At ordinary body temperature the solubility of N2 in water in contact with air at
Chapter 19, Problem 13.107(choose chapter or problem)
At ordinary body temperature the solubility of N2 in water in contact with air at ordinary atmospheric pressure (1.0 atm) is . Air is approximately . Calculate the number of moles of N2 dissolved per liter of blood,which is essentially an aqueous solution.At a depth of 100 ft in water,the pressure is 4.0 atm.What is the solubility of N2 from air in blood at this pressure? 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?
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