00:01
We're told that pure octane, which has a chemical formula of c8h18, is combusted, meaning it reacts with o2, forming carbon dioxide and water.
00:17
And we want to know if a kilogram of octane is burned, then how much carbon dioxide would be added to the atmosphere? this will require stoichiometry, and all stoichiometry requires beginning with a balanced equation.
00:34
So let's do that.
00:36
The easiest way to balance a combustion equation of this type is to take the subscript on hydrogen and put it in front of the water.
00:44
From there, adjust the hydrogen.
00:46
I now have 36 hydrogen on the right, so i'll need to double this.
00:51
I now have 16 carbon on the left, so i'll fix that.
00:56
16 times 2 is 32.
00:58
For oxygen, 18 times 1 is 18, 32 and 18 equals 50.
01:04
Half of that is 25.
01:08
And that will be a balanced equation.
01:10
Now, since molar masses are generally in grams per mole instead of kilograms per mole, let's convert these kilograms.
01:17
King henry died by drinking chocolate milk.
01:22
So i'll take, i'll start from kilograms and move three places to the right.
01:30
Grams has no prefix, so i know it's in the middle there, which means i move the decimal three places to the right.
01:35
So it's not one kilogram...