at 298 k, the Henry's law constant for oxygen is 0.00130 M/atm. Air is 21.0% oxygen. at 298 k, what is the solubility of oxygen in water exposed to air at 1.00 atm?
21.0% oxygen is 21 mole percent.
0.00130 M/atm x 0.21 atm = ??M
2.73 x 10^-4
To find the solubility of oxygen in water exposed to air at 1.00 atm, we need to consider Henry's law. Henry's law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid.
Given:
Henry's Law constant (kH) for oxygen = 0.00130 M/atm
Partial pressure of oxygen in air (P_O2) = 1.00 atm
We are also given that air is 21.0% oxygen. This means that the partial pressure of oxygen in air (P_O2air) can be calculated as follows:
P_O2air = 21.0% * 1.00 atm
P_O2air = 0.21 atm
Now, we can use Henry's law equation:
Solubility of oxygen (S_O2) = kH * P_O2air
Substituting the given values:
S_O2 = 0.00130 M/atm * 0.21 atm
S_O2 ≈ 0.000273 M/atm
Therefore, the solubility of oxygen in water exposed to air at 1.00 atm is approximately 0.000273 M/atm.
To determine the solubility of oxygen in water, we need to use Henry's law.
Henry's law relates the concentration of a gas in a liquid to the partial pressure of that gas above the liquid. The equation is:
C = k * P
Where:
C is the concentration of the gas in the liquid (in this case, oxygen in water)
k is Henry's law constant for the gas at a given temperature
P is the partial pressure of the gas above the liquid.
In this case, we know the Henry's law constant for oxygen at 298 K is 0.00130 M/atm, and the partial pressure of oxygen in air is determined by its mole fraction.
Given that air is 21.0% oxygen, we can calculate the partial pressure of oxygen (P) in air at 1.00 atm as follows:
Partial Pressure of Oxygen (P) = Total Pressure of air (1.00 atm) * Mole Fraction of Oxygen (0.21)
P = 1.00 atm * 0.21
Now, we can substitute the values into Henry's law equation to calculate the solubility of oxygen (C):
C = k * P
C = 0.00130 M/atm * (1.00 atm * 0.21)
By multiplying the values, we can find the solubility of oxygen in water exposed to air at 1.00 atm.