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.

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