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Calculate the mass of oxygen (in mg) dissolved in a 2.50 L bucket of water exposed to a pressure of 2.13 atm of air. Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 × 10-3 M/atm. Molar mass for oxygen (O2) is 31.9988 g/mol. A. 46.5 mg B. 27.0 mg C. 13.7 mg D. 23.5 mg E. 9.87 mg

Calculate the mass of oxygen (in mg) dissolved in a 2.50 L bucket of water exposed to a pressure of 2.13 atm of air. Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 × 10-3 M/atm. Molar mass for oxygen (O2) is 31.9988 g/mol. A. 46.5 mg B. 27.0 mg C. 13.7 mg D. 23.5 mg E. 9.87 mg

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter13: The Chemistry Of Solutes And Solutions
Section: Chapter Questions
Problem 106QRT: Calculate the molality of a solution made by dissolving 115.0 g ethylene glycol, HOCH2CH2OH, in 500....
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Calculate the mass of oxygen (in mg) dissolved in a 2.50 L bucket of water exposed to a pressure of 2.13 atm of air.  Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 × 10-3 M/atm. Molar mass for oxygen (O2) is 31.9988 g/mol.

 

  A.

46.5 mg
  B.

27.0 mg
  C.

13.7 mg
  D.

23.5 mg
  E.

9.87 mg
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