Dalton's law
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In chemistry and physics, Dalton's law (also called Dalton's law of partial pressures) states that the total pressure exerted by a gaseous mixture is equal to the sum of the partial pressures of each individual component in a gas mixture. This empirical law was observed by John Dalton in 1801 and is related to the ideal gas laws
Mathematically, the pressure P of a mixture of n gases can be defined as the summation
or 
where 
represent the partial pressure of each component.
It is assumed that the gases do not react with each other.
Combining Dalton's Law with Boyle's and Avogadro's laws leads to the conclusion that a gas in an ideal gas mixture exerts a partial pressure whose ratio to total pressure equals its mole fraction.
where 
the mole fraction of the i-the component in the total mixture of m components
The relationship below provides a way to determine the volume based concentration of any individual gaseous component.
where: 
is the concentration of the ith component expressed in ppm.
Dalton's law is not exactly followed by real gases. Those deviations are considerably large at high pressures. In such conditions, the volume occupied by the molecules can become significant compared to the free space between them. Moreover, the short average distances between molecules raises the intensity of intermolecular forces between gas molecules enough to substantially change the pressure exerted by them. Neither of those effects are considered by the ideal gas model.
