In order for soda pop to be fizzy, there is excess carbon dioxide (CO) that is added under pressure. This added pressure will force some of the CO to dissolve in the pop. The CO that did not dissolve will be considered excess and comes out when the bottle or can is opened. Your purpose for this experiment is to use the Ideal Gas Law and find the pressure (P) of the CO in the small space above the liquid that is in an unopened bottle or can of pop. You will need to write your own set of procedures to determine the factors in PV=nRT that are needed to solve for P. The value R, the Universal Gas Constant, is 0.0821 L.atm/(mol K). The other parameters V, n, and T must be determined by the set of procedures that you develop