00:01
To verify that each of these mechanisms correspond with the actual rate law of rate equals k multiplied by the concentration of no squared multiplied by the concentration of o2, we always start with a slow step.
00:14
So for mechanism 1, we'll start with the rate determining step, the slow step, which gives us a rate law of rate is equal to k prime, multiplied by the concentration of n03, multiplied by the concentration of n03, however, is an intermediate, so we need to get rid of it by recognizing.
00:30
That the first step in mechanism one is fast and reversible, so the rate in the forward direction expressed as kf multiplied by n0 and o2 will be equal to the rate in the reverse direction expressed as kr multiplied by the n .o3 concentration.
00:45
So the n .o3 concentration then is this expression, which can be substituted into a rate law for the slow step, getting rid of the intermediate, and when we combine all three of these k values into a single k value, we do get the rate law for the overall reaction...