00:01
Okay, so we're given two different reactions here, and we're given the rate of creating, for instance, in the first one, nh3.
00:10
We're told that the rate of creation of nh3 is 0 .032 moles per liter per second.
00:17
And we want to know what the rate of disappearance is for the two reactants.
00:21
And what we're going to do is we're going to use the mole ratio to be able to figure that out for each.
00:27
First of all is we have, if we're using our reactants, the sign of the rate is going to be negative.
00:36
So since this is going to disappear, it's going to be negative.
00:40
And we're going to start out with our 0 .032 moles per liter per second of nh3, what we were given.
00:49
Now we're going to convert that.
00:52
What we know is from the balanced chemical equation that for every two moles of nh3, that get made, we use one mole, because the coefficient, if there is none is one, we use one mole of then two.
01:09
So when we do the math on that, it's gonna be negative 0 .016 moles per liter per second.
01:18
We can do the same thing for the h2.
01:22
We're gonna start out with our given amount of molarity per second of ammonia.
01:28
But this time our mole ratio, we use 3 moles of h2 for every 2 moles of nh3, again based on the balanced chemical equation...