Problem: The Henry’s law constant for oxygen gas in water at 25 °C, kH is 1.3×10-3M/atm. What is the partial pressure of O2 above a solution at 25 °C with an O2 concentration of 2.3×10-4 M at equilibrium?A. 0.18 atm B. 5.7 atmC. 1.3 x 10-3 atmD. 2.3 x 10-4 atmE. 3.0 x 10-7 atm

FREE Expert Solution

We’re being asked to calculate the partial pressure of O2 above a solution at 25 °C


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


Sgas=kH·Pgas


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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Problem Details

The Henry’s law constant for oxygen gas in water at 25 °C, kH is 1.3×10-3M/atm. What is the partial pressure of O2 above a solution at 25 °C with an O2 concentration of 2.3×10-4 M at equilibrium?

A. 0.18 atm 

B. 5.7 atm

C. 1.3 x 10-3 atm

D. 2.3 x 10-4 atm

E. 3.0 x 10-7 atm

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