Suppose the reaction between nitric oxide and oxygen proceeds by the following mechanism: step elementary reaction rate constant (g) (g) (g) (g) (g) (g) (g) Suppose also ≪. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally-observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k-1 and k-2 for the reverse of the two elementary reactions in the mechanism.