For the reaction `NO_(2)+CO to CO_(2)+NO`, the rate law is : Rate `=k[NO_(2)]^(2)`. Propose the probable mechanism of this reaction.

Nitric oxide (NO) reacts with oxygen to produce nitrogen dioxide (NO_(2)) : 2NO(g) + O_(2) to 2NO_(2) (g) The rate law for the reaction is: rate = k[NO]^2[O_(2)] Propose a mechanism for the above reaction.

Nitric oxide, NO, reacts with oxygen to produce nitrogen dioxide : 2NO(g)+O_(2)(g)to2NO_(2)(g) The rate law for this reaction is : Rate =k[NO]^(2)[O_(2)]. Propose a mechanism for the above reaction.

For a reaction, Cl_(2)(g) + 2NO(g) to 2NOCl(g) ,the rate law is expressed as rate = k[Cl_(2)][NO]^(2) . What is the order of the reaction?

For the chemical reaction, 4" HBr"+"O"_(2)to2"H"_(2)"O"+2" Br"_(2) , Rate =k["HBr"]["O"_(2)]. What is the probable mechanism of the reaction ?

For the reaction , NO_(2)(g)+CO(g)toNO(g)+CO_(2)(g) At temperatures below 500K , the rate law is rate =k[NO_(2)]^(2) which mechanism is consistent with this information? Mechanism1: NO_(2)+NO_(2)toNO_(3)+NO ("slow") CO+NO_(3)toCO_(2)+NO_(2)("fast") Mchanism2: NO_(2)+NO_(2)toNO_(3)+NO ("fast") CO+NO_(3)toCO_(2)+NO_(2)("slow")

Under certain conditions the reaction of CO with NO_(2) to give CO_(2) and NO results in the rate law , rate = k[CO][NO_(2)] . What are the units for the rate constant, k?