The ** mole fraction of the gas** is then given by:

$\overline{){\mathit{m}}{\mathit{o}}{\mathit{l}}{\mathit{e}}{\mathbf{}}{\mathit{f}}{\mathit{r}}{\mathit{a}}{\mathit{c}}{\mathit{t}}{\mathit{i}}{\mathit{o}}{\mathit{n}}{\mathbf{}}{\mathbf{\left(}}{\mathit{X}}{\mathbf{\right)}}{\mathbf{=}}\frac{\mathbf{m}\mathbf{o}\mathbf{l}\mathbf{e}\mathbf{}\mathbf{o}\mathbf{f}\mathbf{}\mathbf{gas}}{\mathbf{total}\mathbf{}\mathbf{mass}}}$

You may want to reference (Pages 411 - 412) Section 10.6 while completing this problem.

(a) What are the mole fractions of each component in a mixture of 15.08 g of O_{2}, 8.17 g of N_{2}, and 2.64 g of H_{2}?

(b) **What is the partial pressure in atm of H _{2} for the mixture if it is held in a 15.50 L vessel at 16 ^{o}C?**

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