Question

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?

Answer 1

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

Answer 2

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