# 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.  Do the argon atoms, since they are more massive, exert a greater pressure on the walls of the container? Explain.

###### FREE Expert Solution

${\mathbf{P}}_{\mathbf{gas}}\mathbf{=}{\mathbf{X}}_{\mathbf{gas}}{\mathbf{P}}_{\mathbf{tot}}$

At constant T, P → n is proportional to V, VHe = VAr so:

• mole fraction:
• ${\mathbf{X}}_{\mathbf{He}}\mathbf{=}{\mathbf{X}}_{\mathbf{Ar}}\mathbf{=}\frac{{\mathbf{n}}_{\mathbf{gas}}}{{\mathbf{n}}_{\mathbf{tot}}}\mathbf{=}\frac{{\mathbf{V}}_{\mathbf{gas}}}{{\mathbf{V}}_{\mathbf{tot}}}\mathbf{=}\frac{\mathbf{1}}{\mathbf{2}}\mathbf{=}$0.5
###### 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.  Do the argon atoms, since they are more massive, exert a greater pressure on the walls of the container? Explain.