00:01
So the empirical formula is the simplest positive integer ratio of atoms present in a compound, and the molecular formula is the actual number of atoms present in a compound.
00:13
So the empirical formula is kind of just like the base formula.
00:17
So for instance, h2o would have a molecular formula of this, 2hs and 1o.
00:25
That's the simplest ratio of atoms present in this compound.
00:30
So now, let's just say we have another compound that has a molar mass of 36 grams for mole.
00:48
We can use this empirical formula to help us determine the actual molecular formula for this 36 grams for mole compound.
00:59
And how we would do that is first we need to calculate the.
01:05
The molar mass of h2o.
01:07
And this is done by adding up the individual molar mass of each atom within h2o.
01:12
So we have hydrogen to the molar mass of one, two of those, and then we have 16 for oxygen.
01:20
It's an equal 18...
