Consider the reactions: O_3(~g)+H_2 O_2(l) H_2 O(l)+2 O_2(~g) Why… - Vidyadip

Question

Consider the reactions: $\mathrm{O}_3(\mathrm{~g})+\mathrm{H}_2 \mathrm{O}_2(\mathrm{l}) \rightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{l})+2 \mathrm{O}_2(\mathrm{~g})$ Why it is more appropriate to write these reactions as:
$\mathrm{O}_3(\mathrm{~g})+\mathrm{H}_2 \mathrm{O}_2(\mathrm{l}) \rightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{l})+\mathrm{O}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g})$
Also suggest a technique to investigate the path of the above redox reactions.

✓

Answer

$\mathrm{O}_2$ is produced from each of the two reactants $\mathrm{O}_3$ and $\mathrm{H}_2 \mathrm{O}_2$. For this reason, $\mathrm{O}_2$ is written twice. The given reaction involves two steps. First, $\mathrm{O}_3$ decomposes to form $\mathrm{O}_2$ and O . In the second step, $\mathrm{H}_2 \mathrm{O}_2$ reacts with the O produced in the first step, thereby producing $\mathrm{H}_2 \mathrm{O}$ and $\mathrm{O}_2$.
$\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{O}_{3(\text{g})}\xrightarrow{\ \ \ \ \ \ \ \ }\text{O}_{2(\text{g})}+\text{O}_{(\text{g})}\\ \ \ \ \text{H}_2\text{O}_{2(\text{l})}+\text{O}_{(\text{g})}\xrightarrow{\ \ \ \ \ \ \ \ }\text{H}_2\text{O}_{(\text{l})}+\text{O}_{2(\text{g})}\\\overline{\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ }\\\text{H}_2\text{O}_{2(\text{l})}+\text{O}_{3(\text{g})}\xrightarrow{\ \ \ \ \ \ \ \ \ \ }\text{H}_2\text{O}_{(\text{l})}+\text{O}_{2(\text{g})}+\text{O}_{2(\text{g})}$
The path of this reaction can be investigated by using $\text{H}_2\text{O}_2^{18}$ or $\text{O}_3^{18}.$

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