**Calculate the volume of 1 xenon atom:**

$\overline{)\mathbf{V}\mathbf{=}\frac{\mathbf{4}}{\mathbf{3}}{\mathbf{\pi r}}^{\mathbf{3}}}\phantom{\rule{0ex}{0ex}}\mathbf{V}\mathbf{=}\frac{\mathbf{4}}{\mathbf{3}}\mathbf{\pi}{(1.3\times {10}^{-8}\mathrm{cm})}^{\mathbf{3}}$

**V = 9.2028x10 ^{-24} cm**

**Calculate the number of moles of Xe present in the flask:**

$\mathbf{PV}\mathbf{=}\mathbf{nRT}\phantom{\rule{0ex}{0ex}}\frac{\mathbf{PV}}{\mathbf{RT}}\mathbf{=}\frac{\mathbf{n}\overline{)\mathbf{RT}}}{\overline{)\mathbf{RT}}}\phantom{\rule{0ex}{0ex}}\overline{)\mathbf{n}\mathbf{=}\frac{\mathbf{PV}}{\mathbf{RT}}}$

$\mathbf{V}\mathbf{=}\mathbf{100}\mathbf{}\overline{)\mathbf{mL}}\mathbf{\times}\frac{{\mathbf{10}}^{\mathbf{-}\mathbf{3}}\mathbf{}\mathbf{L}}{\mathbf{1}\mathbf{}\overline{)\mathbf{mL}}}$

**V = 0.100 L**

The radius of a xenon atom is 1.310^{-8} cm. A 100-mL flask is filled with Xe at a pressure of 1.3 atm and a temperature of 276 K .

Calculate the fraction of the volume that is occupied by Xe atoms. (*Hint*: The atoms are spheres.)

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