Saturday
April 19, 2014

Homework Help: chemistry

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.

Answer this Question

First Name:
School Subject:
Answer:

Related Questions

CHEMISTRY - A mixture contains 5.00 g each of O2, N2, CO2, and Ne gas. Calculate...
Chemistry - A gaseous mixture contains 413.0 Torr of H2(g), 372.1 Torr of N2(g...
Chemistry - A gaseous mixture contains 413.0 Torr of H2(g), 372.1 Torr of N2(g...
Chemistry - A gaseous mixture contains 436.0 Torr of H2(g), 341.5 Torr of N2(g...
Density of Gas at STP - Hi Can anyone explain how to calculate the density in g ...
Chem - A gas mixture in a 3.100 L container at 415C contains 1.30 g each of Ar...
CHEMISTRY - A mixture contains 5.00 g each of O2, N2, CO2, and Ne gas. Calculate...
chemistry - The gases in a mixture have the following partial pressures at the ...
Chemistry - A mixture contains 5.0 g of He, 1.0 g of Ar, and 3.5 g of Ne. ...
Chemistry - Given that a sample of air is made up of nitrogen, oxygen, and argon...

Search
Members