Posted by **UTramos** on Sunday, June 18, 2006 at 8:55pm.

A mixture of Ar and N2 gases has a density of 1.361 g/L at STP. What is the mole fraction of each gas?

not sure on really where to start

Work this as the classic mixture:

the mass of 22.4 liters of the gas is 1.361*22.4 grams.

molmassargon*Far + molmassN2*Fn2=1.361*22.4

where Far + Fn2=1

You are solving for Far and Fn2.

What do u mean by Far and Fn2 where do i get those values?

That is the mole fractions: Far is the argon mole fraction, and fn2 is the nitrogen mole fraction. YOu get them by solving the two equations.

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