At T K,a gaseous mixture of H_2 and O_2 cont | vedclass

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(C) Given: $P_{	ext{total}} = 2 \ bar$. For $100 \ g$ of the mixture,mass of $H_2 = 20 \ g$ and mass of $O_2 = 80 \ g$. Moles of $H_2$ $(n_{H_2})$ =

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$0.4$

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(C) Given: $P_{	ext{total}} = 2 \ bar$. For $100 \ g$ of the mixture,mass of $H_2 = 20 \ g$ and mass of $O_2 = 80 \ g$. Moles of $H_2$ $(n_{H_2})$ = $\frac{20 \ g}{2 \ g/mol} = 10 \ mol$. Moles of $O_2$ $(n_{O_2})$ = $\frac{80 \ g}{32 \ g/mol} = 2.5 \ mol$. Mole fraction of $O_2$ $(x_{O_2})$ = $\frac{n_{O_2}}{n_{H_2} + n_{O_2}} = \frac{2.5}{10 + 2.5} = \frac{2.5}{12.5} = 0.2$. Partial pressure of $O_2$ $(P_{O_2})$ = $x_{O_2} 	imes P_{	ext{total}} = 0.2 	imes 2 \ bar = 0.4 \ bar$.

At $T \ K$,a gaseous mixture of $H_2$ and $O_2$ containing $20 \%$ (weight/weight) of $H_2$ exerts a total pressure of $2 \ bar$. What is the partial pressure of $O_2$ (in bar)?

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