Editing Partial pressure (section)

==Dalton's law of partial pressures==
{{main|Dalton's law}}
[[File:Schematic Depicting Dalton's Law-en.svg|thumb|Schematic showing the concept of Dalton's Law.]]
Dalton's law expresses the fact that the total pressure of a mixture of ideal gases is equal to the sum of the partial pressures of the individual gases in the mixture.<ref>[http://www.chm.davidson.edu/vce/gaslaws/daltonslaw.html Dalton's Law of Partial Pressures]</ref> This equality arises from the fact that in an ideal gas, the molecules are so far apart that they do not interact with each other. Most actual real-world gases come very close to this ideal. For example, given an ideal gas mixture of [[nitrogen]] (N<sub>2</sub>), [[hydrogen]] (H<sub>2</sub>) and  [[ammonia]] (NH<sub>3</sub>):

<math chem display="block">p = p_\ce{N2} + p_\ce{H2} + p_\ce{NH3}</math>
where:
*<math>p </math> = total pressure of the gas mixture
*<math chem>p_\ce{N2}</math> = partial pressure of nitrogen (N<sub>2</sub>)
*<math chem>p_\ce{H2}</math> = partial pressure of hydrogen (H<sub>2</sub>)
*<math chem>p_\ce{NH3}</math> = partial pressure of ammonia (NH<sub>3</sub>)