At ordinary body temperature (37 C) the solubility of n_2 in water in contact with air at ordinary atmospheric pressure (1.0 atm) is 0.015 g/l. Air is approximately 78 mol % N_2.
a) Calculate the number of moles of N_2 dissolved per liter of blood, which is essentially an aqueous solution.
b) At a depth of 100ft in water, the pressure is 4.0 atm. What is the solubility of N_2 from air in blood at this pressure?
c) If a scuba diver suddenly surfaces from this depth, how many milliliters of N_2 gas, in the form of tiny bubbles, are released into the bloodstream from each liter of blood?