The rate law for the reaction $2 \mathrm{NO}_{(\mathrm{g})}+\mathrm{O}_{2(\mathrm{~g})} \longrightarrow 2…

The rate law for the reaction $2 \mathrm{NO}_{(\mathrm{g})}+\mathrm{O}_{2(\mathrm{~g})} \longrightarrow 2 \mathrm{NO}_{2(\mathrm{~g})}$ is rate $=\mathrm{k}[\mathrm{NO}]^{2}\left[\mathrm{O}_{2}\right]$, then which among the following statement is correct?
  1. The reaction is first order in $\mathrm{O}_{2}$, first order in NO and second order overall.
  2. The reaction is second order in NO, zero order in $\mathrm{O}_{2}$ and second order overall.
  3. The reaction is second order in $\mathrm{NO}$, first order in $\mathrm{O}_{2}$ and third order overall.
  4. The reaction is zero order overall.

Solution

Rate $=k[\mathrm{NO}]^{2}\left[\mathrm{O}_{2}\right]$ Here, $x=2, y=1$ Overall order of reaction $=x+y=3$

Asked in: MHT CET 2020 (13 Oct Shift 1)

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