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## Homework Statement

At surface of the earth, 0.000488 moles of N

_{2}dissolved in each liter of blood. (P

_{tot}=1 atm at surface, and P

_{N2}= 0.78 atm). Calculate Henry's law constant for N

_{2(g)}dissolving into blood at the Earth surface and then calculate the number of moles of N

_{2(g)}that would dissolve if P

_{N2}increased from 0.78 to 2.3 atm, corresponding to ~20 meters depth underwater.

## Homework Equations

None

## The Attempt at a Solution

For the first part of the question, I did the following

Henry's Law states

Solubility = K

_{H}* P

therefore

4.88E-4 = K

_{H}* 0.78

K

_{H}= 6.26E-4 mol/L-atm

However I am unable to calculate the second part of the question, what I have so far

S

_{2.3}/S

_{0.78}= 2.3/0.78 = 2.94

S

_{2.3}= 4.88E-4 * 2.94 = 1.43E3 mol/L

Now I know the solubility of N

_{2}at 2.3 atm, how do I approach the problem from here?

Sincerely.