study questions
Modified True/False
Indicate whether the sentence or statement is true or false. If false, change the identified word or phrase to make the
sentence or statement true.
____
1. Thermochemistry is the study of energy changes that accompany transformations in solids.
____________________
____
2. Energy transformations are the basis for all the activities that make up our lives. ____________________
____
3. Thermal energy is a form of potential energy that can be released to the surroundings.
____________________
____
4. Chemical systems contain both kinetic and potential forms of energy. ____________________
____
5. The energy of protons and neutrons in the atomic nuclei is a form of potential energy in a chemical system.
____________________
____
6. A negative enthalpy change is a measure of the amount of energy absorbed from the surroundings.
____________________
____
7. Temperature, theoretically, is a measure of the maximum kinetic energy of the molecules in a substance.
____________________
____
8. Inside a calorimeter, the amount of energy gained by the surroundings (the water) must equal the amount of
energy released by the reaction in the calorimeter. _____________________
____
9. The molar heat of reaction refers to the amount of heat needed to increase the temperature of one mole of a
substance by one degree Celsius. ____________________
____ 10. A chemical equation that represents a change in matter and includes the molar enthalpy is termed a
thermochemical equation. ____________________
____ 11. The enthalpy change per mole of a substance undergoing a change is called the molar enthalpy.
____________________
____ 12. Enthalpy changes for an exothermic reaction are given a negative sign. ____________________
____ 13. Enthalpy changes for an endothermic reaction are given a negative sign. ____________________
____ 14. The amount of energy involved in a change depends on the quantity of matter undergoing the change.
____________________
____ 15. If a chemical equation is reversed, according to Hess's Law, no change occurs to the H of the reaction.
____________________
____ 16. According to Hess's Law, if the coefficients of a chemical equation are altered by multiplying or dividing by a
constant factor, then the H is altered the same way. ____________________
____ 17. The following diagram represents an exothermic reaction. ____________________
____ 18. The reactants in a heat of formation reaction can be elements or compounds as long as they are in their
standard form. _________________________
____ 19. The major energy sources that we use in Ontario are all infinite. ____________________
____ 20. Uranium is a very concentrated energy source. ____________________
____ 21. CANDU reactors use natural uranium containing 50% uranium-235 and 50% uranium-238.
______________________________
____ 22. To date there have been no major nuclear accidents in Canada. ____________________
____ 23. Nuclear fusion occurs naturally in the sun. ____________________
____ 24. Uranium would be an ideal reactant for a nuclear fusion reaction. ____________________
____ 25. Chemical kinetics is the study of ways to make chemical reactions produce or consume energy.
_________________________
____ 26. The rate of the reaction can be obtained by measuring the rate at which a product is formed.
_________________________
____ 27. It is possible to use the units of seconds/mL to express rate. _________________________
____ 28. Many different properties can be used or measured to determine the rate of the reaction.
_________________________
____ 29. The average rate of reaction is the speed at which the reaction is proceeding at any given moment.
______________________________
____ 30. The average rate of reaction can be determined by measuring the slope of a secant drawn on a graph of the
reaction progress. _________________________
____ 31. The instantaneous rate of reaction is measured by taking the slope of the secant drawn at that point on the
graph of the reaction. _________________________
____ 32. Evidence shows that, for most reactions, the concentration changes are more rapid at the beginning of the
reaction. _________________________
____ 33. The rate of the reaction usually increases with time. _________________________
____ 34. The concentration of a product during the progress of a reaction, increases continuously, most rapidly at the
beginning of the reaction. _________________________
____ 35. The rate of production of a colour in a solution can be measured by its conductivity.
_________________________
____ 36. The physical nature of the reactants affects the rate of the reaction. _________________________
____ 37. The concentration of the reactants affects the rate of the reactant. _________________________
____ 38. For most reactions, increasing the temperature of a reaction decreases the rate of the reaction.
___________________________________
____ 39. Catalysts can be used to speed up a reaction. _________________________
____ 40. Some reactions only proceed in the presence of a catalyst. _________________________
____ 41. The reaction,
finely powdered. _________________________
would probably proceed at a slower rate if the zinc was
____ 42. According to the rate law: The rate will always be proportional to the product of the final concentrations of
the reactants, where these concentrations are raised to some exponential powers.
______________________________
____ 43. The value of the rate constant, k, is valid only for a specific reaction at a specific temperature.
_________________________
____ 44. The overall order of reaction is the product of the individual orders of reaction for each reaction.
_________________________
____ 45. The order of the reaction for any given reactant is always the coefficient in the balanced chemical reaction.
_________________________
____ 46. Rate law equations must be determined empirically. _________________________
____ 47. The following diagram represents a first order reaction. ______________________________
____ 48. The following diagram represents a first order reaction. ______________________________
____ 49. Half-life is the time required for one half of the sample to react. _________________________
____ 50. An ineffective collision is one that has sufficient energy and correct orientation so that the reaction can
proceed. _________________________
____ 51. The activation energy is the maximum amount of energy with which particles must collide to result in an
effective collision. _________________________
____ 52. The activated complex in an unstable chemical species containing partially broken and partially formed
bonds. ______________________________
____ 53. The activated complex represents the minimum potential energy in the reaction process.
___________________________________
____ 54. The first step in a reaction mechanism is known as the rate-determining step. _________________________
____ 55. A catalyst can be used as part of a reaction mechanism, perhaps involved in forming a reaction intermediate.
_________________________
Completion
Complete each sentence or statement.
56. In ____________________ changes, energy is released from a system to the surroundings.
57. In ____________________ changes, energy is absorbed by a system.
58. The amount of energy transferred between substances is known as ____________________.
59. ____________________ is a measure of the average kinetic energy of the particles in a sample of matter.
60. A system in which both matter and energy can move in or out is called a(n) ____________________ system.
61. An ideal system in which neither matter nor energy can move in or out is a(n) ____________________
system.
62. A system in which energy and not matter can move in or out is a(n) ____________________ system.
63. A _________________________ is a device in which a fuel is burned inside an insulated container to obtain
accurate measurements of heat transfers during chemical reactions.
64. Chemical systems have both ____________________ and ____________________ forms of energy.
65. The enthalpy change per mole of a substance undergoing a change is called the ____________________.
66. A ____________________ change typically has enthalpy changes in the range
67. A enthalpy change in the
.
kJ/mol probably was a ____________________ change.
68. A ____________________ change has a typical enthalpy change in the
kJ/mol
69. The magnitude of the energy change from a nuclear change is the result of ____________________ equation.
70. Enthalpy changes for exothermic reactions are given a ____________________ sign.
71. An enthalpy change for an endothermic reaction are given a ____________________ sign.
72. This statement, "The total energy change of the chemical system is equal to the total energy change of the
surroundings" is based on the ________________________________________.
73. A chemical equation that includes the energy term involved in the reaction is called a
____________________ equation.
74. A _________________________ diagram is a graphical representation of the energy transferred during a
physical or chemical change.
75. ____________________ states: The value of the
for any reaction that can be written in steps equals the
sum of the values of
for each of the individual steps.
76. A ____________________ reaction is a reaction in which compounds are formed from their elements.
77. The standard enthalpy of formation of an element already in its standard state is ____________________.
78. The most widely used nuclear reaction is the ____________________ of uranium into two smaller nuclei.
79. The potential energy of the products is ____________________ than the potential energy of the reactants in
an exothermic reaction.
80. _________________________ is the study of ways to make chemical reactions go faster or slower.
81. A _________________________ is obtained by measuring the rate of product formation or the rate at which
a reactant is consumed.
82. The rate of reaction over a period of time is the _________________________.
83. The rate at any particular point in time is known as the _______________________________.
84. The concentration of a product during the progress of a reaction increases ____________________.
85. The rate of consumption of a reactant is fastest at the ____________________ of the reaction
86. The rate of a reaction that produces ions can be measured by measuring the change in its
____________________.
87. The rate of the reaction of sodium, silver and gold with gases in the air is different due to
___________________________________.
88. Chlorophyll, in the reaction of photosynthesis, plays the role of a ______________________.
89. A rate at which a solid reactant is consumed can be increased by increasing the ________________________
of the solid
90. An automobile's _________________________ increases the rate of oxidation of exhaust gases.
91. An enzyme, a protein in living cells, acts like a _________________________ to control the rate of a specific
biochemical reaction.
92. The rate, r, will always be _________________________ the product of the initial concentrations of the
reactants raised to some exponential value.
93. In a Rate Law Equation,
, k is known as a _________________________.
94. The value of the rate constant is specific to a reaction at a specific _________________________.
95. The _____________________________ is the sum of the exponents in the rate law equation.
96. The following diagram represents a _____________________________.
97. The _________________________ of a reactant is the time required for half of the sample to react.
98. Nuclear decay, the change that occurs as a radioactive isotope breaks down into smaller isotopes, is a
_________________________.
99. Rates of reaction, theoretically, can be explained with _________________________.
100. The value of the rate constant can be calculated by the ________________________.
101. If finely divided platinum is used as a catalyst to speed the process of the reaction between hydrogen gas and
oxygen gas in a fuel cell. The platinum is call a ___________________ catalyst.
102. A catalyst can be involved in the reaction mechanism, combining to form a reaction intermediate as long as it
is ____________________ unchanged in the final step of the mechanism.
Essay
103. Outline some of the arguments both for and against the use of nuclear power.
104. "In the 1950s, people had high expectations of endless, inexpensive nuclear energy". Discuss this statement in
terms of what changes have occurred that this has yet to come to fruition.
study questions
Answer Section
MODIFIED TRUE/FALSE
1. ANS:
LOC:
2. ANS:
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21. ANS:
REF:
F, matter
ECV.01
T
ECV.01
F, kinetic
ECV.01
T
EC2.02
T
EC2.01
F, released to
EC2.02
F, average
EC2.01
T
EC2.02
F, molar heat capacity
EC2.01
T
EC2.02
T
EC2.02
T
EC2.02
F, positive sign
EC2.02
T
EC2.02
F, sign is reversed
EC1.02
T
EC1.02
F, endothermic
EC1.05
F, elements only
EC2.05
F, finite
EC3.01
T
EC3.01
F, 0.7% U-235 and 99.3% U-238
REF: K/U
OBJ: 5.1
REF: K/U
OBJ: 5.1
REF: K/U
OBJ: 5.1
REF: K/U
OBJ: 5.1
REF: K/U
OBJ: 5.1
REF: K/U
OBJ: 5.1
REF: K/U
OBJ: 5.1
REF: K/U
OBJ: 5.1
REF: K/U
OBJ: 5.1
REF: K/U
OBJ: 5.2
REF: K/U
OBJ: 5.2
REF: K/U
OBJ: 5.2
REF: K/U
OBJ: 5.2
REF: K/U
OBJ: 5.2
REF: K/U
OBJ: 5.4
REF: K/U
OBJ: 5.4
REF: K/U
OBJ: 5.3
REF: K/U
OBJ: 5.5
REF: K/U
OBJ: 5.6
REF: K/U
OBJ: 5.6
K/U
LOC: EC3.01
OBJ: 5.6
22. ANS:
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45. ANS:
LOC:
T
EC3.01
T
EC3.01
F, hydrogen
EC3.01
F, go faster or slower
EC2.01
T
EC2.01
F, mL/second
EC2.01
T
EC1.04
F, instantaneous rate of reaction
EC1.03
T
EC1.03
F, tangent
EC1.03
T
EC1.03
F, decreases
EC1.03
T
EC1.03
F, light absorbency
EC2.06
F, chemical
EC1.04
T
EC1.04
F, decreasing the temperature
EC1.04
T
EC1.04
T
EC1.04
F, faster rate
EC1.04
F, initial concentrations
EC1.03
T
EC1.03
F, sum
EC1.03
F, sometimes
EC1.03
REF: K/U
OBJ: 5.6
REF: K/U
OBJ: 5.6
REF: K/U
OBJ: 5.6
REF: K/U
OBJ: 6.1
REF: K/U
OBJ: 6.1
REF: K/U
OBJ: 6.1
REF: K/U
OBJ: 6.1
REF: K/U
OBJ: 6.1
REF: K/U
OBJ: 6.1
REF: K/U
OBJ: 6.1
REF: K/U
OBJ: 6.1
REF: K/U
OBJ: 6.1
REF: K/U
OBJ: 6.1
REF: K/U
OBJ: 6.1
REF: K/U
OBJ: 6.2
REF: K/U
OBJ: 6.2
REF: K/U
OBJ: 6.2
REF: K/U
OBJ: 6.2
REF: K/U
OBJ: 6.2
REF: K/U
OBJ: 6.2
REF: K/U
OBJ: 6.3
REF: K/U
OBJ: 6.3
REF: K/U
OBJ: 6.3
REF: K/U
OBJ: 6.3
46. ANS: T
LOC: EC1.03
47. ANS: F, greater than first order reaction
REF: K/U
OBJ: 6.3
REF:
48. ANS:
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51. ANS:
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53. ANS:
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55. ANS:
LOC:
K/U
OBJ: 6.3
F, second order reaction
EC1.03
T
EC1.03
F, effective collision
EC1.04,EC1.05
F, minimum
EC1.04,EC1.05
T
EC1.04,EC1.05
F, maximum potential energy
EC1.04,EC1.05
F, slowest step
EC1.06
T
EC1.04
LOC: EC1.03
REF: K/U
OBJ: 6.3
REF: K/U
OBJ: 6.3
REF: K/U
OBJ: 6.4
REF: K/U
OBJ: 6.3
REF: K/U
OBJ: 6.4
REF: K/U
OBJ: 6.4
REF: K/U
OBJ: 6.4
REF: K/U
OBJ: 6.5
exothermic
ECV.01
endothermic
ECV.01
heat
EC2.01
Temperature
EC2.01
open
EC2.01
isolated
EC2.01
closed
EC2.01
bomb calorimeter
ECV.02
kinetic, potential
EC2.01
molar enthalpy
EC2.02
physical
EC1.01
chemical
EC1.01
REF: K/U
OBJ: 5.1
REF: K/U
OBJ: 5.1
REF: C
OBJ: 5.1
REF: C
OBJ: 5.1
REF: C
OBJ: 5.1
REF: C
OBJ: 5.1
REF: C
OBJ: 5.1
REF: K/U
OBJ: 5.1
REF: K/U
OBJ: 5.1
REF: K/U
OBJ: 5.2
REF: K/U
OBJ: 5.1
REF: K/U
OBJ: 5.1
COMPLETION
56. ANS:
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57. ANS:
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73. ANS:
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76. ANS:
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77. ANS:
zero
0
78.
79.
80.
81.
82.
83.
84.
85.
86.
87.
REF:
ANS:
LOC:
ANS:
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REF:
88. ANS:
LOC:
89. ANS:
LOC:
90. ANS:
nuclear
EC1.01
Einstein's
EC1.01
negative
EC2.02
positive
EC2.02
Law of Conservation of Energy
EC2.03
thermochemical
EC2.02
potential energy
EC1.05
Hess's Law
EC1.02
formation
EC2.05
REF: K/U
OBJ: 5.1
REF: K/U
OBJ: 5.1
REF: K/U
OBJ: 5.2
REF: K/U
OBJ: 5.1
REF: K/U
OBJ: 5.2
REF: K/U
OBJ: 5.3
REF: K/U
OBJ: 5.3
REF: K/U
OBJ: 5.4
REF: K/U
OBJ: 5.5
K/U
OBJ: 5.5
fission
EC3.01
lower
EC1.05
Chemical kinetics
EC2.01
rate of reaction
REF:
EC1.03
average rate of reaction
EC1.03
instantaneous rate of reaction
EC1.03
continuously
EC1.03
beginning
EC1.03
conductivity
EC1.03
the chemical nature of the reactants
LOC: EC2.05
REF: K/U
OBJ: 5.6
REF: K/U
OBJ: 5.3
REF: K/U
OBJ: 6.1
K/U
6.1
K/U
OBJ: 6.2
catalyst
EC1.04
surface area
EC1.04
catalytic converter
OBJ:
REF: K/U
OBJ: 6.1
REF: K/U
OBJ: 6.1
REF: K/U
OBJ: 6.1
REF: K/U
OBJ: 6.1
REF: K/U
OBJ: 6.1
LOC: EC1.04
REF: K/U
OBJ: 6.2
REF: K/U
OBJ: 6.2
REF: K/U
OBJ: 6.2
LOC: EC1.04
91. ANS: catalyst
LOC: EC1.04
92. ANS: proportional
LOC: EC1.03
93. ANS: rate constant
LOC: EC1.03
94. ANS: temperature
LOC: EC1.03
95. ANS:
(overall) order of reaction
overall
order of reaction
REF:
96. ANS:
LOC:
97. ANS:
LOC:
98. ANS:
LOC:
99. ANS:
LOC:
100. ANS:
LOC:
101. ANS:
LOC:
102. ANS:
LOC:
K/U
OBJ: 6.3
zeroth-order reaction
EC1.03
half-life
EC1.03
first-order reaction
EC1.03
collision theory
EC1.04
Arrhenius equation
EC2.06
heterogeneous
EC1.04
regenerated
EC1.04
REF: K/U
OBJ: 6.2
REF: K/U
OBJ: 6.3
REF: K/U
OBJ: 6.3
REF: K/U
OBJ: 6.3
LOC: EC1.03
REF: K/U
OBJ: 6.3
REF: K/U
OBJ: 6.3
REF: K/U
OBJ: 6.3
REF: K/U
OBJ: 6.4
REF: K/U
OBJ: 6.5
REF: K/U
OBJ: 6.5
REF: K/U
OBJ: 6.5
ESSAY
103. ANS:
Advocates:
- has low uranium fuel costs, including transportation
- causes very little air pollution, such as green house and acid gases
- reduces our dependence on fossil fuels for electricity generation, allowing those materials to be used for
other purposes.
Opponents:
- the possible release of radioactive materials in a reactor malfunction
- the difficulty of disposing of the highly toxic radioactive wastes
- the large capital costs of building nuclear reactors and then decommissioning them at the end of their
relatively short lifetime
- unknown health effects of long-term low level exposure to radiation
- thermal pollution from cooling water
REF: I
OBJ: 5.6
LOC: EC3.01
104. ANS:
Students answers should include some of the following points:
Arguments from the opponents of nuclear waste including:
- possible reactor malfunction
- disposal of radioactive waste
- large capital costs of building reactors
- unknown long-term effects
Also, some accidents in the recent past, have also slowed the more recent development of nuclear power
stations including:
- the near-accident at Three Mile Island in 1979
- the nuclear explosion at Chernobyl in Ukraine in 1986
Moreover, the development of nuclear fusion has yet to be advanced to be a useable source.
REF:
I
OBJ: 5.6
LOC: EC3.01