If decomposition of hydrogen peroxide is a first order reaction, it's rate law equation can be represented as

If decomposition of hydrogen peroxide is a first order reaction, it's rate law equation can be represented as
  1. $\mathrm{r}=\frac{\mathrm{k}}{\left[\mathrm{H}_2 \mathrm{O}_2\right]}$
  2. $\mathrm{r}=\mathrm{k}\left[\mathrm{H}_2 \mathrm{O}_2\right]$
  3. $\mathrm{r}=\mathrm{k} \frac{\left[\mathrm{H}_2 \mathrm{O}\right]\left[\mathrm{O}_2\right]^{1 / 2}}{\left[\mathrm{H}_2 \mathrm{O}_2\right]}$
  4. $\mathrm{r}=\mathrm{k} \frac{\left[\mathrm{H}_2 \mathrm{O}_2\right]}{\left[\mathrm{H}_2 \mathrm{O}_2\right]\left[\mathrm{O}_2\right]^{1 / 2}}$

Solution

$\mathrm{H}_2 \mathrm{O}_2 \longrightarrow \mathrm{H}_2 \mathrm{O}+\frac{1}{2} \mathrm{O}_2$ Reaction is first order reaction. Rate law equation can be represented as, $\mathrm{R}=\mathrm{k}\left[\mathrm{H}_2 \mathrm{O}_2\right]^1$

Asked in: MHT CET 2021 (23 Sep Shift 1)

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