Calculate the solubility of dinitrogen in blood that is in contact with air (78% N2) at 4.00 atm, the pressure

Question

At body temperature (37oC), the Henery's law constant for N2 is 3.8 × 10-4.

Answer 1

S= 3.8*10^-4*0.78 =3*10^-4L

you must use 0.78 since at 1 atmosphere , partial pressure is only 0.78 atm and not 1

Answer 2

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Answer 3

Solubility= ok(Henrys consistent) x Partial stress of Nitrogen Partial stress formulation= (Mole Fraction of Nitrogen) x (entire Atmospheric stress) Partial stress of Nitrogen = (.seventy 8 moles of Nitrogen) x (a million.2 ATM) = .936 Solubility of Nitrogen= (6.1x10^-4) x (.936) = (5.7x10^-4)

Answer 4

3.84 x 10^-4/1atm = S2/4.00atm

based on the data you have given me, this would be the derived equation. Just solve for S2. I used 1atm because that is the standard pressure of our bodies. :)

Answer 5

Data required.