Arterial blood contains about 0.25 g of oxygen per liter at 37°C and standard atmospheric pressure. Under these conditions, the Henry's law constant is kH = 3.7 ×× 10–2 mol/(L • atm), and the mole fraction of O2 in the atmosphere is 0.209.Part1:Calculate the solubility (in M) of O2 in the blood of a climber on Mt. Everest, where Patm = 0.35 atm.___MPart2: Calculate the solubility (in M) of O2 in the blood of a scuba diver at a depth of 100 feet, where Patm = ~3 atm.___M

Given: Henry's constant , kH = 3.7 × 10–2 mol/(L • atm) mole fraction of O2 = 0.209

Answered: Arterial blood contains about 0.25 g of…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter12: Solutions

Section: Chapter Questions

Problem 12.52QE

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Arterial blood contains about 0.25 g of oxygen per liter at 37°C and standard atmospheric pressure. Under these conditions, the Henry's law constant is k_H = 3.7 ×× 10^–2 mol/(L • atm), and the mole fraction of O₂ in the atmosphere is 0.209.

Part1:Calculate the solubility (in M) of O₂ in the blood of a climber on Mt. Everest, where P_atm = 0.35 atm.___M

Part2: Calculate the solubility (in M) of O₂ in the blood of a scuba diver at a depth of 100 feet, where P_atm = ~3 atm.___M

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