00:01
Hi, so we are to solve for the empirical formula of the substance based on the given information here.
00:06
So we need to solve first for the mass of the component elements.
00:10
We'll start with carbon, mass of carbon, using the amount of co2 produced, 677 .6.
00:16
This is milligrams of co2.
00:19
Now we need to convert milligrams to grams because we will be using the molar mass of the compounds in terms of grams.
00:25
This is the conversion factor, 1000 milligrams is 1 gram.
00:31
And then we will convert this to moles by dividing the molar mass of co2, that's 44 .01 grams here, and then moles of co2 in here.
00:42
And for every one mole of co2, we'll have one mole of carbon, because we have it here, one mole of carbon.
00:51
And then we'll multiply the atomic mass of carbon, that's 12 .01 grams here, then moles in the denominator.
00:59
So that means you could cancel this one, grams, moles co2, moles of carbon, and we'll get 0 .1849.
01:10
This is grams of carbon.
01:12
And then for hydrogen, we have 79 .20.
01:17
This is milligrams of h2o, convert this to grams, 1000 milligrams is 1 gram.
01:26
Divide the molar mass of water, 18 .02 grams per mole of h2o.
01:33
Then one mole of h2o has how many moles of h? we have here two.
01:40
So write that in the numerator, two moles of h.
01:45
Then multiply the atomic mass of h, 1 .01 grams per mole.
01:50
Cancel units, milligrams, grams, moles h2o, moles of h, and we'll get 8 .878 times 10 to the negative 3 grams of h.
02:05
And then we still have sulfur.
02:07
So mass of sulfur will be, we will subtract the mass of carbon and hydrogen from the mass of our sample.
02:14
So we have 264 .4.
02:17
This is milligrams, so we need to convert this to grams, 1000 milligrams is 1 gram.
02:24
Subtract the amount of carbon, 0 .1849 grams minus mass of hydrogen, 8 .878 times 10 to the negative 3, which is also in grams.
02:37
So that means we'll have 0 .070622 grams of sulfur...