Chemistry 12
Unit 1 Provincial Practice
Chemistry 12
Unit 1 Provincial Practice Questions – Multiple Choice
1. As an activated complex changes into products, what changes occur in the chemical bonds
of the activated complex and the PE of the system?
A.
B.
C.
D.
Bonds
form
form
break
break
PE
increases
decreases
increases
decreases
2.
A.
B.
C.
D.
An activated complex can be described as
a particle of maximum KE and minimum PE.
a stable particle found in a reaction mechanism.
an unstable particle that is neither reactant nor product.
a particle which is first used then regenerated in a reaction mechanism.
3. When a catalyst is added to a reaction
I.
the enthalpy change of reaction increases
II. a new mechanism is provided
III. the activation energies for forward and reverse reactions are decreased

A. II only
B. I and II only
C. II and III only
D. I, II and III
4.
A.
B.
C.
D.
E.
A catalyst changes the rate of a reaction by ...
changing H.
increasing the temperature.
decreasing the energy of the products.
providing an alternate reaction mechanism.
increasing the number of collisions.
5. Which of the following changes will increase the average kinetic energy of reactant
molecules?
A. adding a catalyst
B. increasing the temperature
C. increasing the surface area
D. increasing the concentration
Unit 1 Provincial Practice 2/17/2016
Page 1
Chemistry 12
6. Collision theory states that...
A. all collisions lead to chemical reactions.
C. very few reactions involve particle
collisions.
E. reactions do not require particles to
collide.
Unit 1 Provincial Practice
B. most collisions lead to chemical reactions.
D. effective collisions lead to chemical
reactions.
7. Which of the following are necessary for successful collisions to occur?
I. Favourable collision geometry
II. Sufficient kinetic energy
III. Large H
A. I only
B. I and II only
C. II and III only
D. I and III only
E. I, II, and III
8. When a collision occurs between two reactant species which possess between them the
minimum kinetic energy, called activation energy, a product does not always form. This
may be a result of....
A. low temperature.
B. small surface area.
C. low concentrations.
D. unfavourable geometry.
E. a lack of a catalyst.
F.
9.
A.
B.
C.
D.
Which of the following would result in a successful collision between reactant particles?
particles have sufficient KE
particles convert all their PE into KE
particles are in an excited state and are catalyzed
particles have sufficient KE and proper molecular orientation
10. What happens to the activation energy as the temperature in a reacting system
increases?
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
Unit 1 Provincial Practice 2/17/2016
Page 2
Chemistry 12
Unit 1 Provincial Practice
11. Which of the following potential energy curves represents a catalyzed endothermic
reaction in the forward direction?

A.
B.
C.
D.
I
II
III
IV
12.
A.
B.
C.
D.
Activation energy is described as
the energy of the activated complex.
a point on the PE diagram where KE = PE.
the unstable high PE structural arrangement of atoms.
the minimum PE difference between the activated complex and the reactants.
13. Consider the following PE diagram:
What are the values of H and activation energy (Ea) for the forward reaction?
H (kJ)
A.
B.
C.
D.
-50
-50
+50
+50
Ea (kJ)
100
200
100
200
Unit 1 Provincial Practice 2/17/2016
Page 3
Chemistry 12
Unit 1 Provincial Practice
14. Consider the following PE diagram for a catalyzed and uncatalyzed reaction:
Which of the following describes the reverse reaction?
Reaction
Activation Energy (kJ)
A.
Catalyzed
300
B.
Uncatalyzed
300
C.
Catalyzed
400
D.
Uncatalyzed
400
H(kJ)
-100
-100
+100
+100
15. When a 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 the activation energy.
C. is part of the rate determining step.
D. lowers the activation energy barrier.
E. lowers the H of the reaction.
16. Consider the following reaction:
1/2 H2(g) + 1/2 I2(g) --> HI(g)
H = +28 kJ
The activation energy for the formation of HI is 167 kJ. The activation energy for the
decomposition of HI is .....
A. 28 kJ
B. 139 kJ
C. 153 kJ
D. 167 kJ
E. 195 kJ
Unit 1 Provincial Practice 2/17/2016
Page 4
Chemistry 12
Unit 1 Provincial Practice
17. Consider the following PE diagram:
Which of the following describes this reaction?
H
ACTIVATION
(kJ ) ENERGY (kJ)
REACTION
A.
-20
40
catalyzed
B.
-20
60
catalyzed
C.
-20
60
uncatalyzed
D. +20
40
uncatalyzed
E. +20
60
uncatalyzed
18.
A.
B.
C.
D.
E.
In general, a chemical reaction requiring a large activation energy will proceed ...
at a fast rate.
at a slow rate.
only at low temperatures.
only at low concentrations.
only in the presence of a catalyst.
19. Consider the following PE diagram:
5
Identify the activation energy for the forward uncatalysed reaction.
A. 1
B. 2
C. 3
D. 4
Unit 1 Provincial Practice 2/17/2016
E. 5
Page 5
Chemistry 12
Unit 1 Provincial Practice
20. Consider the following PE diagram:
5
Identify the activation energy for the forward catalysed reaction.
A. 1
B. 2
C. 3
D. 4
E. 5
21. Consider the following PE diagram:
5
Identify the activation energy for the reverse uncatalysed reaction.
A. 1
B. 2
C. 3
D. 4
E. 5
22. Consider the following PE diagram:
5
Identify the activation energy for the reverse catalysed reaction.
A. 1
B. 2
C. 3
D. 4



Unit 1 Provincial Practice 2/17/2016

E. 5
Page 6
Chemistry 12
Unit 1 Provincial Practice
23. Consider the following PE diagram:
5
Identify the H for the forward uncatalysed reaction.
A. 1
B. 2
C. 3
D. 4
E. 5
24. Consider the following PE diagram:
5
Identify the H for the forward catalysed reaction.
A. 1
B. 2
C. 3
D. 4
E. 5
25. Consider the following PE diagram:
5
Identify the H for the reverse catalysed reaction.
A. 1
B. 2
C. 3



Unit 1 Provincial Practice 2/17/2016
D. 4
E. 5

Page 7
Chemistry 12
Unit 1 Provincial Practice
26. Consider the following PE diagram:
5
Identify the H for the reverse uncatalysed reaction.
A. 1
B. 2
C. 3
D. 4
E. 5
27. Consider the following information for a reversible chemical reaction:
1
2
Forward activation energy = 20 kJ
Reverse activation energy = 30 kJ
Which of the following describes the reaction type and enthalpy change for the forward
reaction?
Reaction Type
Enthalpy Change 
A.
Exothermic
-10 kJ
B.
Exothermic
+10 kJ
C.
Endothermic
-10 kJ
D.
Endothermic
+10 kJ
28. Which of the following reactions is endothermic?
A. CH4(g) + 2O2(g) CO2(g) + 2H2O(l) + 890.3 kJ
B. 2N2O2(s) + 2H2O(l) -287.0 kJ 4NaOH(aq) + O2(g)
C. CaO(s) + H2O(l) Ca(OH)2(aq)
H = -65.2 kJ
D. CaO(s) + 3C(s) CaC2(s) + CO(g)
H = +464.8 kJ
29. Consider the following:
1/2 N2(g) + 1/2 O2(g)  NO(g) H = +90 kJ/mol NO
The correct equation including the heat term is
A. N2(g) + O2(g) + 90kJ --> 2NO(g)
B. N2(g) + O2(g) + 180kJ --> 2NO(g)
C. N2(g) + O2(g) --> 2NO(g) + 90kJ
Unit 1 Provincial Practice 2/17/2016
D. N2(g) + O2(g) --> 2NO(g) + 180kJ
Page 8
Chemistry 12
Unit 1 Provincial Practice
30. The following diagram shows reactant molecules approaching one another:
What is happening to the kinetic energy and the potential energy?
Kinetic Energy
Potential Energy
A.
Decreasing
Decreasing
B.
Decreasing
Increasing
C.
Increasing
Increasing
D.
Increasing
Decreasing
31. What happens to the PE and KE of the reactant particles as the activated complex is
formed?
Kinetic Energy
Potential Energy
A.
Increases
Decreases
B.
Increases
Increases
C.
Decreases
Decreases
D.
Decreases
Increases
32. Which of the following will decrease the fraction of effective collisions during a chemical
reaction?
A. Adding a catalyst.
B. Increasing the surface area.
C. Decreasing the temperature.
D. Decreasing reactant concentrations.
E. Decreasing surface area.
33. How do KE and PE change as reactant particles collide with each other?
KE
PE
A. increases;
increases
B. increases;
decreases
C. decreases;
increases
D. decreases;
decreases
Unit 1 Provincial Practice 2/17/2016
Page 9
Chemistry 12
Unit 1 Provincial Practice
34. Consider the following mechanism for a reaction:
Step 1 HBr + O2 --> HOOBr
Step 2
Step 3
HBr + HOOBr --> 2HOBr
2HBr + 2HOBr --> 2H2O + 2Br2
Which of the following statements is correct?
A. Br 2 is a reactant.
B. HBr is a product.
C. HOBr is a catalyst.
D. HOOBr is a reaction intermediate.
35. A proposed mechanism for a reaction is:
H3O+ + I- --> HI + H2O
Step 2 H2O2 + HI --> H2O + HOI
Step 1
Step 3 HOI + H3O+ --> I- + 2H2O + I2
Step 4 I2 + I- --> I3-
In the above mechanism, which of the following is true for the overall reaction?
A. HI is a catalyst
B. H O+ is a product
3
C. H2O2 is a reactant
D. H2O is an intermediate
36. A substance that is produced in one step in a reaction mechanism and consumed in a
subsequent step, without appearing in the overall reaction, is a(n)
A. catalyst.
B. product.
C. reactant.
D. intermediate.
37. Consider the following reaction mechanism:
Step1 2NO2 --> NO3 + NO
Step 2 NO3 + CO --> NO2 + CO2
Identify a product in the overall reaction.
A. CO
B. CO2
C. NO2
D. NO3
Unit 1 Provincial Practice 2/17/2016
Page 10
Chemistry 12
Unit 1 Provincial Practice
38. Consider the following reaction mechanism:
Step1 2NO2 --> NO3 + NO
Step 2 NO3 + CO --> NO2 + CO2
Identify a reactant in the overall reaction.
A. CO
B. CO2
C. NO
D. NO3
39. Consider the following reaction mechanism:
Step 1
NO(g) + O3(g) --> NO2(g) + O2(g)
Step 2
O(g) + NO2(g) --> NO(g) + O2(g)
The catalyst is ....
A. O
B. O2
C. O3
D. NO2
E. NO
D. NO2
E. NO
40. Consider the following reaction mechanism:
Step 1 NO(g) + O3(g) --> NO2(g) + O2(g)
Step 2 O(g) + NO2(g) --> NO(g) + O2(g)
A reaction intermediate is:
A. O
B. O2
C. O3
41. Consider the following reaction mechanism:
Step 1:
M + X --> MX
Step 2: MX + A --> D + X
The chemical species MX is a(n)
A. catalyst
B. inhibitor
C. final product
D. reaction intermediate
E. reactant
42. Consider the following reaction mechanism:
Step 1: ICl + H --> HI + HCl (slow)
Step 2: ICl + HI --> HCl + I2 (fast)
The species HCl is a.....
A. product
D. reaction intermediate
B. catalyst
E. activated complex.
Unit 1 Provincial Practice 2/17/2016
C. reactant
Page 11
Chemistry 12
43. Consider the following reaction mechanism:
Step 1: NO2 + NO2 --> NO + NO3
Step 2: NO3 + CO --> NO2 + CO2
Unit 1 Provincial Practice
The overall reaction is....
A. 2NO2--> NO3 + NO
B. NO2 + CO --> NO + CO2
C. NO3 + CO --> NO2 + CO2
D. NO2 + NO3 + CO --> NO3 + NO2 + NO + CO2
44. Consider the following potential energy diagram:
The above potential energy diagram represents an....
A. exothermic reaction involving one step.
B. exothermic reaction involving two steps.
C. endothermic reaction involving one step.
D. endothermic reaction involving two steps.
E. endothermic and exothermic reaction involving two steps.
45. Consider the following two-step reaction mechanism:
Step 1: NO2(g) + NO2(g) --> NO(g) + NO3(g) slow
Step 2: NO3(g) + CO(g) --> CO2(g) + NO2(g) fast
Which of the following changes would result in the greatest increase in reaction rate?
A. increase [CO]
B. decrease [NO2]
C. decrease [NO3]
D. increase [NO3]
E. increase [NO2]
Unit 1 Provincial Practice 2/17/2016
Page 12
Chemistry 12
Unit 1 Provincial Practice
46. A certain reaction is able to proceed by various mechanisms. Each mechanism has a
different Ea and results in a different overall rate. Which of the following best
describes the relationship between the Ea values and the rates?
A.
B.
C.
D.
47. Consider the following reaction mechanism:
Step 1 O3 --> O2 + O
Step 2
O3 + O --> 2O2
Which of the following could represent the activated complex for Step 2?
A. O
B. O2
C. O3
D. O4
48. A reaction has the following mechanism:
Step 1
2NO --> N2O2
Step 2
Step 3
N2O2 + H2 --> N2O + H2O
N2O + H2 --> N2 + H2O
Which of the following substances is a reactant?
A. N2O2
B. NO
C. H2O
D. N2O
49. Consider the reaction:
C5H12(g) + 8O2(g) --> 5CO2(g) + 6H2O(g)
Which of the following explains, in terms of collision theory, why this reaction occurs in more
than one step?
A. a low C5H5(g) concentration
B. low temperature of reactant mixture
C. low probability of a multi-particle collision
D. particles collide with insufficient kinetic energy
Unit 1 Provincial Practice 2/17/2016
Page 13
Chemistry 12
Unit 1 Provincial Practice
50. Consider the following potential energy diagram for a reversible reaction:
Which of the following descriptions is correct?
Reaction
Activation Energy(kJ)
A.
Reverse
10
B.
Reverse
10
C.
Forward
30
D.
Forward
20
H(kJ)
-20
-30
+10
+30
51. Consider the following PE diagram:
What is the minimum potential energy required to change reactants to the activated
complex?
A. 200 kJ
B. 300 kJ
C. 400 kJ
D. 500 kJ
Unit 1 Provincial Practice 2/17/2016
Page 14
Chemistry 12
Unit 1 Provincial Practice
52.
Select the true statement concerning the above potential energy diagram.
A. The catalyzed reaction has a larger H.
B. The uncatalyzed reaction has a larger H.
C. The catalyzed reaction has a greater rate of reaction.
D. The uncatalyzed reaction has a greater rate of reaction.
E. The catalyzed reaction has a higher reaction time.
53. As reactant molecules approach each other
A. heat is released.
B. a reaction intermediate forms.
C. kinetic energy changes to potential energy.
D. potential energy changes to kinetic energy.
54. The changes in PE and KE, as reactant molecules approach each other, can be
represented by
A.
B.
C.
Unit 1 Provincial Practice 2/17/2016
D.
Page 15
Chemistry 12
Unit 1 Provincial Practice
55. Which of the following best describes activation energy?
A. PE of activated complex
B. (PE of products ) - (PE of reactants)
C. (PE of reactants) - (PE of activated complex )
D. (PE of activated complex ) - (PE of reactants)
56. Consider the following reaction: O(g)+ O3(g) --> 2O2(g)
Which of the following describes how the reaction's catalyzed PE diagram compares to the
reaction's uncatalyzed PE diagram?
Ea
H
A. Ea(catalyzed) < Ea
unchanged
B. Ea(catalyzed) > Ea
C. Ea(catalyzed) < Ea
D.
Unchanged
unchanged
H(catalyzed) < 
H(catalyzed) < H
57. Which of the following is most likely to have the greatest reaction rate at room
temperature?
A. 2H2(g) + O2(g)  2H2O(l)
B. 2Ag+
+ CrO42-(aq) Ag2CrO4(s)
(aq)
C. Pb(s) + 2HCl(aq)  PbCl2 + H2
D. CH4(g) + 2O2(g) CO2(g) + 2H2O(g)
58. Consider the following reaction involving 1.0 g of powdered zinc:
Zn(s) + 2HCl(aq) --> H2(g) + ZnCl2(a
Trial
1
2
3
Temperature (oC)
60
30
30
Concentration of HCl
6.0
6.0
3.0
The rates, in order of fastest to slowest, are
A. 1, 2, 3
B. 2, 1, 3
C. 3, 1, 2
D. 3, 2, 1
Unit 1 Provincial Practice 2/17/2016
Page 16
Chemistry 12
Unit 1 Provincial Practice
59. Increasing the temperature of a reaction increases the reaction rate by
I. increasing frequency of collisions
II. increasing the kinetic energy of collision
III. decreasing the potential energy of collision
A. I only.
B. I and II only.
C. II and III only.
D. I, II and III.
60. Consider the graph for the following reaction: The average rate of reaction is slowest in
the time interval
A.
B.
C.
D.
0000-
1 minute.
2 minutes.
3 minutes.
4 minutes.

61. Consider the following reaction:
N2(g) + 3H2(g) --> 2NH3(g)
If the rate of formation of NH3 is 4.0 x 10-4 mol/s, then the rate of consumption of H2 is
A. 2.0 x 10-4 mol/s
B. 2.0 x 10-4 mol/s
C. 6.0 x 10-4 mol/s
D. 1.2 x 10-3 mol/s
62. Which of the following units could be used to express reaction rate?
A. mL / s
B. mL / g
C. g / mL
D. mL / mol
Unit 1 Provincial Practice 2/17/2016
Page 17
Chemistry 12
Unit 1 Provincial Practice
63. Which of the following reactions occurs most rapidly at standard conditions?
A. 2Sn(s) + O2(g) 2SnO(s)
B. CaO(s) + 3C(s) CaC2(s) + CO(g)
C. SnO2(s) + 2CO(g) Sn(s) + 2CO2(g)

D. 2AgNO3(aq) + K2CrO4(aq) Ag2CrO4(s) + 2KNO3(aq)
64. Consider the following reaction:
CaO(s) + 2HCl(aq) --> CaCl2(aq) + H2O(l)
Which of the following could be used to measure the rate of this reaction?
I. change in pH
II. change in volume
III. change in pressure
IV. change in total mass
A.
B.
C.
D.
I only
I and II only
I, III and IV only
II, III and IV only
65. Consider the following reaction:
COCl2(g) --> CO(g) + Cl2(g)
Which of the following could be used to determine reaction rate in a closed system?
A. a decrease in gas pressure
B. an increase in gas pressure
C. a decrease in the mass of the system
D. an increase in the mass of the system
66. Which factor explains why potassium generally reacts faster than sodium?
A. surface area
B. temperature
C. concentration
D. nature of reactants
67. Which of the following has the lowest rate of reaction?
A. Pb(s) + CuCl(aq)  Cu(s) + PbCl2(aq)
B. HCl(aq) + NaOH(aq)  H2O(l) + NaCl(aq)
C. H2SO4(aq) + BaSO4(aq)  2H2O(l) + BaSO4(s)
D. Pb(NO3)2(aq) + 2NaI(aq)  PbI2(s) + 2NaNO3(aq)
Unit 1 Provincial Practice 2/17/2016
Page 18
Chemistry 12
Unit 1 Provincial Practice
68. Consider the following reaction:
Zn(s) + 2HC1(aq) --> ZnC12(aq) + H2(g)
Solid zinc was added to 1.0 M HC1. In 20.0 s, the temperature of the container increased
by 0.5°C and 25.00 mL of H2 was produced. The rate of this reaction was
A. 0.5°C/s
B. 1. 0 M HC1/s
C. 1. 25 mL H2/s
D. 0. 050 mol HC1/s
69. Consider the reaction:
Ca(s) + 2H2O(l) --> Ca(OH)2(aq ) + H2(g)
At a certain temperature, 2.50 g Ca reacts completely in 30.0 seconds. The rate of
consumption of Ca is ....
A. 0.00208 mol/min
B. 0.0833 mol/min
C. 0.125 mol/min
D. 0.0417 mol/min
E. 5.00 mol/min
70. Consider the following reaction:
2 NO2(g) --> 2 NO(g) + O2(g)
Under certain conditions, the rate of decomposition of NO2 is 3.2 x 10–3 mol/s. The rate of
formation of O2 is .....
A. 1.6 x 10–3 mol/s
B. 3.2 x 10–3 mol/s
C. 4.8 x 10–3 mol/s
D. 6.4 x 10–3 mol/s
E. 9.6 x 10–3 mol/s
71. Consider the following reaction:
CH4(g) + 2O2(g) --> CO2(g) + 2H2O(g)
At a certain temperature, 1.0 mol CH4 is consumed in 4.0 minutes.
The rate of production of H2O is ...
A.
B.
C.
D.
0.25 mol/min
0.50 mol/min
2.0 mol/min
4.0 mol/min
Unit 1 Provincial Practice 2/17/2016
Page 19
Chemistry 12
Unit 1 Provincial Practice
72. The rate of a chemical reaction is equal to the slope of a graph with the axes labelled
x-axis
y-axis
A.
time
rate
B.
mass
time
C. volume of gas
time
D.
time
concentration
E.
rate
time
73. The addition of a catalyst to a reaction provides an alternate mechanism with....
A. higher activation energy and lower reaction rate.
B. higher activation energy and higher reaction rate.
C. lower activation energy and lower reaction rate.
D. lower activation energy and higher reaction time.
E. lower activation energy and higher reaction rate.
74. When a catalyst is added to a reaction, H will...
A. increase slowly
B. remain constant
C. decrease slowly
D. increase rapidly due to the alternate
pathway,
E. decrease rapidly due to the alternate
pathway.
75. 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 number of molecules present in the container.
D. the introduction of an alternate pathway with greater activation energy.
E. a decrease in the fraction of particles possessing sufficient energy.
76. The slowest of the following reactions is ....
A. Ag+
B. H O+
+ Cl–(aq)  AgCl(s)
+ OH–(aq)  2H2O(l)
(aq)
3 (aq)
C. 3Ba2+
D. Cu + 2Ag+
+ 2PO 3–
 Ba (PO ) 
 Cu2+
+ 2Ag
(aq)
4
(aq)
3
E. Pb2+
+ 2Cl–(aq)  PbCl2(s)
(aq)
4 2(s)
(s)
(aq)
(aq)
(s)

77. Which combination of factors will affect the rate of the following reaction?
Zn(s) + 2 HCl(aq) --> ZnCl2(aq) + H2(g)
A.
B.
C.
D.
E.
temperature and surface area only
temperature and concentration only
concentration and surface area only
temperature, concentration and surface area
concentration only
Unit 1 Provincial Practice 2/17/2016
Page 20
Chemistry 12
Unit 1 Provincial Practice
78. In general, reaction rates double when the temperature is increased by 10°C. The
temperature of a reaction is increased by 30°C. The rate of the reaction will increase by
a factor of...
A. 2
B. 4
C. 6
D. 8
E. 16
79. Consider the following reaction at constant temperature in an open system:
MgCO3(s) + 2 HCl(aq) --> CO2(g) + H2O(l) + MgCl2(aq)
Which of the following properties could be used to determine the reaction rate?
A. mass of the system
B. pressure of the gas
C. concentration of H2O
D. concentration of MgCO3
80. Consider the following reaction:
NaOH(aq) + HCl(aq) --> H2O(l) + NaCl(aq)
The rate of this reaction could be determined by monitoring the change in concentration of
A. H+
B. Cl–
C. Na+
D. H2O
81. Consider the following reaction:
Zn(s) + 2 HCl(aq) --> H2(g) + ZnCl2(aq)
Data collected for the above reaction are summarized in the table below:
The rate of this reaction can be measured in units of......
A. g/min
B. g/mL
C. min/mL
D. g/ml°C
Unit 1 Provincial Practice 2/17/2016
E. º C/g
Page 21
Chemistry 12
Unit 1 Provincial Practice
82. Consider the reaction:
2C20H42(s) +
61O2(g)
 40CO2(g)
+
42H2O(g)
If the rate of production of H2O is 0.98 g/min, what is the rate of oxygen consumption? 
A. 1.42 g/min
B. 2.5 g/s
C. 0.079 g/min
D. 150 g/s
E. 0.042 g/s
83. Which of the following reactions is most likely to proceed at the greatest rate under
standard conditions?
A. Zn(s) + S(s)  ZnS(s)
B. H2(g) + I2(g)  2HI(g)
C. Cu(s) + Cl2(g)  CuCl2(s)
D. 2KOH(aq) + H2SO4(aq)  2H2O(l) + K2SO4(aq)
84. Given the following graph:
Curve 1
Curve 2
Which one of the following statements are true?
A. Curve 1 is at a higher temperature than curve 2 and a lower fraction of the colliding particles
possess sufficient kinetic energy for a successful collision.
B. Curve 2 is at a higher temperature than curve 1 and a lower fraction of the colliding particles
possess sufficient kinetic energy for a successful collision.
C. Curve 1 is at a higher temperature than curve 2 and a higher fraction of the colliding particles
possess sufficient kinetic energy for a successful collision.
D. Curve 2 is at a higher temperature than curve 1 and a higher fraction of the colliding particles
possess sufficient kinetic energy for a successful collision.
Unit 1 Provincial Practice 2/17/2016
Page 22
Chemistry 12
Unit 1 Provincial Practice
Answers to Multiple Choice
1D
2C
3C
4D
5B
6D
7B
8D
9D
10 C
11 D
12 D
13 A
14 D
15 B
16 B
17 E
18 B
19 B
20 A
21 C
22 D
23 E
24 E
25 E
26 E
27 A
28 D
29 B
30 B
31 D
32 C
33 C
34 D
35 C
36 D
Unit 1 Provincial Practice 2/17/2016
37 B
38 A
39 E
40 D
41 D
42 A
43 B
44 B
45 E
46 C
47 D
48 B
49 C
50 A
51 B
52 C
53 C
54 A
55 D
56 A
57 B
58 A
59 B
60 D
61 C
62 A
63 D
64 A
65 B
66 D
67 A
68 C
69 C
70 A
71 B
72 D
73 E
74 B
75 E
76 D
77 D
78 D
79 A
80 A
81 A
82 E
83 D
84 D
Page 23