# Problem: At 298 K, the Henry's law constant for oxygen is 0.00130 M/atm. Air is 21.0% oxygen.1) At 298 K, what is the solubility of oxygen in water exposed to air at 1.00 atm2) At 298 K, what is the solubility of oxygen in water exposed to air at 0.89 atm?3) If atmospheric pressure suddenly changes from 1.00 atm to 0.893 atm at 298 K, how much oxygen will be released from 4.70L of water in an unsealed container?

###### FREE Expert Solution

We’re being asked to determine the solubility of O2 in water. Recall that the solubility of a gas is given by Henry’s law:

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

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. ###### Problem Details

At 298 K, the Henry's law constant for oxygen is 0.00130 M/atm. Air is 21.0% oxygen.

1) At 298 K, what is the solubility of oxygen in water exposed to air at 1.00 atm

2) At 298 K, what is the solubility of oxygen in water exposed to air at 0.89 atm?

3) If atmospheric pressure suddenly changes from 1.00 atm to 0.893 atm at 298 K, how much oxygen will be released from 4.70L of water in an unsealed container?