A flask contains helium at #752*"Torr"#, and a second flask contains argon at #712*"Torr"#. What are the partial pressures of each gas in each flask?

1 Answer
Dec 4, 2016

#P_"He"=752*"Torr"#. #P_"Ar"=712*"Torr"#


In a gaseous mixture, the partial pressure exerted by 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.

Here, you have 2 flasks, and each flask contains the ONE gas, each with a specified pressure. We simply read off the partial pressures for each flask.

See here for a similar problem.