A container holds 6.4 moles of gas. Hydrogen gas makes up 25% of the total moles in the container if the total pressure is 1.24 atm. What is the partial pressure of hydrogen?

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A container holds 6.4 moles of gas. Hydrogen gas makes up 25% of the total moles in the container if the total pressure is 1.24 atm. What is the partial pressure of hydrogen?

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Answer 1 · 2017-03-27T07:34:15

$P_{H_{2}} = 25 % \times P_{Total} = 0.31 \cdot a t m$ $P_(H_2)=25%xxP_"Total"=0.31*atm$

Explanation:

$P_{Total} = \frac{n_{Total} R T}{V}$ $P_"Total"=(n_"Total"RT)/V$

$= \frac{n_{H_{2}} + n_{other gases}}{V}$ $=(n_(H_2)+n_"other gases")/V$

But $n_{H_{2}} = 25 % \times n_{Total}$ $n_(H_2)=25%xxn_"Total"$ .

And thus $P_{H_{2}} = 25 % \times P_{Total} = 25 % \times 1.24 \cdot a t m = ? ?$ $P_(H_2)=25%xxP_"Total"=25%xx1.24*atm=??$

For more spray, see [here and links.](https://socratic.org/questions/how-would-you-define-and-explain-dalton-s-law-of-partial-pressure)

This treatment relies on $Dalton's Law of Partial Presssures$ $"Dalton's Law of Partial Presssures"$ , which states that in

$in a gaseous mixture, the partial pressure exerted$ $"in a gaseous mixture, the partial pressure exerted"$
$by a gaseous component, is the same as the pressure it would$ $"by a gaseous component, is the same as the pressure it would"$
$exert if it ALONE occupied the container.$ $"exert if it ALONE occupied the container."$

$The total Pressure is the sum of the individual partial pressures.$ $"The total Pressure is the sum of the individual partial pressures."$

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A container holds 6.4 moles of gas. Hydrogen gas makes up 25% of the total moles in the container if the total pressure is 1.24 atm. What is the partial pressure of hydrogen?

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