Editing Humidity (section)

== Air density and volume ==
{{Main article|Volume (thermodynamics)|Density of air|Ideal gas law}}

Humidity depends on water vaporization and condensation, which, in turn, mainly depends on temperature. Therefore, when applying more pressure to a gas saturated with water, all components will initially decrease in volume approximately according to the ''ideal gas law''. However, some of the water will condense until returning to almost the same humidity as before, giving the resulting total volume deviating from what the ideal gas law predicted. 

Conversely, decreasing temperature would also make some water condense, again making the final volume deviate from predicted by the ideal gas law. Therefore, gas volume may alternatively be expressed as the dry volume, excluding the humidity content. This fraction more accurately follows the ideal gas law. On the contrary the saturated volume is the volume a gas mixture would have if humidity was added to it until saturation (or 100% relative humidity).

Humid air is less dense than dry air because a molecule of water ({{nowrap|[[Molecular mass|''m'']] ≈ {{val|18|ul=Da}}}}) is less massive than either a molecule of nitrogen ({{nowrap|''m'' ≈ 28}}) or a molecule of oxygen ({{nowrap|''m'' ≈ 32}}). About 78% of the molecules in dry air are nitrogen (N<sub>2</sub>). Another 21% of the molecules in dry air are oxygen (O<sub>2</sub>). The final 1% of dry air is a mixture of other gases.

For any gas, at a given temperature and pressure, the number of molecules present in a particular volume is constant.  Therefore, when some number N of water molecules (vapor) is introduced into a volume of dry air, the number of air molecules in that volume must decrease by the same number N for the pressure to remain constant without using a change in temperature. The numbers are exactly equal if we consider the gases as [[ideal gas|ideal]]. The addition of water molecules, or any other molecules, to a gas, without removal of an equal number of other molecules, will necessarily require a change in temperature, pressure, or total volume; that is, a change in ''at least'' one of these three parameters.  

If temperature and pressure remain constant, the volume increases, and the dry air molecules that were displaced will initially move out into the additional volume, after which the mixture will eventually become uniform through diffusion.  Hence the mass per unit volume of the gas—its density—decreases. Isaac Newton discovered this phenomenon and wrote about it in his book ''[[Opticks]]''.<ref name="optics">
{{cite book
 |author=Isaac Newton
 |url=https://books.google.com/books?id=iTpXLrPR2TQC&q=isaac+newton+optics
 |publisher=Dover
 |title=Opticks
 |year=1704
 |isbn=978-0-486-60205-9
}}
</ref>