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?

1 Answer
Mar 27, 2017

P_(H_2)=25%xxP_"Total"=0.31*atm

Explanation:

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=??

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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."