00:01
In this problem, we're given this mechanism for the gas phase reaction of nitrogen dioxide with carbon monoxide to form nitric oxide and carbon dioxide.
00:08
We're first asked to write the rate law, and then we're asked to write the overall balanced equation.
00:14
So in order to write the rate law, what we're going to need to evaluate is which of these steps is slower.
00:23
And in order to do that, we can look at the stability of the reactants, because a less stable reactant is more reactive.
00:31
It will sooner form more stable products.
00:35
So, for instance, nitrogen dioxide is a fairly stable compound.
00:41
So we can assume that this step to form nitrogen trioxide and nitrogen monoxide, which are both relatively unstable in comparison, to be a relatively slow step of reaction.
00:53
Whereas the next step, we have nitrogen trioxide and carbon monoxide.
00:57
Carbon monoxide, we know to be pretty reactive.
00:59
And nitrogen trioxide, as i previously stated, is pretty reactive to form these relatively less reactive products.
01:06
So we can assume that this is a fast step of reaction.
01:14
And now that we have this information, we can write the rate wall.
01:16
The rate is determined solely from the slowest step...