Question
The solubility of $\mathrm{N}_{2}$ in blood at $37^{\circ} \mathrm{C}$ and at a partial pressure of 0.80 atm is $5.6 \times 10^{-4}$ mol/L. A deepsea diver breathes compressed air with the partial pressure of $\mathrm{N}_{2}$ equal to 4.0 atm. Assume that the total volume of blood in the body is 5.0 L. Calculate the amount of $\mathrm{N}_{2}$ gas released (in liters at $37^{\circ} \mathrm{C}$ and 1 atm) when the diver returns to the surface of the water, where the partial pressure of $\mathrm{N}_{2}$ is 0.80 atm.
Step 1
80 atm is $5.6 \times 10^{-4}$ mol/L. This can be represented by the equation $C = K \times P$, where $C$ is the concentration of $\mathrm{N}_{2}$, $K$ is the Henry's law constant, and $P$ is the partial pressure. Show more…
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The solubility of $\mathrm{N}_{2}$ in blood at $37^{\circ} \mathrm{C}$ and at a partial pressure of 0.80 atm is $5.6 \times 10^{-4} \mathrm{mol} / \mathrm{L}$. A deep-sea diver breathes compressed air with the partial pressure of $\mathrm{N}_{2}$ equal to 4.0 atm. Assume that the total volume of blood in the body is $5.0 \mathrm{L}$. Calculate the amount of $\mathrm{N}_{2}$ gas released (in liters at $37^{\circ} \mathrm{C}$ and 1 atm) when the diver returns to the surface of the water, where the partial pressure of $\mathrm{N}_{2}$ is 0.80 atm.
The solubility of N2 in blood at 37°C and at a partial pressure of 0.80 atm is 5.6 x 10^24 mol/L. A deepsea diver breathes compressed air with the partial pressure of N2 equal to 4.0 atm. Assume that the total volume of blood in the body is 5.0 L. Calculate the amount of N2 gas released (in liters at 37°C and 1 atm) when the diver returns to the surface of the water, where the partial pressure of N2 is 0.80 atm.
At ordinary body temperature $\left(37^{\circ} \mathrm{C}\right),$ the solubility of $\mathrm{N}_{2}$ in water at ordinary atmospheric pressure $(1.0 \mathrm{atm})$ is 0.015 $\mathrm{g} / \mathrm{L} .$ Air is approximately 78 $\mathrm{mol} \% \mathrm{N}_{2}$ . (a) Calculate the number of moles of $\mathrm{N}_{2}$ dissolved per liter of blood, assuming blood is a simple aqueous solution. (b) At a depth of 100 $\mathrm{ft}$ in water, the external pressure is 4.0 atm. What is the solubility of $\mathrm{N}_{2}$ from air in blood at this pressure? (c) If a scuba diver suddenly surfaces from this depth, how many milliliters of $\mathrm{N}_{2}$ gas, in the form of tiny bubbles, are released into the bloodstream from each liter of blood?
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