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Calculate the mass of oxygen gas (O2) dissolved in a 5.00 L bucket of water exposed...

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Chemistry

Calculate the mass of oxygen gas (O2) dissolved in a5.00 L bucket of water exposed to a pressure of 1.13 atm of air.Assume the mole fraction of oxygen in air to be 0.210 and theHenry's law constant for air in water at this temperature to be1.30 × 10-3 M/atm.

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4.2 Ratings (763 Votes)

partial pressure of O2 = mole fraction x total pressure

                                       = 0.210 x 1.13

                                       = 0.2373 atm

Henry's law constant = 1.30 × 10^-3 M/atm.

concentration of O2 = 1.30 × 10^-3 x 0.2373

                                   = 3.085 x 10^-4 M

Molarity = moles / volume

3.085 x 10^-4 = moles / 5

moles of O2 = 1.54 x 10^-3

moles = mass / molar mass

1.54 x 10^-3 = mass / 32

mass of O2 = 0.0493 g
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