_1 ) and ( M_2 ) are their molar masses. This relationship allows us to predict how different gases will behave in diffusing through a medium, making Graham's Law a vital concept in physical chemistry and gas behavior.

The other laws mentioned do not address the relationship between diffusion rates and molar masses. Boyle's Law discusses the relationship between pressure and volume at constant temperature; Charles's Law focuses on the relationship between volume and temperature at constant pressure; while Avogadro's Law relates the volume of gas to the number of moles at constant temperature