Kinetics Quiz #3 Collision Theory Answers
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- D. Effective collisions lead to chemical reactions
- D. Decreasing the activation energy of the overall reaction
- C . A decrease in the fraction of particles possessing sufficient energy
- C. Increases and more are effective
- B. Supplies activation energy
- D. An increase in the frequency of successful collisions
- D. CH 4 Cl 2 lower
- C. the activation energy stays the same
- C. It reduces the required activation energy.
- D. particles have sufficient KE and good molecular orientation
- A. more collisions and greater collision energy
- B. more collisions but the same collision energy
| Kinetics Quiz #3 Collision Theory Answers
1. Which of the following are necessary for successful collisions to occur? I Favorable collision geometry II Sufficient Kinetic energy III Large ∆H
A. I only B. I and II only C. II and III only D. I, II, and III
B. Most collisions lead to chemical reactions C. Very few reactions involve particle collisions
B. Decreasing the concentration of the reactant(s) C. Increasing the activation energy of the overall reaction
B. A decrease in ∆H for the reaction C. A decrease in the fraction of particles possessing sufficient energy D. The introduction of an alternate pathway with greater activation energy 5. In general, a chemical reaction requiring a large activation energy will proceed A. At a fast rate B. At a slow rate C. Only at a low temperature D. Only at low concentrations
B. Decreases and fewer are effective C. Increases and more are effective D. Decreases but more are effective 7. The minimum amount of energy needed to start a reaction is called the A. Activation energy B. Energy of a reaction C. Entropy of a reaction. D. Reaction mechanism energy 8. When a lit match is touched to the wick of a candle, the candle begins to burn. When the match is removed, the candle continues to burn. In this reaction, the match A. Behaves as a catalyst B. Supplies activation energy C. Is part of the rate-determining step D. Lowers the activation energy barrier 9. Consider the following collisions, each one occurring at the same temperature Before Collision Collision After Collision 
Which one of the following factors explains why collision one is successful while collision two is not successful? A. Catalyst B. Geometry C. Concentration
10. Consider the following factors I Reactant particles collide II Sufficient kinetic energy is present III A favorable geometry exists IV Catalysts are present Which combination of the above factors is required for successful collisions
B. II and III only C. I, II, and III only D. I, II, III, and IV 11. To increase the rate of a reaction, there must be A. Decrease in the frequency of collisions B. An Increase in the frequency of collisions. C. A decrease in the frequency of successful collisions
B. Sufficient heat of reaction only C. Sufficient potential energy only
CH4 + Cl2 → CH2Cl2 + H2 Which answer best describes the activated complex? Formula KE relative to reactants A. CH4 higher B. CH4 lower C. CH4Cl2 higher
B. changing the surface area C. changing the reactant concentration D. changing the average kinetic energy 15. Which of the following would change the value of the activation energy for a heterogeneous reaction? A. adding an inhibitor B. changing the surface area C. changing the temperature D. changing the average kinetic energy 16. What happens to the activation energy as the temperature in a reacting system decreases? A. the activation energy increases B. the activation energy decreases
D. the activation energy is converted to kinetic energy 17. How does the addition of a catalyst increase the reaction rate of an endothermic reaction? A. It reduces the ΔH of the reaction. B. It increases the ΔH of the reaction.
D. It causes the reaction to become exothermic. 18. Which of the following would result in a successful collision between reactant particles? A. particles have sufficient KE B. particles convert their entire PE into KE C. particles are in an excited state and are catalyzed D. particles have sufficient KE and good molecular orientation 19. A spark causes propane gas to explode. According to the collision theory, the spark: A. lowered the Ea B. increased the Ea C. provided the Ea D. acted as a catalyst 20. Consider the following reaction: 2H2O2(aq) → O2 + 2H2O(l) A small amount of KI is added and the reaction rate increases. The best explanation is that KI:
B. causes more collisions C. causes harder collisions D. increases the temperature 21. The reaction temperature is increased. There are: A. more collisions and greater collision energy B. more collisions but the same collision energy C. the same number of collisions and greater collision energy D. the same number of collisions but the same collision energy 22. A reactant concentration is increased. There are: A. more collisions and greater collision energy B. more collisions but the same collision energy C. the same number of collisions and greater collision energy D. the same number of collisions but the same collision energy
A. more collisions and greater collision energy B. more collisions but the same collision energy C. the same number of collisions and greater collision energy D. the same number of collisions but the same collision energy
B. successful collisions have favourable geometry C. successful collisions have sufficient energy D. a collision is required Download 33.32 Kb. Share with your friends:
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