To determine which catalyzed reaction breaks up ozone, we need to identify the reaction that involves the decomposition of ozone (O₃).
Here are the reactions provided:
1. [tex]\( 2 H_2O_2(l) \xrightarrow{2+ O_2} 2H_2O(l) + O_2 \)[/tex]
2. [tex]\( O_3 + O \xrightarrow{\Delta} 2O_2 \)[/tex]
3. [tex]\( 2 H_2O_2(aq) \xrightarrow{Pt} 2H_2O(l) + O_2 \)[/tex]
4. [tex]\( O_2 + 2SO_2 \xrightarrow{NO} 2SO_3 \)[/tex]
Let's analyze each reaction to see which one involves the breakdown of ozone (O₃):
1. The first reaction involves hydrogen peroxide ([tex]\(H_2O_2\)[/tex]) breaking down into water ([tex]\(H_2O\)[/tex]) and oxygen ([tex]\(O_2\)[/tex]). This reaction does not involve ozone.
2. The second reaction shows ozone ([tex]\(O_3\)[/tex]) reacting with an oxygen atom (O) to form two molecules of oxygen ([tex]\(O_2\)[/tex]). This reaction clearly involves the decomposition of ozone.
3. The third reaction again involves hydrogen peroxide ([tex]\(H_2O_2\)[/tex]) breaking down into water ([tex]\(H_2O\)[/tex]) and oxygen ([tex]\(O_2\)[/tex]), but it does not involve ozone.
4. The fourth reaction involves oxygen ([tex]\(O_2\)[/tex]) reacting with sulfur dioxide ([tex]\(SO_2\)[/tex]) to form sulfur trioxide ([tex]\(SO_3\)[/tex]). This reaction does not involve ozone.
From this analysis, it's clear that the second reaction, [tex]\(O_3 + O \xrightarrow{\Delta} 2O_2\)[/tex], is the one that breaks up ozone (O₃). Therefore, the index of the correct reaction is 2.
