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?

Md Ariful Islam

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Md Ariful Islam

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$P_"Total"=(n_"Total"RT)/V$

$=(n_(H_2)+n_"other gases")/V$

But $n_(H_2)=25%xxn_"Total"$.

And thus $P_(H_2)=25%xxP_"Total"=25%xx1.24*atm=??$

For more spray, see

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

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

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

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