00:02
For this question, we need to know the balanced chemical reaction, which i wrote below.
00:05
So we have magnesium plus two oxygen, because oxygen is diatomic, yields mgo.
00:11
When we try to balance that, we have to have two oxygen on the product side, which means we need two magnesium on the reactive side.
00:18
The molar mass of magnesium is 24 .31.
00:24
The molar mass of oxygen is 32, and the molar mass of magnesium oxide is 40 .3.
00:35
So we know we're starting with 10 grams of each.
00:38
We have to calculate how much is produced, how much magnesium oxide is produced.
00:45
So this is a limiting reactant problem, and therefore we need to determine what is being produced.
00:56
So we're going to start with magnesium.
00:58
So if we have 10 grams of the magnesium, we need to first get rid of our grams of magnesium.
01:02
So we're going to put the mass of magnesium on the bottom and one mold magnesium up top.
01:12
Then we're going to put mole of magnesium on the bottom, and we're going to put mole of magnesium oxide up top.
01:18
Whenever we have mole on top of mole, we have to look at our coefficients.
01:22
In this case, it's 2 and 2.
01:24
It could be simplified.
01:25
Sometimes it can't be.
01:26
The last step then is to get rid of our moles of magnesium oxide...