00:03
Hi there.
00:03
In this question, we have a percent yield problem.
00:08
And percent yield is defined as the actual yield, which you actually get when you conduct the experiment, divided by the theoretical yield, what you expect to get based upon a mathematical calculation.
00:28
In other words, stoichiometry.
00:32
Dividing these two gives you a decimal number.
00:35
So to express it as a percent, you multiply by 100, and add the percent.
00:39
Sign.
00:41
Okay.
00:43
In this question, we are given the percent yield.
00:47
We are told that it is 35 .3 percent.
00:55
And what we're trying to determine is the actual yield.
01:04
But to calculate that, we need the theoretical yield.
01:10
So let's look back up at our equation here.
01:13
Our theoretical yield is what is calculated by stoichiometry, what we would expect to get.
01:20
So we are starting with five moles of the n2.
01:30
And we want to calculate how much nh3 in moles should be produced.
01:39
Right.
01:39
So this is a one -step calculation where we're going to use our mole ratio.
01:44
Mole ratio comes from the coefficients in the balanced equation.
01:47
Since nothing is in front of the nitrogen, we see that it's a one.
01:51
So for every one mole of nitrogen that we start with, theoretically we should make two moles of ammonia...