00:01
Okay, we have 0 .1105 grams of menthol.
00:05
It reacts with o2, and our combustion reaction, it makes the o2 in h2.
00:09
We measured how much carbon dioxide and water we made in this reaction.
00:14
We want to know what the empirical formula.
00:20
The empirical formula is the lowest number of, smallest ratio we can have of all the elements within the molecule.
00:32
And so what i'm going to do is i'm going to convert these into moles of co2 and h2 because we can't do much with grams.
00:39
And so co2, these will be in grams per mole.
00:44
Co2, it has one carbon at 12 .01 grams.
00:51
And that's going to be plus 16 for oxygen times two oxygens.
00:56
It comes out to 44 .01 grams per mole for co2.
01:01
And for h2o, that's 16 for the oxygen plus 2 times 1 .01, 18 .02.
01:09
And so we calculated the molar mass of these simply by pulling them off the periodic table.
01:16
So now let's convert these to moles.
01:18
We have 0 .2829 grams of co2.
01:25
Use the molar mass by dividing it to get moles, grams cancel and get moles.
01:32
And we have 0 .00643 moles co2.
01:41
Okay.
01:43
Now we have to do the same for water.
01:47
So 0 .119 grams of h2o divide by our 18 .02 grams per one mole.
01:55
And we have 0 .00643 moles of h2o.
02:02
Alright.
02:03
So we found the moles of these.
02:05
We have to get, we eventually want to find something that relates to menthol.
02:09
And so what we're getting out of menthol is the carbon and hydrogen.
02:13
Most of the oxygen get out of this combustion is coming in through their o2 inherent in combustion.
02:19
So maybe a few of these oxygens are coming from menthol, but most of it comes from o2.
02:22
So it's not going to be a reliable measure to count these...