Beer Coke
Beer Coke
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If you put a sealed drink in the freezer (beer...coke) why is it that it does not freeze...?
...until it is opened or shook?
Example I put a beer in the freezer to get it ice cold. I take it out and you can plainly see it is not frozen. You then open the bottle and take a drink and the beer instantly freezes into slush. I have found that if I warm the bottle slightly with my hands and then take slow drinks as to not upset the beer you can keep it from freezing. Swish it in your mouth for a second and it freezes in your mouth. What is the science behind this?
At first, I thought that the answer to this question was obvious. However, after further thought and investigation, I realized that there are several processes at work all of varying degrees of significance. The tough thing to decide is probably which process is most significant.
A few important facts to note in analyzing this problem.
1. Beer bottles/cans and soda bottles/cans are pressurized.
2. They all contain solutes in the solvent, water.
3. Both contain the solute CO2, carbon dioxide.
Most solutes will lower the freezing point of solvents when they are combined into a homogeneous mixture. In this case, we have carbon dioxide, the solute, dissolved into water, the solvent. Dissolved carbon dioxide in water will, in fact, lower the freezing point of the solution below 0 C.
For beer, there are a few more solutes than carbon dioxide such as alcohol and various salts, but they all act to lower the freezing point of the solution relative to that of water. I read that -0.42 * (percent alcohol by volume) degrees C is accurate. That is, 1 percent of alcohol dissolved in water will lower the freezing point by 0.42 C and the relationship is linear. (I won't really back this up because I didn't get access to the journal article that finds this. The information is out there, though.)
That said, the pressurized bottles and cans keep the carbon dioxide in the solution as the bottles and cans are cooled. This in turn lowers the freezing point of the solution below that of water 0 C. For cream soda, it's about -10 C. If the freezer is cool enough, this solution will freeze too. But since most household freezers are kept around 0 C, this tends not to happen. When the bottle is opened, there is a pressure differential between the outside environment and inside the bottle. Typically bottles are pressurized around 5 atmospheres (http://www.newton.dep.anl.gov/askasci/gen01/gen01625.htm). So as the pressure inside the bottle equilibrates with the environment, it lowers, thereby releasing carbon dioxide from the solution.* This has a three-pronged effect.
(1) First dissolved solute leaves the solution thereby *raising* its freezing temperature.
(2) Second the gaseous bubbles of carbon dioxide forming in the solution expand adiabatically (to very good approximation) and under a constant pressure for the solution. Therefore, the escaping gas bubbles temperatures increase, while the solution cools. (T_initial/V_initial = T_final/V_final)
(3) Thirdly, the escaping bubbles agitate the now supercooled solution providing for nucleation sites for crystal growth.**
*This is basic chemistry. If a gas is in contact with an incompressible liquid, and the pressure on the gas is increased, more gas is going to be able to stay in solution with the liquid at equilibrium.
**This probably warrants more explanation. A solution is called supercooled when its temperature is below its freezing point yet remains a liquid. Similarly, a solution is called superheated when its temperature is above its boiling point yet still a liquid. The beer or soda is essentially supercooled after the carbon dioxide leaves the solution and it doesn't freeze. All crystallization processes (of which water freezing is one) require a nucleation point; some place to begin. The carbon dioxide bubbles leaving solution are generating these nucleation points for crystal growth. Suspended particles in solution can provide nucleation sites, but these tend not to be present in soda and beer. (http://en.wikipedia.org/wiki/Nucleation)
When just shaking the can or bottle without having opened it, the agitation increases the entropy of the solution thereby releasing carbon dioxide sufficiently so that (1), (2), and (3) may also occur.
Lastly, I used the ideal gas law PV = nRT and the fact that the beer and soda are very good approximations to incompressible fluids to verify this. I believe for water it takes 135 atm to lower its freezing point by 1 C, so incompressible. So the math is there, and I'd be happy to discuss it.
