Hi, this is the question I'm having trouble with:(adsbygoogle = window.adsbygoogle || []).push({});

A gas mixture is known to contain equal numbers of moles of two gases. The mixture has a density of 1.47g/L at 1.00 atm and 298K. In a diffusion experiment, one of the gases was found to diffuse 1.25 times faster than the other under the same conditions. What are the respective molar mases of the two gases?

I've found that [tex]1.25=\sqrt{\frac{M_B}{M_A}}[/tex] Therefore [tex]1.5625=\frac{M_B}{M_A}[/tex], where [tex]M_B[/tex] is the molar mass of gas B. However, from there I have no idea where to go next. I think I'm supposed to use the ideal gas law, but I'm not sure how to apply it when there's a mixture of gases. Any help is appreciated! Thanks!

**Physics Forums | Science Articles, Homework Help, Discussion**

Dismiss Notice

Join Physics Forums Today!

The friendliest, high quality science and math community on the planet! Everyone who loves science is here!

The friendliest, high quality science and math community on the planet! Everyone who loves science is here!

# Ideal Gas Law/Molar Mass

**Physics Forums | Science Articles, Homework Help, Discussion**