The reaction of Nitric Oxide (NO(g)) with molecular hydrogen (H2(g)) results in the production of molecular Nitrogen and water as follows; 2 NO(g) + 2 H2(g) --> N20(g) + 2 H2O(g) The experimentally determined rate-law expression for this reaction is first order in H2(g) and second order in NO(g). a.) Is the reaction as written consistent with the experimentally determined rate-law? b.) An alternative mechanism for the reaction is; k1 2 NO(g) <=> N2O2(g) [fast] k-1 k2 H2(g) + N2O2(g) --> N2O(g) + H2O(g) k3 H2(g) + N2O(g) --> N2(g) + H2O(g) Show that this mechanism is consistent with the experimental rate law.