As a scuba diver descends under water, the pressure increases. At a total air pressure of 2.73 atm and a temperature of 25.0 ∘C, what is the solubility of N2 in a diver's blood?[Use the value of the Henry's law constant k calculated in Part A, 6.26*10-4mol / (L⋅atm).]Assume that the composition of the air in the tank is the same as on land and that all of the dissolved nitrogen remains in the blood.

1.33 x 10⁻³ mol/L

Explanation:

The solubility of a gas in a liquid is directly proportional to its partial pressure. This is know as Henry's law and is given by the formula:

S (g) = Kh x P

where S = solubility of the gas

Kh = henry's constant for the gas

P = partial pressure of the gas above solution

we are told to assume that the composition of the air in the tank is the same as on land, hence its partial pressure and we know nitrogen composition in air is 78 %, so the partial pressure of N₂ is:

P N₂ = 0.78 x 2.73 atm = 2.13 atm

Now we can calcualte the solubility as follows:

S N₂ = 6.26 x 10⁻⁴ mol / L·atm x 2.13 atm = 1.33 x 10⁻³ mol / L