The density of a gaseous mixture containing He and O2 at 27 degree Celsius and 760 torr is 0.50 g/l . The amount fraction of he in the mixture is?
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First, you can use the ideal gas law to calculate the average molar mass of the gas mixture:
PV=nRT
n=mass/molar mass
PV=(mass/molar mass)RT
density=mass/V
Rearranging the equation we get
molar mass=(density)RT/P
Molar mass=(0.50g/L)(0.0821 Latm/molk)(300k)/0.9487atm
molar mass=12.98g/mol
Now let x=mole fraction of He and
1-x=mole fraction of O2
12.98g/mol=4(x)+32(1-x)
12.98=4x+32-32x
-19.02=-28x
x=0.67*100%
67%
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