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
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter11: Properties Of Solutions
Section: Chapter Questions
Problem 58E: Calculate the solubility of O2 in water at a partial pressure of O2 of 120 torr at 25C. The Henrys...
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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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