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Answer to Question #63251 in General Chemistry for Lauren
Question #63251
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?
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?
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