So I completely understand this question and the steps that I am doing, however

Question

So I completely understand this question and the steps that I am doing, however need some help explaining how to write the actual rate law itself:

Given the following proposed mechanism, predict the rate law for the overall reaction

After cancelling the reaction intermediate (Cl) you are left with:

In previous rate problems I have done I am always left with K= whatever the rate is in brackets...however I've never had to do one like this

Would it be k = [Cl2] [2NO2]?????? and why

Thanks for any help

Explanation / Answer

Answer – We know the rate law contain the rate constant and the reactant concentration. We are given the reaction mechanism like slow step and fast step reaction and when we combine then we will get overall reaction.

We know the rate of reaction is determined in the slow step only, so we are looking for the slow step reaction reactant and which is present in the overall.

In this one we are given

NO2 + Cl2 -----> NO2Cl + Cl (slow)

NO2 + Cl ------> NO2Cl (fast)

Overall reaction – 2 NO2 + Cl2 -----> 2 NO2Cl

So in the slow step there is NO2 and Cl2 , these both are present in the overall reaction

So rate is depending on the NO2 and Cl2 , so rate law is

Rate = k[NO2] [Cl2]

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