Question
Total lung capacity of a typical adult is approximately 5.0L. Approximately 20% of the air is oxygen, as air is 20% oxygen. 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?
n=PV/RT
V=5.0L=.005m^3
P=1.013e^5Pa
R=8.31J/mole*K
T=37c=310k
so n=124.85
then I times by .20 to get the moles of Oxygen...but I'm missing something?
n=PV/RT
V=5.0L=.005m^3
P=1.013e^5Pa
R=8.31J/mole*K
T=37c=310k
so n=124.85
then I times by .20 to get the moles of Oxygen...but I'm missing something?
Answers
ana
Never mind this question...i figured out my mistakes
Anonymous
Wait!! You might know how to do it, but I still don't. Help :(
Anonymous
Avogadro's number?