A vessel contains a mixture of H2 and N2 gas....
A vessel contains a mixture of H2 and N2 gas. The density of the gas mixture is 0.2g/L at 300K and 1atm. Assuming that both the gases behave ideally,the mole fraction of N2(g) in the vessel is___. (Final answer should be rounded off to two decimal places) [Given,R=0.082L.atm.mol^-1.K^-1, atomic weight of hydrogen=1 and atomic weight of nitrogen=14]?
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 YOGESH SHARMA Sep 25, 2019
Related A vessel contains a mixture of H2 and N2 gas. The density of the gas mixture is 0.2g/L at 300K and 1atm. Assuming that both the gases behave ideally,the mole fraction of N2(g) in the vessel is___. (Final answer should be rounded off to two decimal places) [Given,R=0.082L.atm.mol^-1.K^-1, atomic weight of hydrogen=1 and atomic weight of nitrogen=14]?
Ans.

Given: density of mixture=0.2g/L ,T=300K,P=1atm
Using formula d=PM/RT

Hence, M= (dxRxT)/P
M=(0.2x0.0821x300)/1
M=4.926g

Now, let mole fraction of N2 (X1) be 'n' and mole fraction of H2(X2) be '(1-n)'
M1=( 2x14=28)=mol.mass of N2
M2=(2x1=2)=mol.mass of H2

Applying formula of molar mass of mixture—
M= M1 X1 +M2 X2
4.926={ 28xn + 2x(1-n) }
solving for ‘n’ we find n=0.11

Hence the mole fraction of N2 (g)in the vessel is 0.11

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