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The atmospheric pressure is 1.0 atm and Henry’s law constant for O2 is 1.66 x 10−6 M/mm Hg at 25 °C. Assume air contains 21% oxygen. Calculate the partial pressure of oxygen. (21% of air is oxygen and the mole fraction of O2 is 0.21).

The atmospheric pressure is 1.0 atm and Henry’s law constant for O2 is 1.66 x 10−6 M/mm Hg at 25 °C. Assume air contains 21% oxygen. Calculate the partial pressure of oxygen. (21% of air is oxygen and the mole fraction of O2 is 0.21). Correct Answer 160 mm Hg

The partial pressure of oxygen is: P (O2) = (1.0 atm) ((760 mm Hg)/(1 atm)) (0.21) = 160 mm Hg.

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