In a gaseous mixture, how does #P_"Total"# relate to the individual partial pressures, i.e. #P_1#, #P_2#...#P_n# exerted by each gaseous component?

1 Answer
anor277
Dec 30, 2016

I am not quite sure that you have grasped the issue.........

Explanation:

In a gaseous mixture, the partial pressure, #P_1#, exerted by a component gas is the same as the pressure it would exert if it alone occupied the containers. The total pressure, #P_"total"# is the sum of the individual partial pressures.

#P_"total"=P_1+P_2+..........P_n#

But if we use the Ideal Gas Equation:

#P_"total"=(n_"total"RT)/V#

#=(RT)/V{n_1+n_2+.....................+n_n}#

And the partial pressure of a component gas is thus simply,

#n_i/{n_1+n_2+.....................n_n}xxP_"total"#

If I have missed the direction of your question, please qualify it.

Related questions
See all questions in Partial Pressure
Impact of this question
1676 views around the world
You can reuse this answer
Creative Commons License