Deep-sea divers can suffer a condition known as the "bends" if they breathe ordinary air at a pressure equal to the ambient hydro static pressure, because nitrogen gas dissolves in blood at high pressure and is released as bubbles in the bloodstream when the diver decompresses.
A. How many moles of N2 are dissolved in 5.00L of water (roughly the volume of blood in an adult human) if the water is in equilibrium with air at 1.00 atm?
The mole fraction of N2 in air is 78.09% and the Henry's law constant for N2 in water is 1.08*10^5 atm at 37°C. The density of pure water (MW 18.015) at this temperature is .9933 g/mL.
B. How many moles of N2 are dissolved in 5.00L of water if the water is in equilibrium with air at 5.84 atm (approximately the hydrostatic pressure at a depth of 50m) at 37°C?
C. If the extra N2 dissolved in the blood at 5.84 atm pressure of air (compared with 1.00 atm) is released as pure N2 gas at 37°C and 1.00 atm pressure, what volume would it occupy? (assume ideal gas behavior)