Problem: Use the rate laws given below to determine which reaction is most likely to occur in a single step. a. 2NO2 + F2 → 2NO2F           Rate = k[NO2] [F2] b. H2 + Br2 → 2HBr                  Rate = k[H2] [Br]1/2 c. NO + O2 → NO2 + O            Rate = k[NO] [O2] d. NO2 + CO → NO + CO         Rate = k[NO2]2

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Use the rate laws given below to determine which reaction is most likely to occur in a single step. 

a. 2NO2 + F2 → 2NO2F           Rate = k[NO2] [F2

b. H2 + Br2 → 2HBr                  Rate = k[H2] [Br]1/2 

c. NO + O2 → NO2 + O            Rate = k[NO] [O2

d. NO2 + CO → NO + CO         Rate = k[NO2]2

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