00:01
So this question is a limiting reagent stoichiometry problem.
00:03
So you start out with...
00:04
So this question is 9 .6 grams of iron and 4 .5 grams of oxygen, and it wants to know how many grams of iron two oxide you will produce in the end.
00:15
So 9 .6 grams of iron.
00:20
Well, the first roll we have to do is to convert that into moles.
00:24
So we need to use the periodic table.
00:27
And for every one mole of iron, it's 55 .85 grams of iron.
00:35
And then from the equation that i wrote balanced, for every two moles of iron, it's two moles of iron oxide.
00:46
And then for every one mole of iron oxide, iron two oxide, it's 71 .85 grams of iron oxide.
00:56
Now we do the same process with the oxygen.
01:01
So 4 .5 grams of oxygen, 1 mole of oxygen is 32 grams of oxygen.
01:14
For every 1 mole of oxygen, it's 2 moles of iron oxide, and for 1 mole of iron oxide, it's 71 .85 grams of iron oxide.
01:32
And then we have to do the math.
01:35
So this question.
01:37
So before we jump into the answers, let's just review one more time where the numbers come from.
01:43
These are the given from the problem.
01:45
And these are just molar masses.
01:47
They're obtained by adding up all the masses found in the periodic table for the different elements...