The experimentally determined rate law for

At 225 degrees Celsius nitrogen dioxide NO2 reacts with carbon monoxide CO to produce carbon dioxide CO2 and nitrogen monoxide NO according to the following equation.NO2(g) CO(g) = CO2(g) NO(g)The experimentally determined rate law for the reaction is Rate=kobs[NO2]^2and NO3(g) has been experimentally identified as an intermediate in the reaction.a.) Explain why the mechanism for this reaction CANNOT consist of a single step; that is based on the experimental data provided above why must the reaction mechanism involve more than one step?b.) Assuming that the reaction mechanism does NOT involve a fast pre-equilibrium step propose a two-step mechanism for this reaction that satisfies the two tests discussed in lecture and explain your reasoning.