For the reaction `NO_(2)+COrarrCO_(2)+NO`, the experimental rate expresison is `-dc//dt = k[NO_(2)]^(2)`. Find the number of molecules of `CO` involved in the slowest step.

For the reaction: 2HIrarr H_(2)+I_(2) , the expresison -d(HI)//2dt represents

For the reaction NO_(2)(g) + CO(g) to NO(g) + CO_(2)(g) , the experimentally determined rate expression at 40 K is: rate = k[NO_(2)]^(2) What is the proposed mechanism for the reaction?

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.

For the reaction NO_2 + CO to CO_2 + NO , the experimentally determined rate expression below 400 K is rate = k[NO_2]^2 . What mechanism can be proposed for this reaction ?