For the reaction, $\mathrm{NO}_{2(\mathrm{~g})}+\mathrm{CO}_{(\mathrm{g})} \longrightarrow…

For the reaction, $\mathrm{NO}_{2(\mathrm{~g})}+\mathrm{CO}_{(\mathrm{g})} \longrightarrow \mathrm{NO}_{(\mathrm{g})}+\mathrm{CO}_{2(\mathrm{~g})}$ rate of reaction is proportional to square of [ $\mathrm{NO}_2$ ] and independent of [CO]. What is the rate law equation?
  1. $r=k \frac{\left[\mathrm{NO}_2\right]^{\frac{1}{2}}}{[\mathrm{CO}]}$
  2. $\mathrm{r}=\mathrm{k}\left[\mathrm{NO}_2\right]^2[\mathrm{CO}]^0$
  3. $\mathrm{r}=\frac{1}{2} \mathrm{k}\left[\mathrm{NO}_2\right][\mathrm{CO}]$
  4. $\mathrm{r}=\mathrm{k}\left[\mathrm{NO}_2\right]^2[\mathrm{CO}]$

Solution

The correct rate law equation is: (B) $r=k \times\left[\mathrm{NO}_2\right]^2 \times[\mathrm{CO}]^0$, which simplifies to $r=k \times\left[\mathrm{NO}_2\right]^2$.

Asked in: MHT CET 2024 (09 May Shift 1)

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