Problem: Consider a 1.0-L sample of helium gas and a 1.0-L sample of argon gas, both at room temperature and atmospheric pressure.Which gas sample would have the fastest rate of effusion?a) sample of helium b) sample of argon c) samples would have the same rate of effusion

FREE Expert Solution

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.

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

Thus, the lower molar mass faster rate of effusion:

• Molar Mass He = 4.0 g/mol
• Molar Mass Ar = 39.39 g/ mol
Problem Details

Consider a 1.0-L sample of helium gas and a 1.0-L sample of argon gas, both at room temperature and atmospheric pressure.

Which gas sample would have the fastest rate of effusion?

a) sample of helium

b) sample of argon

c) samples would have the same rate of effusion