Ask Question
2 August, 13:21

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
Answers (1)
  1. 2 August, 16:53
    0
    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
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “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 ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers