A reaction intermediate is a short-lived, high-energy molecule formed during a chemical reaction. It is not present in the initial reactants or final products, but rather forms and reacts in the middle of the reaction pathway.
In the given reaction:
step 1 O3 ----> O2 + O
step 2 O3 + O ---> 2O2
The oxygen atom (O) is a reaction intermediate because it is formed in step 1 and then consumed in step 2. It is not present in the initial reactant (O3) or the final product (O2). So, the oxygen atom is a reaction intermediate.
A catalyst, on the other hand, would be a substance that participates in the reaction but is not consumed in the overall reaction. A catalyst would be present in both the reactants and the products of the reaction. In this case, there is no substance that fulfills this criterion, so there is no catalyst in this reaction.
The decomposition of ozone may occur through the two-step mechanism shown below:
step 1 O3 ----> O2 + O
step 2 O3 + O ---> 2O2
The oxygen atom is considered to be: a catalyst or reaction intermediate?
How am I supposed to be able to tell the difference between the two? I know a catalyst speeds up a reaction without be consumed, but I'm not sure on how to be able to identify a reaction intermediate.
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