I need to propose a 2-step reaction mechanism for the following reaction:
$$2NO_2Br\rightarrow 2NO_2+Br$$$$\ce{2NO2Br -> 2NO2 +Br}$$
And prove the mechanism is consistent with: $$v=k[NO_2Br]^2$$$$v=k[\ce{NO2Br}]^2$$
For the mechanism to be consistent with the rate equation, the first equation would have to be the limiting one and also be in this form:
$$2NO_2Br\rightarrow Products$$$$\ce{2NO_2Br -> Products}$$
I've tried using:
$$2NO_2Br\rightarrow N_2O_4+Br_2$$$$\ce{2NO2Br -> N2O4 +Br2}$$
$$N_2O_4\rightarrow 2NO_2$$$$\ce{N2O4 -> 2NO2}$$
But the problem with this mechanism is that N2O4$\ce{N2O4}$ is not unstable enough to be consumed immediately.
Any help with this problem?
Would also appreciate some advice on proposing reaction mechanisms. Thank you.
Replaced math formatting with chemistry formatting.
