Calculate the number of moles of N2 dissolved per liter of blood. assuming blood

Question

Calculate the number of moles of N2 dissolved per liter of blood. assuming blood is a simple aqueous solution. Express your answer using two significant figures. odic Table N2 in 15 g/L 18.36. 10-4 mol Na/L blood Submit X Incorrect; Try Again; 2 attempts remaining PartB At a depth of 100 ft in water, the external pressure is 40 atm What is the solubility of Na from air in blood at this pressure? Express your answer using two significant figures. s, - 0.002 Submit Incorrect; Try Again; 2 attempts remaining

Explanation / Answer

Part A

Given,

the solubility of N2 in body at 1.0 atm and at 37 oC = 0.015 g/L

The moles of N2 dissolved per liter of blood = 0.015 / 28 = 5.4 x 10-4 mol

Therefore the quantity of dissolved N2 = 5.4 x 10-4 mol/L

Part B

Given that air is approximately = 78 % N2

Therefore at 1 atm of air pressure the partial pressure of N2 = 0.78 atm

From Henry's law

p = kH x c

where p = Partial pressure of solute i.e. N2 = 0.78 atm

kH = Henry's law constant

c = concentration of solute i.e. N2 = 5.4 x 10-4 mol/L = 5.4 x 10-4 M

p = kH x c

or, 0.78 = kH x 5.4 x 10-4

or, kH = 1.4 x 103 atm/M

At a depth of 100 ft with external pressure of 4.0 atm, partial pressure of N2 = 4.0 x 0.78 atm = 3.12 atm

Concentration of N2 per liter of blood = 3.12 / 1.4 x 103 = 2.2 x 10-3 M

Part C:

Moles of N2 that will come out from 1 L of blood into the blood stream as the scuba driver suddenly

surfaces = 2.2 x 10-3 - 5.4 x 10-4 = 0.00166 mol

1 mol of N2 = 22400 mL

0.00166 mol of N2 = 22400 x 0.00166 = 37 mL

Therefore the mililiters of N2 gas that are released into the bloodstream = 37 mL

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