UNIT 5: Electrochemistry
____ 93. In the reaction
+
+
+
+
Which of the following statements is correct?
a.
is the reducing agent, and
is the oxidizing agent
b.
is the reducing agent, and
is the oxidizing agent
c.
is the reducing agent, and
is the oxidizing agent
d.
is the reducing agent, and
is the oxidizing agent
e.
is the reducing agent, and
is the oxidizing agent
____ 94. The oxidation number of chromium (
) in the dichromate ion (
a. +2
d. +7
b. +4
e.
c. +6
____ 95. Manganese (Mn) has an oxidation number of +6 in
a.
d.
b.
) is
e.
c.
____ 96. The oxidation number of sulfur ( ) in
is
a. +6
d. +2
b. +4
e. 0
c. +3
____ 97. In which of the following compounds does manganese (Mn) have an oxidation number of +4?
a.
d.
b.
e.
c.
____ 98. In which of the following compounds does nitrogen have the highest oxidation number?
a.
d.
b.
e.
c.
____ 99. The oxidation number of
in
is
a. +1
b. +2
c. +3
____ 100. The oxidation number of fluorine ( ) in
a.
3
b.
2
c.
1
____ 101. The oxidation number of oxygen in ozone,
a. +3
d. +4
e. 0
is
d. 0
e. +1
, is
d.
2
b.
3
c. +2
e. 0
____ 102. The oxidation number of nitrogen , , in the nitrite ion,
, is
a. +1
d.
3
b. +2
e.
1
c. +3
____ 103. In
the oxidation numbers of
and respectively are
a. +2, +3, 4
d. +2, +4, 2
b. +3, +6, 2
e. +4, +5, 3
c. +2, +4, 8
____ 104. Sulfur ( ) has an oxidation number of +7 in
a.
d.
b.
e.
c.
____ 105. In the reaction
+
+
+
+
Which of the following statements is correct?
a.
hydrogen is oxidized and
is the oxidizing agent
b.
hydrogen is oxidized and
is the oxidizing agent
c.
carbon is oxidized and
is the oxidizing agent
d.
manganese is oxidized and
is the oxidizing agent
e.
carbon is oxidized and
is the oxidizing agent
____ 106. Which substance in the following reaction has undergone oxidation?
+
+
+
a.
d.
b.
e.
+
c.
____ 107. Given the following unbalanced redox equation:
+
+
+
+
the coefficient of
in the balanced equation with lowest whole-number coefficients is
a. 2
d. 5
b. 3
e. 6
c. 4
____ 108. This question consists of an assertion (statement) in the left-hand column and a reason in the right-hand
column.
Reason
Assertion
Chlorine is a stronger oxidizing agent
than iodine.
Chlorine will cause iodine to form
when chlorine is bubbled through a
solution of potassium iodide.
Select one of the following.
a. if both assertion and reason are true statements, and the reason is a correct explanation of
the assertion
b. if both assertion and reason are true statements, and the reason is not a correct explanation
of the assertion
c. if the assertion is true but the reason is false
d. if the assertion is false but the reason is a true statement
e. if both assertion and reason are false statements
____ 109. Which of the following statements are true for the redox reaction:
+
+
I. the oxidation number of
II.
+
+
changes from +7 to +3
is the oxidizing agent
III.
is oxidized to
IV.
is the reducing agent
V. the oxidation number of
changes from +1 to 0
a. II and IV
d. IV and V
b. I and III
e. III and V
c. II and III
____ 110. Which of the following equations does not represent an oxidation-reduction reaction?
a.
+
+
b.
+
c.
+
d.
+
e.
+
+
+
____ 111. Which of the following reactions are oxidation-reduction reactions?
I.
+
+
II.
III.
+
+
+
+
IV.
+
V.
+
+
a. II and III
d. II, IV and V
b. I and V
e. I and III
c. IV and V
____ 112. Consider the following unbalanced redox reaction:
+
+
+
+
The coefficients in the balanced equation are, from left to right
a. 1, 1, 6, 1, 1, 3
d. 1, 6, 6, 1, 6, 3
b. 1, 2, 6, 1, 2, 3
e. 2, 1, 12, 2, 1, 6
c. 2, 3, 12, 2, 3, 6
____ 113. Experiments were performed with four strips of metals , , , and , and their corresponding nitrate
solutions
,
,
, and
. The following observations were obtained:
A
no reaction
no reaction
no reaction
no reaction
precipitate
no reaction
precipitate
precipitate
precipitate
no reaction
no reaction
no reaction
precipitate
no reaction
precipitate
no reaction
Which of the following is the correct list of the metal ions in order of decreasing strength as oxidizing
agents (strongest oxidizing agent first)?
a.
d.
b.
e.
c.
____ 114. Experiments were performed with four strips of metals A, B, C, and D, and their corresponding nitrate
solutions
,
,
, and
. Metal was placed in each of the
solutions and reactions were observed only in solutions containing
and
ions. Metal B did not
react in any of the solutions. Metal C reacted in the solution containing
ions, but was not tested in
the other solutions. A list of the metals in order of decreasing strength as reducing agents (strongest
reducing agent is listed first) is
a. B A D C
d. D A C B
b. C B D A
e. B C A D
c. C D A B
____ 115. Consider the following reaction:
Which of the following is the oxidizing agent?
a. Cu
d.
b. N in HNO3
e.
in
in
+
c. H in HCl
____ 116. Consider the following redox reaction:
Which of the following is the reducing agent?
a.
d.
in
b.
c.
in
in
e.
____ 117. Which element is oxidized in the following reaction?
in
in
a.
in
d.
in
b.
e.
in
c.
in
____ 118. Consider the following oxidation-reduction reaction:
Which of the following statements about this oxidation-reduction process is true?
a. iodine is oxidized and potassium is reduced
b. iodine is reduced and potassium is oxidized
c. potassium is oxidized and chlorine is reduced
d. chlorine is oxidized and hydrogen is reduced
e. iodine is both oxidized and reduced
____ 119. Which element is reduced in the following oxidation-reduction reaction?
a.
in
b.
in
c.
in
d.
in
e.
in
____ 120. Consider the following unbalanced reaction:
When the equation is balanced with the smallest whole-number coefficients, the coefficient of
be
a. 1
d. 4
b. 2
e. 5
c. 3
____ 121. Given the following unbalanced oxidation-reduction equation:
In the balanced equation, the coefficient of
is
a. 2
d. 5
b. 3
e. 6
c. 4
____ 122. Given the following unbalanced redox reaction:
The coefficient of aluminum,
, in the balanced equation is
a. 1
d. 4
b. 2
e. 6
c. 3
____ 123. Which of the following half-reaction equations are balanced?
I.
II.
III.
IV.
will
V.
a. I and II
d. III and V
b. II and IV
e. all are balanced
c. I and III
____ 124. Which one of the following half-reactions is completely balanced?
a.
b.
c.
d.
e.
____ 125. Consider the following oxidation-reduction reaction:
Which of the following statements are true?
I.
in
is reduced
II.
in
is oxidized
III.
in
is oxidized
IV.
in
is reduced
V.
is the reducing agent
a. I and III
b. II and V
c. I and II
____ 126. Consider the following equation:
d. II and IV
e. III and IV
In this reaction
a. carbon ( ) is reduced and manganese (
) is oxidized
b. carbon ( ) is reduced and hydrogen ( ) is oxidized
c. manganese (
) is reduced and hydrogen ( ) is oxidized
d. manganese (
) is reduced and carbon ( ) is oxidized
e. hydrogen ( ) is reduced and carbon ( ) is oxidized
____ 127. Consider the following reaction:
In this reaction, the reducing agent is
a.
d.
b.
e.
c.
____ 128. Consider the redox reaction
Which of the following is oxidized?
a.
d.
in
b.
c.
in
e.
in
in
____ 129. This question consists of an assertion (statement) in the left-hand column and a reason in the right-hand
column.
Assertion
Reason
Copper reacts spontaneously with zinc ions
Copper ions is a stronger oxidizing
and forms copper ions and zinc.
agent than zinc ions.
Select one of the following.
a. if both assertion and reason are true statements, and the reason is a correct explanation of
the assertion
b. if both assertion and reason are true statements, and the reason is not a correct explanation
of the assertion
c. if the assertion is true but the reason is false
d. if the assertion is false but the reason is a true statement.
e. if both assertion and reason are false statements
____ 130. This question consists of an assertion (statement) in the left-hand column and a reason in the right-hand
column.
Assertion
Reason
Zinc ions react with metallic silver
Silver is a stronger reducing agent
spontaneously and form zinc and silver
than zinc.
ions.
Select one of the following.
a. if both assertion and reason are true statements, and the reason is a correct explanation of
the assertion
b. if both assertion and reason are true statements, and the reason is not a correct explanation
of the assertion
c. if the assertion is true but the reason is false
d. if the assertion is false but the reason is a true statement
e. if both assertion and reason are false statements
____ 131. This question consists of an assertion (statement) in the left-hand column and a reason in the right-hand
column.
Assertion
Reason
Hydrogen ions react with metallic zinc and
Zinc ions is a stronger oxidizing
form hydrogen gas and zinc ions.
agent than hydrogen ions.
Select one of the following.
a. if both assertion and reason are true statements, and the reason is a correct explanation of
the assertion
b. if both assertion and reason are true statements, and the reason is not a correct explanation
of the assertion
c. if the assertion is true but the reason is false
d. if the assertion is false but the reason is a true statement.
e. if both assertion and reason are false statements
____ 132. This question consists of an assertion (statement) in the left-hand column and a reason in the right-hand
column.
Assertion
Copper ions react with metallic magnesium
and form copper and magnesium ions.
Reason
Copper ions is a stronger oxidizing
agent than magnesium ions.
Select one of the following.
a. if both assertion and reason are true statements, and the reason is a correct explanation of
the assertion
b. if both assertion and reason are true statements, and the reason is not a correct explanation
of the assertion
c. if the assertion is true but the reason is false
d. if the assertion is false but the reason is a true statement
e. if both assertion and reason are false statements
____ 133. Consider the four hypothetical metals W, X, Y and Z and their corresponding nitrate solutions
. The following observations were made when metals W
and Y were inserted into
and
solutions:
no reaction
The metallic ions, in order of decreasing ease of reduction (easiest to reduce first) are
a.
b.
c.
d.
e.
____ 134. Consider the four hypothetical metals W, X, Y and Z. The following observations were made when Y and
were inserted into
and
solutions
no reaction
The best reducing agent is
a.
d.
b.
e.
c.
____ 135. Experiments show that chlorine is reduced by both
iodine is not reduced by either
or
and
; bromine is reduced by
only;
. Which of the following is the strongest oxidizing
agent?
a.
d.
b.
e.
ion
ion
c.
____ 136. Which of the following statements are true for all electric cells?
I. electrons flow from the anode to the cathode
II. reduction occurs at the anode
III. oxidation occurs at the cathode
IV. oxidation occurs at the anode
V. reduction occurs at the cathode
a. I, IV and V
d. IV and V
b. I, II and III
e. I and III
c. II and III
____ 137. The following two half-reactions are involved in a galvanic cell:
At standard conditions, what species are produced at each electrode?
a.
is produced at the cathode and
at the anode
b.
is produced at the cathode and
at the anode
c.
is produced at the anode and
at the cathode
d.
is produced at the cathode and
at the anode
e.
is produced at the cathode and
at the anode
____ 138. An electrochemical cell consists of a left compartment with a zinc electrode in contact with 1.0 mol/L
and a right compartment with a silver electrode in contact with 1.0 mol/L
. The
standard reduction potentials are
When this cell is allowed to operate at 25C, which of the following statements is true?
a. electrons will flow from right to left through the wire
b.
ions will be reduced to
metal
c.
the concentration of
ions in right compartment will increase
d. the silver electrode will be the cathode
e. the standard cell potential for this cell is 0.04 V
____ 139. An electrochemical cell is set up with a copper electrode in contact with 1.0 mol/L
electrode in contact with 1.0 mol/L
. The standard reduction potentials are
and a lead
At 25 C, the standard cell potential for this galvanic cell in volts is
a. 0.13
d. 0.21
b. 0.34
e. 0.94
c. 0.47
____ 140. In the electrochemical cell above, the left half cell is set up with a zinc electrode in contact with 1.0 mol/L
and the right half-cell is set up with a silver electrode in contact with 1.0 mol/L
.
The relevant reduction potentials are
Which of the following statements is false?
a. the silver electrode is the cathode
b.
increasing the
will increase the cell voltage
c. electrons in the external circuit will flow from zinc to silver
d. the standard cell potential for this cell is 1.56 V
e. the zinc electrode is the anode
____ 141. Consider the above cell at 25 C.
In the left half-cell, a lead electrode is in contact with 0.10 mol/L
a copper electrode is in contact with 0.20 mol/L
and in the right half-cell,
. The standard reduction potentials are as
follows:
Which of the following statements about this cell is false?
a.
ions migrate into the left half-cell through the salt bridge
b. electrons flow from the copper electrode to the lead electrode
c. the cell is not at standard conditions
d.
ions migrate into the right half-cell through the salt bridge
e. reduction occurs at the copper electrode
____ 142. The following half reactions are involved in an electrochemical cell:
The addition of sodium chloride solution,
, to the silver half-cell results in the precipitation of
silver chloride,
. Which of the following voltage changes will occur as
is added to the
silver half-cell?
a. the cell voltage will decrease
d. the cell voltage will not change
b. the cell voltage will drop to zero
e. the cell voltage will double
c. the cell voltage will increase
____ 143. This question consists of an assertion (statement) in the left-hand column and a reason in the right-hand
column.
Assertion
Reason
The voltage of an electrochemical cell does
Operating an electrochemical cell changes
not remain constant as electrons flow in the
the concentration of ions in the half-cells
external circuit
which results in an increase in the cell
voltage
Select one of the following.
a. if both assertion and reason are true statements, and the reason is a correct explanation of
the assertion
b. if both assertion and reason are true statements, and the reason is not a correct explanation
of the assertion
c. if the assertion is true but the reason is false
d. if the assertion is false but the reason is a true statement
e. if both assertion and reason are false statements
____ 144. This question consists of an assertion (statement) in the left-hand column and a reason in the right-hand
column.
Assertion
Reason
In the electrochemical cell:
At the zinc electrode, zinc atoms are
oxidized to
the zinc electrode is the negative terminal
of the cell.
ions and electrons
are released.
Select one of the following.
a. if both assertion and reason are true statements, and the reason is a correct explanation of
the assertion
b. if both assertion and reason are true statements, and the reason is not a correct explanation
of the assertion
c. if the assertion is true but the reason is false\
d. if the assertion is false but the reason is a true statement
e. if both assertion and reason are false statements
____ 145. This question consists of an assertion (statement) in the left-hand column and a reason in the right-hand
column.
Assertion
n the electrochemical cell:
Reason
At the silver electrode, silver atoms
are oxidized to
the silver electrode is the negative terminal
of the cell.
ions and
electrons are released.
Select one of the following.
a. if both assertion and reason are true statements, and the reason is a correct explanation of
the assertion
b. if both assertion and reason are true statements, and the reason is not a correct explanation
of the assertion
c. if the assertion is true but the reason is false
d. if the assertion is false but the reason is a true statement
e. if both assertion and reason are false statements
____ 146. Given
The
for the reaction
is
a. +0.18 V
b.
0.18 V
c.
0.67 V
d. +0.37 V
e.
0.37 V
____ 147. Given the following half-cell reactions:
At 25C, the initial cell voltage of the cell shown in the diagram above is
a.
1.18 V
d.
0.30 V
b.
0.30 V
c.
1.18 V
____ 148. Consider the above cell:
e.
1.34 V
The standard reduction potentials are
Which of the following statements about this cell is false?
a. the chromium ( ) electrode is the anode
b. reduction occurs at the iron ( ) electrode
c. electrons flow from the iron ( ) electrode to the chromium (
circuit
d. the iron ( ) electrode is the positive terminal
e. oxidation occurs at the chromium ( ) electrode
) electrode in the external
____ 149. The concentration of both solutions in the cell below are 1.0 mol/L.
Given the following standard reduction potentials:
Which of the following statements are true?
I. oxidation occurs at the Ag electrode.
II. the Ag electrode is the negative terminal of the cell.
III. electrons flow from the Ni electrode to the Ag electrode through the external circuit.
IV. the Ni electrode is the anode.
a. I and II
d. III and IV
b. I and III
e. II and IV
c. II and III
____ 150. Consider the electrochemical cell above.
The half-cell reactions are
When the cell is allowed to operate, which of the following statements is true?
a.
ions migrate from the Ag half-cell to the Ni half-cell through the salt bridge
b. the Ag electrode is the anode
c. the Ni electrode is the cathode
d. reduction occurs at the Ni electrode
e.
the initial
for the cell is 0.56 V
____ 151. Given the following standard reduction potentials:
Which reactions are expected to occur in the beakers below
I.
II.
III.
a. I only
b. I and II
c. I and III
____ 152. Given
d. II and III
e. III only
for
, which of the following are able to oxidize
I.
II.
III.
IV.
a. I and II
b. II and III
d. I, III and IV
e. I, II and III
?
c. I and IV
____ 153. An electrochemical cell involves the following half-reactions:
What is the standard cell potential,
, for this electrochemical cell?
a. 1.46 V
d. 0.66 V
b. 1.08 V
e. 0.52 V
c. 0.94 V
____ 154. Given the standard reduction potentials for the following half-reactions:
What is the standard reduction potential for the reaction
?
a. +1.16 V
d. +0.58 V
b. +0.10 V
e.
0.58 V
c.
0.10 V
____ 155. Given the standard reduction potentials for the following half-reactions:
What is
for the reaction
?
a. +0.05 V
b. +0.43 V
c. +1.11 V
____ 156. Given
Calculate
a. +0.59 V
b. +0.92 V
c. +1.40 V
____ 157. Given
d. +1.20 V
e. +1.88 V
for the reaction
d. +1.80 V
e. +2.13 V
Which of the following reactions is not spontaneous under standard conditions?
a.
b.
c.
d.
e.
____ 158. An electric cell consists of a silver electrode in 1.0 mol/L solution of
(silver nitrate), a copper
electrode in 1.0 mol/L solution of
(copper nitrate) and a salt bridge. The spontaneous cell
reaction is
When the two electrodes are connected by a wire, which of the following does not take place?
a. electrons flow in the wire from the copper electrode to the silver electrode
b. the silver electrode increases in mass as the cell operates
c. there is a net movement of silver ions through the salt bridge from the silver half-cell to
the copper half-cell
d. there is a net movement of copper ions through the salt bridge from the copper half-cell to
the silver half-cell
e. the copper electrode decreases in mass as the cell operates
____ 159. An electrochemical cell consists of a chromium electrode in 1.0 mol/L solution of
(chromium
nitrate), a silver electrode in 1.0 mol/L solution of
(silver nitrate) and a salt bridge. The
spontaneous cell reaction is
When the two electrodes are connected by a wire, which of the following does not take place?
a. the silver electrode increases in mass as the cell operates
b. negative ions pass through the salt bridge from the silver half-cell to the chromium halfcell
c. some positive chromium ions pass through the salt bridge from the chromium half-cell to
the silver half-cell
d. the chromium electrode decreases in mass as the cell operates
e. electrons flow in the external circuit from the silver electrode to the chromium electrode
____ 160. Consider the following:
Which of the following half-cells, when combined with a standard hydrogen reference half-cell under
standard conditions, will produce an electric cell with the greatest voltage?
a. zinc-zinc ions
d. platinum-platinum ions
b. iron-iron ions
e. cobalt-cobalt ions
c. nickel-nickel ions
____ 161. Given
If we used the silver/silver ion electrode as the standard for
values instead of the hydrogen/hydrogen
ion electrode, the standard reduction potentials ( ) for the four half-reactions above in corresponding
order are
a.
0.40 V 0.00 V 0.80 V 1.24 V
d.
2.00 V 0.00 V 1.24 V 1.68 V
b.
1.20 V 0.00 V 0.80 V 0.44 V
e.
2.00 V 0.00 V 1.24 V 1.68 V
c.
0.40 V 0.00 V 0.80 V 1.24 V
____ 162. Given
If we used the iron/iron ion electrode as the standard for
electrode, the standard reduction potentials (
are
a. +1.64 V +1.24 V +0.44 V 0.00
b.
1.64 V 1.24 V 0.44 V 0.00
c. +1.20 V +0.80 V +0.44 V 0.00
____ 163. Consider the following:
values instead of the hydrogen/hydrogen ion
) for the four half-reactions above in corresponding order
d.
0.76 V 0.36 V 0.44 V 0.00
e. +0.76 V +0.36 V +0.44 V 0.00
Which half-cell, when combined with a standard hydrogen reference half-cell under standard conditions,
will produce an electrochemical cell with the greatest voltage?
a.
d.
X
W
b.
Y
c.
e.
Q
Z
____ 164. An electrochemical cell consists of a chromium electrode in 1.0 mol/L solution of
(chromium
nitrate), a silver electrode in 1.0 mol/L solution of
(silver nitrate) and a salt bridge. The cell halfreactions are
When the two electrodes are connected by a wire, which of the following takes place?
I.
ions migrate from the cathode to the anode through the salt bridge.
II. electrons migrate from the anode to the cathode through the salt bridge.
III.
ions migrate to the silver half-cell through the salt bridge.
a. I only
d. I and II
b. II only
e. I and III
c. III only
____ 165. Consider the following:
In an electrochemical cell, the combination of electrodes (and corresponding electrolytes) that would
produce the highest voltage is
a.
d.
b.
e.
c.
____ 166. Which of the following statements are true?
I aluminum is protected from corrosion by the formation of a thin layer of aluminum oxide on the
surface.
II. ron is protected from corrosion by the formation of a layer of iron oxide on the surface.
III. cathodic protection of iron uses a metal that is more easily reduced than iron.
IV. cathodic protection of iron uses a metal that is more easily oxidized than iron.
a. I and II
d. II and III
b. I and III
e. II and IV
c. I and IV
____ 167. The function of the salt bridge in a galvanic cell is
a. to act as a nonelectrolyte
b. to provide an external circuit for the flow of electrons from one half-cell to the other
c. to provide a path for the migration of ions from one half-cell to the other
d. to allow the solution in each half-cell to become electrically charged
e. to provide a path for the flow of electrons internally from one half-cell to the other
4u exam mc2
Answers
Unit 5 - Electrochemistry
93.
94.
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138.
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D
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K/U
K/U
K/U
K/U
K/U
K/U
C
C
K/U
K/U
K/U
C
C
C
C
C
K/U
K/U
K/U
C
C
C
C
C
C
K/U
C
K/U
C
C
C
C
C
C
C
K/U
K/U
C
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
9.3
9.1
9.1
9.1
9.1
9.1
9.1
9.1
9.1
9.1
9.1
9.1
9.3
9.1
9.2
9.3
9.1
9.1
9.1
9.2
9.3
9.3
9.3
9.3
9.1
9.1
9.1
9.2
9.2
9.2
9.2
9.2
9.1
9.1
9.3
9.1
9.3
9.3
9.3
9.3
9.3
9.3
9.3
9.5
9.5
9.5
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
EL1.01
EL1.01
EL1.01
EL1.01
EL1.01
EL1.01
EL1.01
EL1.01
EL1.01
EL1.01
EL1.01
EL1.01
EL1.01
EL1.01
EL2.03
EL2.02
EL1.01
EL1.01
EL1.01
EL2.03
EL2.02
EL2.02
EL2.01
EL2.01
EL1.01
EL1.01
EL1.01
EL2.03
EL2.03
EL2.03
EL2.03
EL2.03
EL2.01
EL1.01
EL2.01
EL1.01
EL2.05
EL2.05
EL2.05
EL2.05
EL2.02
EL2.02
EL2.01
EL1.02
EL1.02
EL2.04
139.
140.
141.
142.
143.
144.
145.
146.
147.
148.
149.
150.
151.
152.
153.
154.
155.
156.
157.
158.
159.
160.
161.
162.
163.
164.
165.
166.
167.
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
ANS:
C
B
B
A
C
A
E
E
D
C
D
A
D
E
C
D
B
D
A
C
E
D
C
A
D
E
C
B
C
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
REF:
C
K/U
C
K/U
K/U
C
C
K/U
K/U
K/U
C
K/U
C
C
K/U
K/U
K/U
K/U
C
C
C
K/U
K/U
K/U
K/U
C
K/U
K/U
K/U
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
OBJ:
9.5
9.5
9.5
9.5
9.5
9.5
9.5
9.5
9.5
9.5
9.5
9.5
9.3
9.3
9.5
9.5
9.3
9.3
9.3
9.5
9.5
9.5
9.5
9.5
9.5
9.5
9.3
9.6
9.5
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
LOC:
EL2.04
EL1.02
EL2.04
EL1.02
EL1.02
EL2.04
EL2.04
EL1.03
EL1.03
EL1.02
EL2.04
EL1.02
EL2.05
EL2.05
EL1.03
EL1.03
EL1.03
EL1.03
EL2.05
EL2.04
EL2.04
EL1.04
EL1.04
EL1.04
EL1.04
EL2.04
EL1.03
EL1.06
EL1.02