Suppose Gabor, a scuba diver, is at a depth of 15 m. Assume that: 1. The air pressure in his air tract is the same as the net water pressure at this depth. This prevents water from coming in through his nose. 2. The temperature of the air is constant (body temperature). 3. The air acts as an ideal gas. 4. Salt water has an average density of around 1.03 g/cm^3, which translates to an increase in pressure of 1.00 atm for every 10.0 m of depth below the surface. Therefore, for example, at 10.0 m, the net pressure is 2.00 atm. If the temperature of air in Gabor's lungs is 37 Celsius and the volume is 6 L, how many moles of air n must be released by the time he reaches the surface? Let the molar gas constant be given by R = 8.31 J/ (mol*K) _________________________________ I know that the number of moles of air in 6L at the underwater pressure of is 0.006(?) Now I know that the difference between this and the moles of air in the lungs that I calculate at the surface pressure gives me my answer but how do I know what the conditions are at the surface? am I just approaching this problem in an incorrect way?? Thanks in advance..