A scuba diver is breathing compressed air that is 21% (by volume) oxygen at a depth of 66 ft. beneath the surface. The total pressure at this depth is 3.0 atm. The Henry's law constant (k) for O2 in water at a normal body temperature (37 °C ) is 1.93 * 10-3 mol>(L atm). What is the solubility of O2 in the blood of the diver at 66 ft. beneath the surface? (LO 13.9) (a) 1.22 * 10-3 M (b) 2.76 * 10-2 M (c) 1.22 * 10-1 M (d) 2.76 * 10-1 M

Video transcript

Hey everyone, we're told that a diver is using a 1845 try mix, which means it's composed of 18% oxygen, 45% helium and 37% nitrogen and dives to a depth of 40 m where the total pressure is five atmospheric pressure. Given that the Henry's law constant of nitrogen at 37 degrees Celsius is one point oh times 10 to the negative third moles per liter times atmospheric pressure, calculate the salt ability of nitrogen in the blood at a depth of m. To answer this question, let's first go ahead and determine the pressure of our nitrogen. In order to calculate the pressure of our nitrogen. We're going to take Our total pressure which was said to be five atmospheric pressure and we're going to multiply this by 0.37 since we were told that we had 37% of our nitrogen. When we calculate this out, this gets us to a total of 1.85 atmospheric pressure of our nitrogen. Now let's go ahead and calculate the soluble itty of our nitrogen in order to do so we're going to take our Henry's law constant and multiply this by the pressure of our nitrogen. So let's go ahead and plug in these values. So we were told that our Henry's law constant was one point oh times 10 to the negative three mol per leader times atmospheric pressure. Now we're going to multiply this by the pressure. We just calculated which was 1.85 atmospheric pressure. Now, when we calculate this out and cancel out our unit, we end up with 1.85 times 10 to the negative three molar, which is going to be our final answer. Now, I hope that made sense and let us know if you have any questions.