Full description please on how you find the answer :) The rate equation for the

Question

Full description please on how you find the answer :)

The rate equation for the reaction 2NO(g) + Br_2(g) rightarrow 2NOBr(g) was determined experimentally to be: Rate = k[NO]^2[Br_2] Five possible mechanisms have been proposed (i) - (v). Determine the rate equation for each mechanism below and then decide with reasons, (based on the information given) which mechanism is the most likely. (i) 2NO(g) + Br_2 (g) rightarrow 2NOBr (g) (ii) NO (g) + Br_2 NOBr_2 (g) NOBr_2 (g) + NO(g) rightarrow 2NOBr (g) (iii) Br_2 Br + Br Br + NO (g) rightarrow NOBr (g) Br + NO (g) rightarrow NOBr (g) (iv) NO (g) + Br_2(g) rightarrow NBr_2 (g) fast NBr_2 (g) + O_2 (g) rightarrow 2NOBr (g) slow (v) 2NO (g) rightarrow N_2O_2 (g) slow N_2 O_2 (g) + Br_2 (g) rightarrow 2NOBr (g) fast

Explanation / Answer

From the rate law the order of the reaction with respect to NO is 2 & with respect to Br2 is 1

So in the chemical reaction the number of moles of NO are 2 & that of Br2 is 1.

This is possible only in case (i)

Therefore (i) is correct.

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