At surface of the earth, 0.000488 moles of N2 dissolved in each liter of blood. (Ptot=1 atm at surface, and PN2 = 0.78 atm). Calculate Henry's law constant for N2(g) dissolving into blood at the Earth surface and then calculate the number of moles of N2(g) that would dissolve if PN2 increased from 0.78 to 2.3 atm, corresponding to ~20 meters depth underwater.
The Attempt at a Solution
For the first part of the question, I did the following
Henry's Law states
Solubility = KH * P
4.88E-4 = KH * 0.78
KH= 6.26E-4 mol/L-atm
However I am unable to calculate the second part of the question, what I have so far
S2.3/S0.78 = 2.3/0.78 = 2.94
S2.3 = 4.88E-4 * 2.94 = 1.43E3 mol/L
Now I know the solubility of N2 at 2.3 atm, how do I approach the problem from here?