A flask at room temperature contains exactly equal amounts (in moles) of nitrogen and xenon. b. The molecules or atoms of which gas have the greater average velocity? d. If a small hole were opened in the flask, which gas effuses more quickly?

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Hey everyone. So here we ask to use the root mean square velocity and the kinetic energy of N. H. Two minus NH three and NH four plus to determine the lowest infusion rate, the lowest velocity and the lowest kinetic energy. So the root mean square velocity he goes to square root free R. T. By the molar mass. And the kinetic energy one half of the mass times velocity squared. So for a infusion rate is inversely proportional to the Mueller mass. As the molar mass increases, the rate of effusion decreases. If you look at the molar mass of each, For NH 2 -, We're gonna have 14.007 g. Us too. That was 1.008 grams. And this gives us 16.0-3 grams in the Mueller mass. NH three Gonna give us 14.007g plus three. 1.008. This will give us 17.031 in the Mueller mass. NH four Gonna give us 14.007g plus four Times 1.008. This give us 18.039. The largest smaller mass is gonna have the lowest effusion rate. So NH four plus. And I have the lowest infusion rate. And for b the lower the mass the Lord the velocity NH 2 - has the lowest mass. NH two minus gonna have the lowest velocity. And for c the lower the mass the lower the kinetic energy NH 2 - has the lowest mass. So NH 2 -. Gonna have the lowest kinetic energy. Thanks for watching my video, and I hope it was helpful.

A flask at room temperature contains exactly equal amounts (in moles) of nitrogen and xenon. b. The molecules or atoms of which gas have the greater average velocity? d. If a small hole were opened in the flask, which gas effuses more quickly?

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