At ordinary body temperature (37^∘ C), the solubility of N2 in water at ordinary atmospheric pre

step 1 To calculate the molarity of n2, malaria M, molarity m is mass by molar mass by volume, which is

At ordinary body temperature (37^∘ C), the solubility of N2...

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?

Key Concepts

Henry's Law

Henry's Law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas above the liquid. This concept is crucial in understanding how the amount of a dissolved gas changes when the pressure is altered, as seen in problems involving gas solubility in blood or water. It allows one to calculate variations in gas concentration under different pressure conditions.

Dalton's Law of Partial Pressures

Dalton's Law of Partial Pressures explains that the total pressure exerted by a mixture of gases is equal to the sum of the pressures that each individual gas would exert if it occupied the same volume alone. This concept is important for determining the partial pressure of a specific gas, such as nitrogen, when air consists of multiple gases. It thereby connects the composition of gas mixtures to the solubility of individual gases according to Henry's Law.

Ideal Gas Law

The Ideal Gas Law, expressed as PV = nRT, relates the pressure, volume, number of moles, and temperature of an ideal gas. This law is key to converting between the number of moles of a gas and its volume under different conditions, enabling the calculation of gas volumes emitted or dissolved under changing pressures and temperatures, which is applicable to the analysis of gas behavior in biological and environmental systems.

Mole Concept and Unit Conversions

The mole concept is a fundamental chemical principle for quantifying the amount of substance, using Avogadro's number to relate moles to the number of particles. Converting between mass, moles, and volume (using molar mass and the Ideal Gas Law) is essential for solving problems that involve chemical concentrations and reaction stoichiometry, such as determining the moles of gas dissolved in a solution or the volume of gas released from solution under varying conditions.

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