A human lung at maximum capacity has a volume of 3.0 liters. If the partial pressure of oxygen in the air is 21.1 kilopascals an

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2 months ago

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d the air temperature is 295 K, how many moles of oxygen are in the lung?

1 answer:

lions [2.9K] · Answer 1 · 2026-04-01T01:07:39+03:00

Answer: 0.026 moles of oxygen are present in the lung

Explanation:

We can address this question using the ideal gas law.

The relevant equation is shown below.

$PV = nRT$

We know P = 21.1 kPa

Now, converting pressure from kPa to atmospheres is essential.

The conversion factor used is 1 atm = 101.3 kPa.

$21.1 kPa \times \frac{1atm}{101.3kPa}= 0.208 atm$

V = 3.0 L

T = 295 K

R = 0.0821 L-atm/mol K

We proceed to rearrange the equation to solve for n.

$n = \frac{PV}{RT}$

$n = \frac{0.208atm\times 3.0L}{0.0821 L.atm/mol K\times 295 K}$

$n = 0.026 mol$

0.026 moles of oxygen are present in the lung