The reaction 2 NO+Br_2 2 NOBr takes places through the mechanism given below: NO+Br_2 NOBr_2 (fast) NOBr_2+NO 2 NOBr (slow) The overall order of the reaction is ___________.

Rate K[NOBr_2] [NO] [RDS] \\ k_eq=[NOBr_2][NO][Br_2] [NOBr_2]=\\ K_eq[NO][Br_2] \\ Rate =K_eq[NO][Br_2] K[NO] \\ =K_eq ~K[NO]^2[Br_2]\\ Overall order =2+1=3

The reaction 2 NOBr2 arrow 2 NOBr takes places through the m: (Chemistry)

Rate $\mathrm{K}\left[\mathrm{NOBr}_2\right] \quad[\mathrm{NO}] \quad[\mathrm{RDS}] \\$

$\mathrm{k}_{\mathrm{eq}}=\frac{\left[\mathrm{NOBr}_2\right]}{[\mathrm{NO}]\left[\mathrm{Br}_2\right]} \Rightarrow\left[\mathrm{NOBr}_2\right]$ = $\\ \mathrm{K}_{\mathrm{eq}}[\mathrm{NO}]\left[\mathrm{Br}_2\right] \\$

Rate $=\mathrm{K}_{\mathrm{eq}}[\mathrm{NO}]\left[\mathrm{Br}_2\right] \mathrm{K}[\mathrm{NO}] \\$

$=\mathrm{K}_{\mathrm{eq}} \mathrm{~K}[\mathrm{NO}]^2\left[\mathrm{Br}_2\right]\\$

Overall order =2+1=3

Explanation

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