Suppose the reaction between nitric oxide and oxygen proceeds by the following mechanism: step elementary reaction rate constant 1 NO(g) + O₂(g) → NO₂ (g) + O (g) k₁ 2 NO (g) + O(g) → NO₂ (g) k₂ Suppose also k₁ « k₂. 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. 0 rate = &

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