Question
Consider the reactions: O3(g) + H2O2(l) → H2O(l) + 2O2(g)
Why it is more appropriate to write these reactions as:
O3(g) + H2O2(l) → H2O(l) + O2(g) + O2(g)
Also suggest a technique to investigate the path of the above redox reactions.✓
Answer
O2 is produced from each of the two reactants O3 and H2O2. For this reason, O2 is written twice. The given reaction involves two steps. First, O3 decomposes to form O2 and O. In the second step, H2O2 reacts with the O produced in the first step, thereby producing H2O and O2.
$\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{O}_{3(\text{g})}\xrightarrow{\ \ \ \ \ \ \ \ }\text{O}_{2(\text{g})}+\text{O}_{(\text{g})}\\ \ \ \ \text{H}_2\text{O}_{2(\text{l})}+\text{O}_{(\text{g})}\xrightarrow{\ \ \ \ \ \ \ \ }\text{H}_2\text{O}_{(\text{l})}+\text{O}_{2(\text{g})}\\\overline{\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ }\\\text{H}_2\text{O}_{2(\text{l})}+\text{O}_{3(\text{g})}\xrightarrow{\ \ \ \ \ \ \ \ \ \ }\text{H}_2\text{O}_{(\text{l})}+\text{O}_{2(\text{g})}+\text{O}_{2(\text{g})}$
The path of this reaction can be investigated by using $\text{H}_2\text{O}_2^{18}$ or $\text{O}_3^{18}.$Need a full question paper?
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