Each of the lungs holds 2.0 $l$ of air at the physiological temperature of 37^oC. The number of moles of air in the lungs (where the gauge pressure is 21 kPa) is

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Quizplus · Accepted Answer

To find the number of moles of air in the lungs, we can use the ideal gas law, $PV = nRT$, where $P$ is the pressure, $V$ is the volume, $n$ is the number of moles, $R$ is the ideal gas constant, and $T$ is the temperature in Kelvin. The pressure in the lungs is the atmospheric pressure plus the gauge pressure, so $P = 101.3 \, kPa + 21 \, kPa = 122.3 \, kPa$. The volume $V = 2.0 \, l = 2.0 \times 10^{-3} \, m^3$, and the temperature $T = 37^\circ C = 310 \, K$. The ideal gas constant $R = 8.314 \, J/(mol \cdot K)$. Substituting these values into the ideal gas law and solving for $n$ gives the number of moles of air in the lungs.

Each of the Lungs Holds 2 lll Of Air at the Physiological Temperature of 37oC

Each of the Lungs Holds 2 $l$ Of Air at the Physiological Temperature of 37^oC