00:01
So here we have a two -step reaction where the overall reaction we're looking for is 2n0 plus cl2 becoming 2nocl.
00:15
So the two steps that we propose have to add up to this.
00:18
So we have a first step.
00:20
We're told it's the fast step.
00:22
That's in equilibrium.
00:24
And then we have the second step, which we're told is the slow step.
00:27
And so, you know, really this is sort of a guess and check approach where we got to figure out.
00:31
Some way, you know, some mechanism and then see if it matches the rate law that we should expect.
00:40
And then from there, we can see if it's correct or not.
00:45
And so an example of what we could do is we could say, okay, well, we need to start with one of these.
00:51
Let's start with cl2.
00:53
That be that's something that can react pretty easily to break up into two cls.
00:59
So that's a start.
01:00
And so then just this two cl is going to be an interesting.
01:03
Intermediate, it's not part of the total reaction.
01:05
We would also need to react in the second step.
01:08
Now, the only other thing that's left to react is 2no.
01:14
And so this works out nicely.
01:15
We can see that we can have 2 cls and 2 nos form 2 nocls.
01:22
And so this is, this is an idea.
01:24
Now, or the real important step is that we test whether this works.
01:28
And so this is the slow step.
01:30
So this is the rate determining step that we're going to base our rate off of.
01:34
Now, before we're, we're we go and write some rate laws, i'm going to describe, i'm going to put some rate constants here.
01:39
We're going to have k1, k1, k1 is going to be the rate constant for the forward reaction for the first, for the first step, k -negative 1 is for the second step...