State and explain Dalton's law of partial pressure.

(N/A) Law: The total pressure exerted by a mixture of non-reacting ideal gases is equal to the sum of the partial pressures of the individual gases.
Let the volume of the container be $V$ and the temperature of the gases be $T$. Let the total pressure of the mixture be $P$.
Let the number of moles of the individual gases be $\mu_{1}, \mu_{2}, \ldots, \mu_{n}$.
The total number of moles is $\mu = \mu_{1} + \mu_{2} + \ldots + \mu_{n}$.
According to the ideal gas equation,$PV = \mu RT$.
Substituting the total moles: $PV = (\mu_{1} + \mu_{2} + \ldots + \mu_{n}) RT$.
Therefore,$P = \frac{\mu_{1} RT}{V} + \frac{\mu_{2} RT}{V} + \ldots + \frac{\mu_{n} RT}{V}$.
Since the partial pressure of an individual gas $i$ is defined as $P_{i} = \frac{\mu_{i} RT}{V}$,we get:
$P = P_{1} + P_{2} + \ldots + P_{n}$.
Thus,in a mixture of non-interacting gases,the total pressure of the mixture is equal to the sum of the partial pressures of the individual gases.