Air is a mixture of gases that is about 78.0% N2 by volume. When air is at stand

Question

Air is a mixture of gases that is about 78.0% N2 by volume. When air is at standard pressure and 25.0 C, the N2 component will dissolve in water with a solubility of 4.88×104 M. What is the value of Henry's law constant for N2 under these conditions?

Express your answer with the appropriate units. Enter the unit M using the compound form mol/L.

6.26×104 molLatm

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Part B

As a scuba diver descends under water, the pressure increases. At a total air pressure of 2.58 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, 6.26×104mol/(Latm).]

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.

6.26×104 molLatm

Explanation / Answer

According to Henry's law constant,

Solubility of gas = Henry's law constant * Parptial above the solution

4.88 * 10-4 = k * (1 * 78/100)

k = Henry's law constant = 6.26 * 10-4 mol/L.atm

PART (B)

Solubility = 6.26 * 10-4 * (2.58*78/100)

Solubility of N2 under new pressure = 1.26 * 10-3 mol/L

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