Recall that ** Graham's Law of Effusion** allows us to compare the rate of effusion of two gases. Graham's Law states that the rate of effusion of a gas is inversely proportional to its molar mass.

$\mathbf{rate}\mathbf{=}\frac{\mathbf{1}}{\sqrt{{\mathbf{MM}}_{\mathbf{gas}}}}$

The *partial pressure and the average kinetic energy of a gas* are __not__ related to the **amount*** of the gas particles*. The* rate of effusion and the average velocity *of gas particles **decreases** as the *molar **mass of the particles increases*.

Molar mass of N_{2} : 28 g/mol → lighter → faster rate of effusion

Molar mass of Xe: 131.29 g/mol → heavier → slower rate of effusion

You may want to reference (Pages 224 - 230) Sections 5.8 while completing this problem.

A flask at room temperature contains exactly equal amounts (in moles) of nitrogen and xenon. Sort the conditions based on the gas described. Drag the appropriate items to their respective bins.

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