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If decomposition of hydrogen peroxide is a first order reaction, it's rate law equation can be represented as
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Verified Answer
The correct answer is:
$\mathrm{r}=\mathrm{k}\left[\mathrm{H}_2 \mathrm{O}_2\right]$
$$
\mathrm{H}_2 \mathrm{O}_2 \longrightarrow \mathrm{H}_2 \mathrm{O}+\frac{1}{2} \mathrm{O}_2
$$
Reaction is first order reaction.
Rate law equation can be represented as,
$$
\mathrm{R}=\mathrm{k}\left[\mathrm{H}_2 \mathrm{O}_2\right]^1
$$
\mathrm{H}_2 \mathrm{O}_2 \longrightarrow \mathrm{H}_2 \mathrm{O}+\frac{1}{2} \mathrm{O}_2
$$
Reaction is first order reaction.
Rate law equation can be represented as,
$$
\mathrm{R}=\mathrm{k}\left[\mathrm{H}_2 \mathrm{O}_2\right]^1
$$
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