Total lung capacity of a typical adult is approximately 5.0 l. approximately 20% of the air is oxygen. you may want to review (pages 360 - 366) . part a at sea level and at an average body temperature of 37∘c, how many moles of oxygen do the lungs contain at the end of an inflation?

You need to understand the ideal gas equation to solve this question. Sea level pressure should be around 1 atm. So, the calculation would be:

PV= nRT
n= RT/PV
n= (0.082057 L atm / mol K) (37+273.15)/ 1 atm (5L*20%)
n=25.4499786 moles

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safiurrehman safiurrehman · Answer 2 · 2019-12-23T16:37:48+01:00

Answer:

n = 0.039 moles

Explanation:

Given that as we know that air content for oxygen are 20%, so as same for lungs which is equals to 1 liter.

For mole (n) calculation we use

pV = nRT

we know that

10^5 Pa is the pressure(p) at sea level

1 liter or 1000cm^3 or 0.001m^3 is the volume(V) of air

8.314 is the value of R which is molar gas constant

For this equation we need to have temperature(T) in Kelvin (273+37)

273 is the temperature at zero in kelvins + 37 normal human body temperature

Re arranging the equation

n = pV/RT

substituting the values

n=10^5 x 0.001 / (8.314 * (273 + 37))

n = 0.039 moles