A mixture containing 1.6 g of O2, 1.4 g of N2 and 0.4 g of He occupies a volume of 10 L at 27∘C. Calculate the partial pressure of each component of the mixture.
PN2=0.123 atm
PO2=0.123 atm
PHe=0.246 atm
PHe = 0.246 atm, PO2= PN2 = 0.123 atm
Given that V=10 L , T = 27∘C=300 K
The number of moles are :-
nHe=0.44=0.1
nN2 =1.428= 0.05
nO2 = 1.632 = 0.05
therefore , the total number of moles = 0.1+0.05+0.05 = 0.2
Using the ideal gas equation PV = nRT ⇒P×10=0.2×0.082×300⇒P=0.492 atm
As partial pressure = total pressure × mole fraction , we have
PHe = 0.492×0.10.2 = 0.246 atm
PN2= 0.492×0.050.2=0.123 atm
PO2= 0.492×0.050.2 = 0.123 atm