The following reaction exhibits the rate law: Rate = k[NO2]^2[Cl2].

2NO(g)+Cl2(g)---->2NOCl (g)

(a) Explain why the following mechanism is not plausible for this reaction.
Fast: NO + Cl2<-->NOCl + Cl

Slow: NO + Cl---->NOCl

(b) Propose a two-step mechanism involving one fast reversible step and one slow step that is consistent with the net equation and the observed rate law.

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