00:01
The rate of vapor formation above a liquid will depend on the liquids intermolecular forces that are present.
00:08
So if we have a liquid with very weak intermolecular interactions, then what we will see is a very small surface tension of pulling the molecules inwards.
00:17
And what we see as a result is the rate of evaporation will be lower.
00:22
And so the liquid will have a lower pressure.
00:25
So with this vast example, what we have is c2h6 and c2 cl6.
00:34
So some similarities, they are both symmetrical, they are both uncharged, and so what we have is dispersion forces.
00:47
These are the only intermolecular forces, but the c2 cl6 will have a large electron cloud compared to ethane, and so it will be more easily polarised by neighbouring molecules and so can form temporary dipoles.
01:03
And so the dispersion forces will be a lot stronger, compared to ethan and so its molecule will evaporate at a lower rate and so as a result we can say that ethane has a higher vapor pressure.
01:18
Next we have another comparison of two structures f2c double bond o and ch30h.
01:27
So the first structure that we drew out is larger in size and does have more electrons than methanol so its dispersion forces will be stronger than methanol...