Question #7a5f8

1 Answer
Dec 17, 2016

Well, once you see that you can convert from "g" to "mol", and once you identify the units of molar volume, this is fairly straightforward:

barV = V/n = 22.4 is in "L/mol", if the standard pressure is "1 atm" and the standard temperature is 0^@ "C".

To get the "mol"s:

11.5 cancel"g Ne" xx "1 mol Ne"/(20.180 cancel"g Ne")

= "0.570 mols Ne"

And the only thing left to do is to get rid of the "mol"s.

"22.4 L"/cancel"mol" xx 0.570 cancel"mols Ne" = color(blue)("12.8 L Ne")

So then, what is the predicted density of "Ne" in "g/L" if assuming ideality? If the true density is "0.9002 g/L", is "Ne" pretty ideal, or not?