When air is inhaled, it enters the alveoli of the lungs, and...

When air is inhaled, it enters the alveoli of the lungs, and varying amounts of the component gases exchange with dissolved gases in the blood. The resulting alveolar gas mixture is quite different from the atmospheric mixture. The following table presents selected data on the composition and partial pressure of four gases in the atmosphere and in the alveoli: If the total pressure of each gas mixture is 1.00 atm, calculate: (a) The partial pressure (in torr) of each gas in the atmosphere (b) The mole $\%$ of each gas in the alveoli (c) The number of $\mathrm{O}_{2}$ molecules in 0.50 $\mathrm{L}$ of alveolar air (volume of an average breath of a person at rest) at $37^{\circ} \mathrm{C}$

When air is inhaled, it enters the alveoli of the lungs, and varying amounts of the component gases exchange with dissolved gases in the blood. The resulting alveolar gas mixture is quite different from the atmospheric mixture. The following table presents selected data on the composition and partial pressure of four gases in the atmosphere and in the alveoli: If the total pressure of each gas mixture is 1.00 atm, calculate:
(a) The partial pressure (in torr) of each gas in the atmosphere
(b) The mole $\%$ of each gas in the alveoli
(c) The number of $\mathrm{O}_{2}$ molecules in 0.50 $\mathrm{L}$ of alveolar air (volume of an average breath of a person at rest) at $37^{\circ} \mathrm{C}$

Key Concepts

Respiratory Gas Exchange

In the context of alveolar air, respiratory gas exchange refers to the process by which gases are exchanged between the alveoli in the lungs and the blood. This concept explains how the composition and partial pressures of inhaled atmospheric air change in the alveoli due to the uptake of oxygen and the release of carbon dioxide.

Pressure Unit Conversion

Pressure unit conversion is a key concept when dealing with different units of pressure such as atmospheres and torr. Recognizing the conversion factor, typically 1 atm = 760 torr, allows for accurate calculation and comparison of gas pressures in various units.

Mole Fraction

The mole fraction is a way of expressing the composition of a gas mixture by representing the ratio of the number of moles of a particular component to the total number of moles in the mixture. It is directly related to the partial pressure of a gas in a mixture, as the partial pressure is equal to the mole fraction multiplied by the total pressure.

Dalton's Law of Partial Pressures

This law states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of each individual gas. It is a crucial principle in gas mixtures as it allows one to calculate the pressure contribution of each component when the overall pressure and mole fractions are known.

Ideal Gas Law

The ideal gas law, given by PV = nRT, relates the pressure, volume, number of moles, temperature, and the gas constant. This law is fundamental for calculations involving gases, such as determining the number of molecules in a given volume at a certain temperature and pressure.

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