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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 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.___M Part2: 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

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.___M

Part2: 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

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