+ The Effect of Pressure on Solubility ?) 5of15 (> Part B The solubility of gas

Question

+ The Effect of Pressure on Solubility ?) 5of15 (> Part B The solubility of gas in a liquid is profoundly affected by pressure. This relation is expressed by Henry's law, which states that the solubility of a gas in a liquid, expressed in moles per liter (or M), at a given temperature is directly proportional to the partial pressure of the gas over the solution. This relation can be expressed mathematically as As a scuba diver descends under water, the pressure increases. At a total air pressure of 2.84 atm and a temperature of 25.0 C, what is the solubility of N2 in a divers blood? [Use the value of the Henry's law constant k calculated in Part A,6.26 x 10-4 mol/(L atm)J 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 solubility k-P The constant k is characteristic of the specific gas and P is the partial pressure of the gas over the solution usually expressed in atmospheres. The constant k usually has units of moles per liter per atmosphere and is reported at 25 C. This expression can be used to calculate any of the three variables provided that the other two are known for any gas. View Available Hint(s) solublity Value Units Submit Previous Answers X Incorrect; Try Again; 4 attempts remaining

Explanation / Answer

Part b

Nitrogen % in air = 78%

Partial pressure of N2 P = 0.78 x 2.84 = 2.2152 atm

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

Solubility = k * P

= (6.26*10^-4 mol/L-atm) * (2.2152 atm)

= 0.0013867152 mol/L

= 1.38*10^-3 mol/L

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