00:01
We have a compound that contains carbon, hydrogen, and oxygen, and it's analyzed via combustion analysis.
00:07
This question doesn't really ask a question.
00:09
It just simply states in order to determine the moles of hydrogen in the compound.
00:13
First determine the moles of water that were produced from the combustion.
00:18
To do that, we'll start with the grams of water that were produced, and we will assume that all of the hydrogen that was in the compound is now tied up in the water.
00:29
So we can convert the grams of water to moles of water by dividing by the molar mass of water, and then convert the moles of water to moles of hydrogen, seeing that there are two moles of hydrogen in every one mole of water, and we get 2 .787 moles of hydrogen.
00:46
I'm going to determine the empirical formula, even though it doesn't specifically ask, it may be part of the problem.
00:53
I'll then convert my moles hydrogen to grams hydrogen by multiplying by the molar mass of hydrogen.
00:59
I'll do something similar with the carbon dioxide to determine the moles of carbon in carbon dioxide, which will be the moles of carbon in the original compound...