🤓 Based on our data, we think this question is relevant for Professor Bindell's class at UCF.

We're being asked to calculate the **milliliters of N _{2 }gas released into the blood stream**.

**For this problem, we will do the following steps:**

**Step 1:** Calculate **Henry’s Law constant** for the gas

Recall that the solubility of a gas is given by * Henry’s law*:

$\overline{){{\mathbf{S}}}_{{\mathbf{gas}}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{{\mathbf{k}}}_{{\mathbf{H}}}{\mathbf{\xb7}}{{\mathbf{P}}}_{{\mathbf{gas}}}}$

where:

**S _{gas}** = solubility of the gas (in mol/L or M)

**k _{H}** = Henry’s law constant for the gas

**P _{gas}** = partial pressure of the gas

At ordinary body temperature (37 ^{o}C), the solubility of N_{2} in water at ordinary atmospheric pressure (1.0 atm) is 0.015 g/L. Air is approximately 78 mol % N_{2}.

At a depth of 100 ft in water, the external pressure is 4.0 atm. If a scuba diver suddenly surfaces from this depth, how many milliliters of N_{2} gas, in the form of tiny bubbles, are released into the bloodstream from each liter of blood?