NO2 + CO Ã NO + CO2 Reaction rate = k[NO2]2 Given the equation and rate law above, what is the overall reaction order

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At temperatures below 500 K, the reaction between carbon monoxide and nitrogen dioxide
CO (g) + NO₂ (g) ? CO₂ (g) + NO (g)
has the following rate equation: Rate = k[NO₂]². Which of the three mechanisms suggested here agrees with the experimentally observed rate equation?
Mechanism 1: Step 1 Slow NO₂ + NO₂ ? NO₃ + NO
Step 2 Fast NO₃ + CO ? NO₂ + CO₂
Mechanism 2: Step 1 Fast NO₂ + NO₂ ? N₂O₃ + O
Step 2 Slow N₂O₃ + O + CO ? CO₂ + NO₂ + NO
Mechanism 3: CO + NO₂ ? CO₂ + NO