Question

At ordinary body temperature (37 °C), the solubility of N₂ in water at ordinary atmospheric pressure (1.0 atm) is 0.015 g/L. Air is approximately 78 mol % N₂. (a) Calculate the number of moles of N₂ dissolved per liter of blood, assuming blood is a simple aqueous solution. (b) At a depth of 100 ft in water, the external pressure is 4.0 atm. What is the solubility of N₂ from air in blood at this pressure? (c) If a scuba diver suddenly surfaces from this depth, how many milliliters of N₂ gas, in the form of tiny bubbles, are released into the bloodstream from each liter of blood?