00:03
Hello, in this question, we are given this balanced chemical equation.
00:07
And balanced chemical equations are useful because they give us the mole ratio in which the reactants react and the products are formed.
00:15
And they give us this ratio through the coefficients.
00:19
So in other words, what this equation is telling us is that for every four moles of ammonia that we react, we need five moles of oxygen.
00:29
And we're going to produce four moles of the no and six moles of h2o.
00:37
So we have a mole ratio here, 4 to 5 to 4 to 6.
00:41
The reactants are going to react and the products are going to be produced always in this ratio.
00:48
So what we're given in this problem is it says that we are trying to produce 20 .0 moles of the no.
00:59
And we want to know how many moles of oxygen are needed to do this.
01:05
That's what we're trying to find.
01:07
So we can use the mole ratio between oxygen and no as our conversion factor to calculate our answer.
01:16
Let's go ahead and set this up, see what this looks like, and then solve for our answer.
01:20
So we're starting with 20 .0 moles of no.
01:24
When we're doing stoichiometry or using the mole ratio, it doesn't matter if we're starting with a reactant or a product...