As a scuba diver descends under water, the pressure increases. at a total air pressure of 2.85 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. express your answer with the appropriate units.

Question

Chemistry

Allen Morrow

4 October, 08:37

As a scuba diver descends under water, the pressure increases. at a total air pressure of 2.85 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. express your answer with the appropriate units.

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Corey Haas · Answer 1

Henry's Law is written in equation as:

C = kP

where

C is the concentration

k is the Henry's law constant

P is the partial pressure

This law is applied to soluble gases in liquids. At a certain temperature, there is a specific value of the Henry's Law constant. The C represents the solubility. Hence, we solve for C.

C = (6.26*10 ⁻⁴ mol / (L⋅atm)) * (2.85 atm)

C = 0.0017841 mol/L