the partial pressure of O2 in air is 158 mmHg at 25 degrees C and a total pressu
ID: 878083 • Letter: T
Question
the partial pressure of O2 in air is 158 mmHg at 25 degrees C and a total pressure of 760 mmHg. The air that is expired from your lungs after breathing has a partial pressure of O2 of 115 mmHg under the same conditions. How many moles of O2 are absorbed by your lungs from 1.0 L of air? 4. The partial pressure of O2 in air is 158 mmHg at 25°C and a total pressure of 760 mmHg. The air that is expired from your lungs after breathing has a partial pressure of 02 of 115 mmHg under the same conditions. How many moles of 02 are absorbed by your lungs from 1.0L of air?Explanation / Answer
The solution is as shown below
pressure of O2 absorbed by lungs = 158 - 115 = 43 mmHg
total pressure = 760 mmHg
moles fraction of O2 = 43/760 = 0.057
total volume = 1.0 L
calculate total moles of O2,
n(total) = P(total) x V/RT
= 1 atm x 1 L / 0.0821 x 298 K
= 0.041 mols
moles of O2 = 0.057 x 0.041 = 0.0023 mols
Thus, 0.0023 mols of O2 is absorbed by lungs
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