A submarine has run into trouble and is stuck at the bottom of the ocean. Several people are on board and must make their way to the surface without any diving gear. The air pressure aboard the submarine is 3.000 atm. The air temperature inside the submarine is 18.02 °C and you can take body temperature (inside the lungs) to be 36.04 °C. 1. The second person to leave also takes a breath as deep as possible by exhaling as far as possible (leaving a volume of 1.190 L in their lungs), and then slowly inhaling to increase their lung volume by 4.080 L. His body temperature is also 36.04 °C. This person breathes out all the way to the surface in order to maintain a constant lung volume. How many moles of gas remain in the lungs? Relevant equations: PV = nRT The attempt at a solution: i found the total volume of the lungs to be Vtotal = 1.190L + 4.080L = 5.270L = 0.005270m^3 and using PV = nRT i found the number of moles at full capacity lungs (3.00 x 101300)(0.005270) = n(8.314)(36.04+273.15) n = 0.6230 moles then i found the number of moles when the person exhales using PV = nRT (3.00 x 101300)(0.004080 - 0.001190) = n(8.314)(36.04+273.15) n = 0.365 ∴ the change in moles is n = 0.6230 - 0.341 = 0.281mols BUT the actual answer is 0.208 mols and i don't know what i'm doing wrong HELP!!