Suppose the formation of nitrogen dioxide proceeds by the following mechanism: elementary reaction step rate constant 1 2 NO(g) N2O2(g) k₁ 2 N2O2(g) + O2(g) → 2 NO2(g) k2 Suppose also k₁»k2. That is, the first step is much faster than the second. Suppose also k₁»k2. That is, the first step is much faster 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. rate = k 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. k = 0