(A) In a proposed two-step mechanism for the reaction CO(g) + NO₂(g) → CO₂(g) + NO(g), the second, fast step is NO₃(g) + CO(g) → NO₂(g) + CO₂(g). What must be the slow step? What would you expect the rate law of the reaction to be? Explain.

(B) Show that the proposed mechanism for the reaction 2 NO₂(g) + F₂(g) → 2 NO₂F(g) is plausible. The rate law is rate = k[NO₂][F₂].

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Fast: NO₂(g) + F2(g) = NO₂F2(g) Slow: NO₂F₂(g) Fast: F(g) + NO₂(g) NO₂F(g) + F(g) NO₂F(g)