Arrange the following molecules in order of increasing average molecular speed. H2 at 371K, NO2 at 339K, Ne at 371K, H2 at 425K Enter formulas and temperatures in the boxes below: 1 = slowest, 4 = fastest 1 at K 2 at K 3 at K 4 at K ???

1 Answer
Feb 26, 2018

1 - NO2 at 339 K
2 - Ne at 371 K
3 - H2 at 371 K
4 - H2 at 425 K

Explanation:

Kinetic Energy is directly related to temperature; the higher the temperature the higher the kinetic energy. Kinetic energy is also equal to 12mv2, so if we want a high velocity we want high temp and low mass. So let's list out approximate masses:

m(H2)2
m(NO2)46
m(Ne)20

So we have NO2 at 339 K, the lowest temperature out of the mix, and the highest mass out of the mix, so this is moving the slowest.

In contrast, we have H2 at 425 K, the highest temperature out of the mix, and the lowest mass out of the mix, so this is moving the fastest.

Now we have Ne and H2 at 371 K, since they are at the same temperature they have the same kinetic energy. But H2 is lighter than Ne so it must be faster. To quantify this mathematically, let's assume (this is wrong but just as an assumption for an example) KE at 371 K is 100:

100=12mv2
200=mv2
200m=v
So H2 is about v=10 and Ne is about v=103

So the order to recap is:
1 - NO2 at 339 K
2 - Ne at 371 K
3 - H2 at 371 K
4 - H2 at 425 K

Hope that makes it clearer!