$\mathbf{Volume}\mathbf{}\mathbf{fraction}\mathbf{=}\frac{\mathbf{actual}\mathbf{}\mathbf{volume}}{\mathbf{molar}\mathbf{}\mathbf{volume}\mathbf{}\mathbf{at}\mathbf{}\mathbf{STP}}\mathbf{\times}\mathbf{100}$

Actual volume Ar = b/4

It turns out that the van der Waals constant b equals four times the total volume actually occupied by the molecules of a mole of gas. Using this figure, calculate the fraction of the volume in a container actually occupied by Ar atoms:

Assume b= 0.0322 L/mol.

at STP

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