Answer:
Kindly check the explanation section.
Step-by-step explanation:
Just like it is given or said in the question/problem above we have that the catalytic destruction of ozone occurs via a two-step mechanism. The two step mechanism in which one of the step is fast and the other step is slow is given in the reaction below;
=> X + O3 --------------------------> XO + O2.
This the slow step.
The rate law for the slow step = k(slow) [X][O3].
=> XO + O ---------------------------> X + O2.
This is the fast step.
The rate law for the fast step = k(fast) [XO][O].
Therefore, the overall reaction involves the cancellation of the two XOs present in the first and second step respectively and cancellation of Xs present In the first and second step respectively.
Therefore, the overall reaction gives;
O3 + O ----------------------------------> 2O2.
Note that the XO stands for the intermediate while the X stand for the catalyst.