Answer to Question #63251 in General Chemistry for Lauren

Question

Chapter 13 (13.107)

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.

1) Calculate the number of moles of N2 dissolved per liter of blood, assuming blood is a simple aqueous solution.

2) 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?

3) 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?