Chapter 12, Problem 98RQ

The “bends” is a medical emergency caused by the formation of tiny bubbles in the blood vessels of divers who rise too quickly to the surface from a deep dive. At $\text{37 °C}$

(normal body temperature), the solubility of ${\text{N}}_{\text{2}}$ in water is $\text{0}{\text{.015 g L}}^{\text{-1}}$ when its pressure over the solution is 1 atm. Air is approximately 78 mol% ${\text{N}}_{\text{2}}$. How many moles of ${\text{N}}_{\text{2}}$ are dissolved per liter of blood (essentially an aqueous solution) when a diver inhales air at a pressure of 1 atm? How many moles of ${\text{N}}_{\text{2}}$ dissolve per liter of blood when the diver is submerged to a depth of approximately 100 ft, where the total pressure of the air being breathed is 4 atm? If the diver suddenly surfaces, how many milliliters of ${\text{N}}_{\text{2}}$ gas, in the form of tiny bubbles, are released into the bloodstream from each liter of blood (at $\text{37 °C}$ and 1 atm)?