Suppose the formation of nitrogen dioxide proceeds by the following mechanism: elementary reaction rate constant 2NO(g) → N₂O₂(g) 2 N₂O₂(g) + O₂(g) 2 NO₂(g) Suppose also k₁ »k₂. That is, the first step is much faster than the second. step 1 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. 00 rate=& k = 0 k₁ k ローロ 00 X 2 S

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