The concentration of N in blood at 37 C (body temperature) and atmospheric pressure (partial pressure of N = 0.80 atm) is 0.00056 mol/L. A deep-sea diver breathes compressed air with the partial pressure of N equal to 4.0 atm. Calculate the volume (at 37C and atmospheric pressure (p(N) = 0.80 atm) of N gas released as a diver surfaces. Assume that the total volume of blood in the body is 5.0 L. *Think of the carbonation of a soda bottle (the diver) under pressure in a sealed can compared to a flat soda. Essentially you are calculating how much nitrogen a diver has to exhale as he surfaces in order to avoid getting the bends. **From Chem 105, PV = nRT, R = 0.08206 (L*atm)/(mol*K)