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
2. Collision theory states that
A. All collisions lead to chemical reactions
B. Most collisions lead to chemical reactions
C. Very few reactions involve particle collisions
D. Effective collisions lead to chemical reactions
3. A catalyst increases the rate of a reaction by
A. Increasing the concentration of the reactant(s)
B. Decreasing the concentration of the reactant(s)
C. Increasing the activation energy of the overall reaction
D. Decreasing the activation energy of the overall reaction
4. Milk is refrigerated in order to slow the rate of decomposition by bacterial action.
The decrease in reaction rate is due to
A. A decrease in surface area
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

6. Consider the following reaction:
Mg
(s)
+ 2HCl
(aq)
→ MgCl
2(aq)
+ H
2(g)
As the temperature of the above system is increased, the number of collisions
A. Increases but fewer are effective
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

Collision 1
9. Consider the following collisions, each one occurring at the same temperature
Collision After Collision Before Collision
F F
F
N
O
F
N
F
O
O
F
N
O
O O
F F
F F
Collision 2
O
N
O
F
O
N
F
O
O
N
O
Which one of the following factors explains why collision one is successful while collision two is not successful?
A. Catalyst
B. Geometry
C. Concentration
D. Kinetic energy

10. Consider the following factors
I
II
III
Reactant particles collide
Sufficient kinetic energy is present
A favorable geometry exists
IV Catalysts are present
Which combination of the above factors is required for successful collisions
A. I only
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
D. An increase in the frequency of successful collisions
12. For collisions to be successful, reactants must have
A. Favorable geometry only
B. Sufficient heat of reaction only
C. Sufficient potential energy only
D. Sufficient kinetic energy and favorable geometry
13. Consider the following reaction:
CH
4
+ Cl
2
→ CH
2
Cl
2
+ H
2
Which answer best describes the activated complex?
Formula KE relative to reactants
A. CH
4
B. CH
4 higher lower
C. CH
4
Cl
2
higher
D. CH
4
Cl
2
lower
14. Which of the following would change the value of the activation energy for a heterogeneous reaction?
A. adding a catalyst
B.
C.
D. changing the surface area changing the reactant concentration 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
C. the activation energy stays the same
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
Δ
H of the reaction.
B. It increases the
Δ
H of the reaction.
C. It reduces the required activation energy.
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.
B. lowered the Ea increased the Ea
C.
D. provided the Ea acted as a catalyst
20. Consider the following reaction:
2H
2
O
2(aq)
→ O
2
+ 2H
2
O
(l)
A small amount of KI is added and the reaction rate increases. The best explanation is that KI:
A.
B.
C. is a catalyst causes more collisions causes harder collisions
D. increases the temperature
21. The reaction temperature is increased. There are:
A.
B.
C. more collisions and greater collision energy more collisions but the same collision energy 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
23. A reactant surface area is increased. There are:
A. more collisions and greater collision energy
B.
C.
D. more collisions but the same collision energy the same number of collisions and greater collision energy the same number of collisions but the same collision energy
24. In a chemical reaction, which of the following is not true?
A.
B.
C.
D. most collisions are successful successful collisions have favourable geometry successful collisions have sufficient energy a collision is required