Air in human lungs has a temperature of 37.0^∘ C and a saturation vapor density of 44.0 g / m^3.

step 1 Now, the given temperature is 37 degrees Celsius and the saturation vapor density is 44 gram per

Air in human lungs has a temperature of 37.0^∘ C and a...

Air in human lungs has a temperature of $37.0^{\circ} \mathrm{C}$ and a saturation vapor density of $44.0 \mathrm{g} / \mathrm{m}^{3}$. (a) If $2.00 \mathrm{L}$ of air is exhaled and very dry air inhaled, what is the maximum loss of water vapor by the person? (b) Calculate the partial pressure of water vapor having this density, and compare it with the vapor pressure of $6.31 \times 10^{3} \mathrm{N} / \mathrm{m}^{2}$.

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Key Concepts

Partial Pressure and Dalton's Law

Partial pressure is the pressure contributed by each individual gas in a mixture, and Dalton's Law states that the total pressure is the sum of these individual pressures. This concept is essential when analyzing the behavior of water vapor mixed with other gases, such as in exhaled air.

Ideal Gas Law

The ideal gas law relates pressure, volume, temperature, and the number of particles (or density) of a gas. It provides the foundational framework needed to connect measurable properties like density and pressure in calculating the state of gases under various conditions.

Saturation Vapor Density

This concept refers to the maximum amount of water vapor that air can hold at a specific temperature before it starts condensing into liquid. It is a temperature?dependent property and is crucial in problems involving humidity and condensation since surpassing this limit leads to phase change.

Vapor Pressure

Vapor pressure is the pressure exerted by the water vapor in equilibrium with its liquid phase at a given temperature. It is a measure of a liquid’s tendency to evaporate and plays an important role in determining the state of water in atmospheric studies.

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