A gaseous mixture of radon, dinitrogen, and helium has a pressure of #771*mm*Hg#. If #P_"radon"=222*mm*Hg#, and #P_"dinitrogen"=446*mm*Hg#, what is #P_"helium"# in units of #"Torr"#?

1 Answer
anor277
Nov 28, 2017

#P_"Total"=P_(Rn)+P_(N_2)+P_(He)#...and we note that #"1 mm Hg "-=" 1 Torr"#...

Explanation:

This is a straight application of Dalton's Law of Partial Pressures. The partial pressure exerted by an individual gas in a gaseous mixture 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.

And so #P_"Total"-P_(Rn)-P_(N_2)=P_(He)#

#P_"He"={771-222-446}=103*"Torr"#

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