Henry's Law
William Henry was an English chemist that lived in the late 18th century. His work with gas analysis lead to the development of what would come to be known as Henry's Law.
HENRY'S LAW
p=khC
Where:
c= the concentration of the solute (mol/L)
kh=Henry's Constant, : 29.4 for CO2 at 289K (60.53°F) (L·atm/mol)
Note: kh is actually a changing coefficient that changes rather than a constant. It changes with respect to temperature using this equation: kh = kh,ref Tref.exp(-C.((1/T) - (1/Tref))) This is important when carbonating beer because it will determine how much carbon dioxide get absorbed into the beer.
This relationship tells us that for higher pressures of gas you will get higher concentrations of gas in your solution. This is how the CO2 gets into the beer. Now where does the CO2 come from? There are two different sources for carbon dioxide in beer.
Natural Carbonation
When yeast is put in a solution containing sugar it begins to "eat" causing a chemical reaction producing carbon dioxide and ethanol, two key ingredients in beer creation.
- REACTION: C6H12O6 → 2 CO2 + 2 C2H5OH
Forced Carbonation
The process of forced carbonation is very similar to natural but instead of the yeast creating the and the pressurized CO2, a bottle of liquefied gas is used to create the artificial pressure and carbonate the beer.
Dry Ice Carbonation
I have never actually heard of someone doing this with beer but I thought I would put it on here anyway. You can drop a small brick of dry ice (Frozen carbon dioxide) into a sealed container and have it pressurize that way NOT RECOMMENDED because the amount of pressure you get harder to predict and could cause an exploding bottle/keg.