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
anor277
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=??#

For more spray, see here and links.

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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