Problem 1 (4+3+3=10 points). The gas-phase oxidation of nitric oxide involves the following two elementary reactions: Step 1: 2N0 = N202 with rate constants k,r and k1, for the forward and reverse directions, respectively. Step 2: N202 + O2 + 2N02 with the rate constant k2 for this complete reaction. a/Write the differential equations for the time evolution of the following concentrations: [NO] for step 1 and [N202] for step2. b/ It is observed that step 1 is very fast compared to step 2. What simplification can you then make in the differential equations found in a/? c/Write the overall oxidation reaction by combining step 1 and step 2. Use your answer in b/to propose an overall reaction rate for the consumption of [O2), and then for the overall rate of consumption of [NO). What is the overall order of this reaction? What is its partial order with respect to [NO]