What does Dalton's law of partial pressure mean?

Aug 15, 2016

It means we can solve problems like this one.

Explanation:

And in a gaseous mixture, the partial pressure exerted by a component gas is the same as the pressure it would exert if that component ALONE had occupied the container. The total pressure is the sum of the individual partial pressures.

${P}_{\text{Total}}$ $=$ ${P}_{1} + {P}_{2} + {P}_{3} + \ldots \ldots \ldots \ldots \ldots . + {P}_{n}$

But if we assume ideality, then $P = \frac{n R T}{V}$

And thus,

${P}_{\text{Total}}$ $=$ $\frac{{n}_{1} R T}{V} + \frac{{n}_{1} R T}{V} \ldots \ldots \ldots \ldots . \frac{{n}_{n} R T}{V}$

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

$=$ $\frac{R T}{V} \cdot \Sigma {n}_{i}$, where ${n}_{i}$ is the amount in moles of each particular gas.

Is this for what you were looking?