chemistry

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.

  1. 👍 0
  2. 👎 0
  3. 👁 325
asked by UTramos

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    A gas mixture is composed of 4.3 grams of hydrogen (density at STP = 0.089 g/L) and 2.9 grams of helium (density at STP = 0.179 g/L). What is the percentage (v/v) helium in the mixture? If v/v = Volume of gas/total volume how

    asked by Anon on November 13, 2014

  2. chemistry

    Suppose 100 mL of NO at STP is mixed with 400 mL of O2 at STP. 2 NO (g) + O2 (g)---> 2 NO2 (g) After the reaction goes to completion, what is the partial pressure of NO2 in the resulting mixture of gases at STP? I know the

    asked by Anon on December 13, 2014

  3. chem

    Helium-oxygen mixtures are used by divers to avoid the bends and are used in medicine to treat some respiratory ailments. What percent (by moles)of He(g) is present in a helium-oxygen mixture having a density of 0.538g/L at

    asked by tomi on September 26, 2008

  4. Chemistry

    To prevent the presence of air, noble gases are placed over highly reactive chemicals to act as inert "blanketing" gases. A chemical engineer places a mixture of noble gases consisting of 4.50 g of He, 15.0 g of Ne, and 33.6 g of

    asked by Arian on October 18, 2010

  5. Chemistry-Gases

    A mixture of gases is prepared from 76.9 g of O2 and 16.0 g of H2. After the reaction of O2 and H2 is complete, what is the total pressure of the mixture if its temperature is 178 ºC and its volume is 11.0 L? What are the partial

    asked by Anonymous on April 2, 2014

  6. Chemistry

    Consider the following equation: 4NH3(g) + 5O2(g)----> 4NO(g)+6H2O(g) a. How many liters of oxygen are required to react with 2.5 L NH3? Both gases are at STP b. How many grams of water vapor can be produced from 25 L NH3 if both

    asked by Ivy on November 29, 2010

  7. college chemistry

    Consider the following equation: 4 NH3(g) + 5 O2(g)= 4 NO(g) + 6 H2O(s) a) HOw many liters of oxygen are required to react with 205 L NH3? Both gases are STP. b)How many grams of water vapor can be produced from 25 L NH3 if both

    asked by la fonda on April 29, 2014

  8. Chemistry

    A 1.0 liter flask is filled with a mixture of two gases at 20. oC until a pressure of 14.43 atm is established. If 0.40 grams of the mixture is hydrogen, how many moles are there of the other gases?

    asked by Carrie Boom on April 18, 2014

  9. Chemistry

    I have an exam in a day and I'm confused on how to solve this question. Do I use PV=nRT? Do I find out the molecular formula of the gas from the percentage of nitrogen and oxygen? A sample of a mixture of gases contains 80.0%

    asked by Jenny on June 22, 2014

  10. Density of Gas at STP

    Hi Can anyone explain how to calculate the density in g l -1 of a gaseous oxide at STP. I don't understand the term g l -1 !! Thank You "g l-1" should have the -1 as a superscript, meaning g l^-1, or g/l. It means they want the

    asked by Freddo on January 24, 2007

More Similar Questions