Suppose the reduction of nitric oxide proceeds by the following mechanism: step elementary reaction rate constant H,(g) + 2 NO(g) → N20(g) + H,O(g) k1 1 2 H,(g) + N,0(g) → N2(9) + H2O(g) k2 Suppose also k,»k,. 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. rate = k || 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 k the reverse of the two elementary reactions in the mechanism.

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