# 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?

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, ${P}_{\text{total}}$ is the sum of the individual partial pressures.

${P}_{\text{total}} = {P}_{1} + {P}_{2} + \ldots \ldots \ldots . {P}_{n}$

But if we use the Ideal Gas Equation:

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

$= \frac{R T}{V} \left\{{n}_{1} + {n}_{2} + \ldots \ldots \ldots \ldots \ldots \ldots \ldots + {n}_{n}\right\}$

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

${n}_{i} / \left\{{n}_{1} + {n}_{2} + \ldots \ldots \ldots \ldots \ldots \ldots \ldots {n}_{n}\right\} \times {P}_{\text{total}}$

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