Step 1: HBr + O2 ---> HOOBr Step 2: HBr + HOOBr ---> 2HOBr Step 3: 2HBr + 2HOBr

Question

Step 1: HBr + O2 ---> HOOBr Step 2: HBr + HOOBr ---> 2HOBr Step 3: 2HBr + 2HOBr ---> 2H2O + 2Br2 For the reaction above, I know that the two intermediates are HOOBr and HOBr. The question I have is: If I were unable to detect either of the intermediates among the products, would this disprove my mechanism? Am I correct to think that it would not disprove my mechanism because the products of the initial reactions, step 1 and 2, are used up in subsequent reactions to form the desired final products of H2O and Br2. I would appreciate a correction in my thinking if I am incorrect.

Explanation / Answer

yes you are correct to think that it would not disprove the mechanism because the formation of intermediates is by slow step which is an important step in rate law mechanisms . Hence if we are not able to detect intermediates among products then we can easily go for slowest step mechanism to determine the intermediates

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