AP Chemistryhardmcq1 pt
A mechanism has these steps: NO + NO ⇌ N₂O₂ (fast equilibrium); N₂O₂ + O₂ → 2NO₂ (slow). What is the predicted rate law?
A.rate = k[NO]²[O₂]
B.rate = k[N₂O₂][O₂]
C.rate = k[NO]²
D.rate = k[NO][O₂]
Explanation
Core Concept
The slow step gives rate = k₂[N₂O₂][O₂]. From the fast equilibrium, [N₂O₂] = K₁[NO]². Substituting removes the intermediate: rate = k₂K₁[NO]²[O₂].
Correct Answer
Arate = k[NO]²[O₂]
More Unit 5: Kinetics practice questions
- mediumA first-order decomposition has a half-life of 12 minutes. What percentage of the original reactant concentration remains after 36 minutes?
- hardWhat is the overall order of a reaction with rate = k[A]⁰[B]²?
- hardWhich energy-profile feature distinguishes a catalyzed pathway from an uncatalyzed one?
- hardAn experiment tracks [A] over time and finds the half-life doubles as [A]₀ halves. What is the reaction order?
- hardWhich reaction is expected to be fastest at room temperature?
Practice more AP Chemistry questions with full explanations
Practice Unit 5: Kinetics Questions →