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# Solution: The Henry's law constant (k H) for O2 in water at 20°C is 1.28 x 10 -3 mol/L•atm. How many grams of O2 will dissolve in 1.75 L of H 2O in contact with air, where the partial pressure of O2 is 1.32 atm?A. 0.0541 gB. 0.0473 gC. 0.0946 gD. 0.0270 gE. 0.946 g

###### Problem

The Henry's law constant (k H) for O2 in water at 20°C is 1.28 x 10 -3 mol/L•atm. How many grams of O2 will dissolve in 1.75 L of H 2O in contact with air, where the partial pressure of O2 is 1.32 atm?

A. 0.0541 g

B. 0.0473 g

C. 0.0946 g

D. 0.0270 g

E. 0.946 g

###### Solution

We’re being asked to determine the mass of O2 that will dissolve in 1.75 L H2O.

Recall that the solubility of a gas is given by Henry’s law:

$\overline{){{\mathbf{S}}}_{{\mathbf{gas}}}{\mathbf{=}}{{\mathbf{k}}}_{{\mathbf{H}}}{\mathbf{·}}{{\mathbf{P}}}_{{\mathbf{gas}}}}$

where:

Sgas = solubility of the gas (in mol/L or M)

kH = Henry’s law constant for the gas

Pgas = partial pressure of the gas

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