# 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:

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

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

99% (15 ratings) ###### 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