At ordinary body temperature 137 °C2, the solubility of
N2 in wat...

Question

At ordinary body temperature 137 °C2, the solubility of
N2 in water at ordinary atmospheric pressure (1.0 atm) is
0.015 g>L. Air is approximately 78 mol % N2. (b) At a depth
of 100 ft in water, the external pressure is 4.0 atm. What
is the solubility of N2 from air in blood at this pressure?

Accepted Answer

Hello everyone today. We are being given the following problem and asked us to solve for it. So it says the scalability of carbon dioxide and blood at standard atmospheric pressure is one atmospheres and at a temperature of 37 degrees Celsius is 1.0 to 6 g per liter. If the air approximately if the air is approximately 60.3% moles of C. O. To calculate the suitability of CO two from the air in blood at a depth of ft in water where the external pressure is 6.9 atmospheres. So this is a multi step problem. So the first step we want to do is we want to calculate our salt ability in malls per leader or polarity. And so by doing that we have to take our density of C. 02. So we have to take that 1.0 to 6 g per one liter of blood. And we have to multiply that by the molar mass of C. 02 itself. So we say that one mole sio two is equal to 44.1 g. Once our units can cancel out we are going to get 0. moles of our C. 02. All over one leader or just leaders. The second thing we wanna do is we want to calculate the partial. So we're gonna say we want to calculate the partial pressure at one atmospheres. And so by doing that we see that P. O. P. C. 02 are partial pressure of carbon dioxide is going to be equal to 0.3% mold Times one atmosphere to give us 0. atmospheres. The third thing we wanna do is we want to calculate so we're going to calculate for K. And so we have our cell viability of C. 02 is going to be equal to K. Is equal to the partial pressure of CO two. Rearranging this equation. We get that K. Is equal to our ability of C. 02 over our partial pressure of CO two. And when we plug these values in we're going to get 0.23 moles of C. 02. And then we're going to get all of that over that leaders. But then we have to take that and we have to put that over our partial pressure as indicated by the question as 0.3 atmospheres. To give us a total of 0.766 moles of C. 02 over Leaders times atmospheres. And our last and final step or one of our last our final step step four is going to be to calculate the partial pressure of C. 02 at 6.9 atmospheres. And so by doing that, we see that PCO two is equal to 0.03% times 6.9 atmospheres. A total of 0.207 atmospheres. And lastly we're going to calculate s Or our ability of CO2 At 6. atmospheres. And so we're gonna show that are selling ability of C. 02 is going to equal art zero point moles that we calculated earlier of C. 02 over Leaders Times Atmospheres. We're gonna multiply that by 0.027 atmospheres that we solved any question above. our units of atmospheres are going to cancel out and we are going to be left with a final answer of 0.159 moles of C. 02 over leaders which is also the malaria. T. I hope this helped. And until next time.

At ordinary body temperature 137 °C2, the solubility of N2 in water at ordinary atmospheric pressure (1.0 atm) is 0.015 g>L. Air is approximately 78 mol % N2. (b) At a depth of 100 ft in water, the external pressure is 4.0 atm. What is the solubility of N2 from air in blood at this pressure?

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