|MadSci Network: Engineering|
It is difficult to give you an exact answer because the pressure depends on a couple of different factors - the most important of which are the temperature of the soda and the amount of carbon dioxide that was put into the beverage in the first place. To give you a quick example, let's say that the soda was carbonated to 3.0 volumes of CO2 and it has been sitting in your refrigerator so it's around 40 degrees F. The pressure inside the can will be roughly 17 psig (pounds per square inch, gauge) above atmospheric pressure. If you let the can warm up on the counter so its temperature increases to 70 F or so, the pressure inside the can will have increased to about 36 psig. If you'd like to learn more about pressure/temperature relationships, try researching the Ideal Gas Law in almost any general chemistry reference. I haven't actually done the calculation, but the carbonation is probably behaving according to PV=nRT. Try the numbers I just gave you and see if it works out. ;) Thanks for your question! Kieran
Try the links in the MadSci Library for more information on Engineering.