The Henry’s law constant at 25°C for nitrogen dissolved in water is 8.57 × 104 atm, that for oxygen is 4.34 × 104 atm, and that for helium is 1.7 × 105 atm. (a) Calculate the number of moles of nitrogen and oxy- gen dissolved per liter of water in equilibrium with air at 25°C. (b) Air is dissolved in blood and other bodily luids. As a deep-sea diver descends, the pressure increases and the concentration of dissolved air in the blood increases. If the diver returns to the surface too quickly, gas bubbles out of solution within the body so rapidly that it can cause a dangerous condition called “the bends.” Use Henry’s law to show why divers some- times use a combination of helium and oxygen in their breathing tanks in place of compressed air.
The Henry’s law constant at 25°C for nitrogen dissolved in water is 8.57 × 104 atm, that for oxygen is 4.34 × 104 atm, and that for helium is 1.7 × 105 atm. (a) Calculate the number of moles of nitrogen and oxy- gen dissolved per liter of water in equilibrium with air at 25°C. (b) Air is dissolved in blood and other bodily luids. As a deep-sea diver descends, the pressure increases and the concentration of dissolved air in the blood increases. If the diver returns to the surface too quickly, gas bubbles out of solution within the body so rapidly that it can cause a dangerous condition called “the bends.” Use Henry’s law to show why divers some- times use a combination of helium and oxygen in their breathing tanks in place of compressed air.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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The Henry’s law constant at 25°C for nitrogen dissolved in
water is 8.57 × 104 atm, that for oxygen is 4.34 × 104 atm,
and that for helium is 1.7 × 105 atm.
(a) Calculate the number of moles of nitrogen and oxy-
gen dissolved per liter of water in equilibrium with air at 25°C.
(b) Air is dissolved in blood and other bodily luids. As a
deep-sea diver descends, the pressure increases and the concentration of dissolved air in the blood increases. If the diver returns to the surface too quickly, gas bubbles out of solution within the body so rapidly that it can cause a dangerous condition called “the bends.” Use Henry’s law to show why divers some- times use a combination of helium and oxygen in their breathing tanks in place of compressed air.
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