Suppose the reaction between nitric oxide and oxygen proceeds by the following mechanism: step elementary reaction rate constant 1 NO (g)+0, (g) - NO, (g)+0 (g) ky NO (g) +0 (g) - NO, (g) k2 Suppose also k, « k,. 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. rate = Note: your answer should not contain the concentrations of any intermediates.

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