Experiments show that each of the following redox reactions is second-order overall: (1) NO2(g) + CO(g) → NO(g) + CO2(g) (2) NO(g) + O3(g) → NO2(g) + O2(g) (a) When [NO2] in reaction 1 is doubled, the rate quadruples. Determine the rate law for this reaction. Rate = k[NO2]4[CO]−2 k[NO2][CO] k[NO2]2 k[NO2]3[CO]−1 (b) When [NO] in reaction 2 is doubled, the rate doubles. Determine the rate law for this reaction. Rate = k[NO]2 k[NO][O3] k[NO]2[O3]2 k[O3]2 (c) In each reaction, the initial concentrations of the reactants are equal. For each reaction, what is the ratio of the initial rate to the rate when the reaction is 50% complete? Reaction 1 Ratei Rate50% = Reaction 2 Ratei Rate50% = (d) In reaction 1, the initial [NO2] is twice the initial [CO]. What is the ratio of the initial rate to the rate at 50% completion? Ratei Rate50% = (e) In reaction 2, the initial [NO] is twice the initial [O3]. What is the ratio of the initial rate to the rate at 50% completion? Ratei Rate50% =