Exam 3 hw 1Marks 1The ___________ is outside of the reg.docx

Exam 3 hw
1
Marks: 1
The ___________ is outside of the region of focus and includes
everything but the region of focus.
Choose one answer.
A. surroundings
B. system
C. universe
Question
2
Marks: 1
The ___________ is the region of focus (usually where the
reaction is occuring).
Choose one answer.
A. system
B. surroundings
C. universe

Question
3
Marks: 1
How much heat (in kJ) is evolved (under standard conditions)
when 191.78 g of copper reacts to form copper(II) oxide?
Answer:
Question
4
Marks: 1
What is the change in enthalpy (in kJ) under standard conditions
when 11.22 g of benzene is combusted?
Answer:
Question
5
Marks: 1
What is the change in enthalpy (in kJ) under standard conditions
when 245.02 g of sodium sulfate dissolves in water?
Answer:
Question
6
Marks: 1
What mass (in g) of aluminum is needed to evolve 1026.2 kJ of
heat under standard conditions as it forms aluminum oxide?
Answer:
Question
7
Marks: 1
What mass (in g) of iron is needed to evolve 913.6 kJ of heat

under standard conditions as it forms iron(III) oxide?
Answer:
Question
8
Marks: 1
A system which allows for an transfer of energy but not matter
is
Choose one answer.
A. closed.
B. open.
C. isolated.
Question
9
Marks: 1
A system which does not allow for an transfer of matter or
energy is
Choose one answer.
A. isolated.
B. closed.
C. open.

Question
10
Marks: 1
What is the enthalpy of combustion (in kJ/mol) for acetone
(CH3COCH3) under standard conditions (water is produced as a
liquid)? Use the appendix in your textbook, do not enter units,
and answer with 5 significant digits.
Answer:
Question
11
Marks: 1
What is the enthalpy of combustion (in kJ/mol) for carbon under
standard conditions? Use the appendix in your textbook, do not
enter units, and answer with 4 significant digits.
Answer:
Question
12
Marks: 1
What is the enthalpy of formation of butane (C4H10) if the
enthalpy of combustion for butane is -2876.9 kJ/mol (water is
produced as a liquid)? Use the appendix in your textbook, do
not enter units, and answer with 3 significant digits.
Answer:
Question
13
Marks: 1
What is the sum of the stoichimetric coefficients for the
formation reaction of magnesium carbonate? Enter any fraction
as a decimal (to two significant digits).
Answer:

Question
14
Marks: 1
What is the sum of the stoichiometric coefficients the formation
reaction for methanol (CH3OH)? Enter any fraction as a
decimal.
Answer:
Question
15
Marks: 1
What is the coefficient for oxygen in the formation reaction for
methanol (CH3OH)? Enter any fraction as a decimal.
Answer:
Question
16
Marks: 1
What is the enthalpy of combustion (in kJ/mol) for methanol
(CH3OH) under standard conditions (water is produced as a
liquid)? Use the appendix in your textbook, do not enter units,
and answer with 4 significant digits.
Answer:
Question
17
Marks: 1
What is the enthalpy of formation of propylene (C3H6) if the
enthalpy of combustion for propylene is -2058.3 kJ/mol (water
is produced as a liquid)? Use the appendix in your textbook, do
not enter units, and answer with 3 significant digits.

Answer:
Question
18
Marks: 1
Which processes are spontaneous?
Choose at least one answer.
a. dissolved sodium chloride in water forming solid sodium
chloride
b. solid sodium chloride dissolving in water
c. dissolved sugar in water forming solid sugar
d. solid sugar dissolving in water
Question
19
Marks: 1
How many different ways can four particles be placed in two
different (equally probable) containers?
Answer:
Question
20
Marks: 1

Using Appendix 2 in your textbook, what is the standard change
in entropy (in J/K) at 25oC of the reaction:
2C6H6(l) + 15O2(g) --> 12CO2(g) + 6H2O(l)?
Answer:
21
Marks: 1
2NO(g) + N2(g) --> 2N2O(g)?
Answer:
Question
22
Marks: 1
2O3(g) --> 3O2(g)?
Answer:
Question
23
Marks: 1
What is the sign on the change in entropy for the process:
2N2(g) + O2(g)--> 2N2O(g)
Choose one answer.
a. entropy is increasing
b. entropy is unchanged
c. entropy is decreasing

d. entropy cannot be approximated
Question
24
Marks: 1
2N2O5(g)--> 4NO2(g) + O2(g)
Choose one answer.
Question
25
Marks: 1
Cgraphite(s) at 0oC --> Cgraphite(s) at 25oC
Choose one answer.

Question
26
Marks: 1
H2O(g) --> H2O(l)
Choose one answer.
Question
27
Marks: 1
KBr(s) --> K+(aq) + Br-(aq)
Choose one answer.

Question
28
Marks: 1
PCl5(g) --> PCl3(g) + Cl2(g)
Choose one answer.
Question
29
Marks: 1
What is the order of the lowest entropy (1 = lowest) to highest
entropy (3 = highest)?
H2O(g)
Choose...
1 = lowest

3 = highest
2 = moderate
H2O(l)
Choose...
1 = lowest
3 = highest
2 = moderate
H2O(s)
Choose...
1 = lowest
3 = highest
2 = moderate
Question
30
Marks: 1
Br2(g)
Choose...
3 = highest
1 = lowest
2 = moderate
Cl2(g)
Choose...
3 = highest
1 = lowest
2 = moderate

F2(g)
Choose...
3 = highest
1 = lowest
2 = moderate
Question
31
Marks: 1
C2H4(g)
Choose...
3 = highest
2 = moderate
1 = lowest
C3H6(g)
Choose...
3 = highest
2 = moderate
1 = lowest
C4H8(g)
Choose...
3 = highest
2 = moderate
1 = lowest

Question
32
Marks: 1
What combination will always result in a spontaneous process?
Choose one answer.
a. The entropy of the system increases and the entropy of the
surroundings decreases.
b. The entropy of the system decreases but the entropy of the
surroundings increases.
c. The entropy of the system increases but the entropy of the
surroundings decreases.
d. The entropy of the system increases and the entropy of the
surroundings increases.
Question
33
Marks: 1
What is the second law of thermodynamics?
Choose one answer.
a. The entropy of the universe is constant for a spontaneous
process.
b. The entropy of the universe increases for a spontaneous
process.

c. The entropy of the universe decreases for a spontaneous
process.
d. The entropy of the universe is zero for a spontaneous process.
Question
34
Marks: 1
What will result is a process being spontaneous?
(More than one answer can be correct - each correct answer will
result in full credit)
Choose one answer.
a. Both the change in entropy of the system and the change in
entropy of the surroundings are greater than zero.
b. Both the change in entropy of the system and the change in
entropy of the surroundings are less than zero.
c. The change in entropy of the system is greater than zero
while the change in entropy of the surroundings is less than zero
and the change in entropy of the system is greater in magnitude
than the change in entropy of the surroundings.
d. The change in entropy of the system is greater than zero
while the change in entropy of the surroundings is less than zero
and the change in entropy of the system is lower in magnitude
than the change in entropy of the surroundings.

Question
35
Marks: 1
Which describes an endothermic system in which the entropy of
the universe is increasing (spontaneous)?
Choose one answer.
a. Enthalpy of the surroundings decreases and the entropy of the
system decreases
b. Enthalpy of the surroundings decreases and the entropy of the
system increases
c. Enthalpy of the surroundings increases and the entropy of the
system decreases
d. Enthalpy of the surroundings increases and the entropy of the
system increases
Question
36
Marks: 1
For the reaction, 2CO(g) + O2(g) --> 2CO2(g), which statement
is true?
Choose one answer.
a. This reaction is always spontaneous.
b. This reaction is never spontaneous.

c. This reaction is spontaneous at low temperatures and not
spontaneous at high temperatures.
d. This reaction is not spontaneous at low temperatures and
spontaneous at high temperatures.
Question
37
Marks: 1
Using Appendix 2 in your textbook, at what temperature (in K)
will the reaction, 2CO(g) + O2(g) --> 2CO2(g), change in
spontaneity?
Assume standard change in enthalpy and standard change in
entropy do not change with temperature.
Answer:
Question
38
Marks: 1
Using Appendix 2 in your textbook, what is the value for the
standard change in Gibbs free energy (in kJ) at 25oC of the
reaction:
2C6H6(l) + 15O2(g) --> 12CO2(g) + 6H2O(l)?
Answer:
Question
39
Marks: 1
reaction:
2NO(g) + N2(g) --> 2N2O(g)?

Answer:
Question
40
Marks: 1
reaction:
2O3(g) --> 3O2(g)?
Answer:
41
Marks: 1
reaction:
C2H4(g) + H2(g) --> C2H6(g)?
Answer:
Question
42
Marks: 1
What is the value for the standard change in Gibbs free energy
(in kJ), when the standard change in enthalpy is (-571.8) kJ and
the standard change in entropy is (-149.73) J/K at 25oC?
Answer:
Question
43
Marks: 1
What is the value for the standard change in Gibbs free energy
(in kJ), when the standard change in enthalpy is 559.7 kJ and

the standard change in entropy is 130.62 J/K at 25oC?
Answer:
Question
44
Marks: 1
Which combination will result in a system that is always
spontaneous?
Choose one answer.
a. ΔHsys< 0 and ΔSsys< 0
b. ΔHsys< 0 and ΔSsys > 0
c. ΔHsys > 0 and ΔSsys< 0
d. ΔHsys > 0 and ΔSsys > 0
Question
45
Marks: 1
Which combination will result in a system that is never
spontaneous?
Choose one answer.

Question
46
Marks: 1
Which combination will result in a system that is spontaneous at
high temperatures only?
Choose one answer.
Question
47
Marks: 1
Which combination will result in a system that is spontaneous at
low temperatures only?
Choose one answer.

Question
48
Marks: 1
Given the Ka of benzoic acid from Chapter 16 in your textbook,
what is the value of change in Gibbs free energy (in kJ/mol) at
25oC for this process?
Answer:
Question
49
Marks: 1
Given the Kb of urea from Chapter 16 in your textbook, what is
the value of change in Gibbs free energy (in kJ/mol) at 25oC for
this process?
Answer:
Question
50
Marks: 1
Given the Ksp of cobalt(II) sulfide from Chapter 17 in your
textbook, what is the value of change in Gibbs free energy (in
kJ/mol) at 25oC for this process?
Answer:
Question

51
Marks: 1
Given the Kw of water from Chapter 16 in your textbook, what
is the value of change in Gibbs free energy (in kJ/mol) at 25oC
for this process?
Answer:
Question
52
Marks: 1
What is true for a spontaneous process?
Choose one answer.
a. ΔGsys< 0 and K < 1
b. ΔGsys > 0 and K < 1
c. ΔGsys< 0 and K > 1
d. ΔGsys > 0 and K > 1
Question
53
Marks: 1
When ΔGo > 0 and Q > K,
Choose one answer.
a. ΔG > 0 and the reaction will shift to the right.
b. ΔG > 0 and the reaction will shift to the left.

c. ΔG < 0 and the reaction will shift to the right.
d. ΔG < 0 and the reaction will shift to the left.
Question
54
Marks: 1
When ΔGo < 0 and Q < K,
Choose one answer.
a. ΔG > 0 and the reaction will shift to the right.
b. ΔG > 0 and the reaction will shift to the left.
c. ΔG < 0 and the reaction will shift to the right.
d. ΔG < 0 and the reaction will shift to the left.
Question
55
Marks: 1
When ΔGo < 0 and the system is at equilibrium,
Choose one answer.
a. ΔG = 0 and Q = K.
b. ΔG = 0 and Q = 0.

c. ΔG = ΔGo and Q = K.
d. ΔG = ΔGo and Q = 0.
Question
56
Marks: 1
In the reaction of bromine with potassium iodide to produce
potassium bromide and iodine, what is reduced and what is the
reducing agent?
Choose one answer.
A. bromine is reduced and potassium iodide is the reducing
agent
B. bromine is reduced and bromine is the reducing agent
C. iodine is reduced and potassium iodide is the reducing agent
D. iodine is reduced and bromine is the reducing agent
E. potassium is reduced and potassium iodide is the reducing
agent
F. potassium is reduced and bromine is the reducing agent

Question
57
Marks: 1
In the reaction of sodium with water to produce sodium
hydroxide and hydrogen gas, what is reduced and what is the
reducing agent?
Choose one answer.
A. hydrogen is reduced and sodium is the reducing agent
B. hydrogen is reduced and water is the reducing agent
C. sodium is reduced and sodium is the reducing agent
D. sodium is reduced and water is the reducing agent
E. oxygen is reduced and sodium is the reducing agent
F. oxygen is reduced and water is the reducing agent
Question
58
Marks: 1
In which reaction is iron reduced?
Choose one answer.
A. iron(III) oxide reacting with carbon monoxide to form liquid
iron and carbon dioxide

B. iron(II) chloride reacting with potassium nitrate and
hydrochloric acid to form nitric oxide (NO), iron(III) chloride,
potassium chloride and water
C. iron(II) nitrate reacting with sodium hydroxide to form
iron(II) hydroxide and sodium nitrate
D. iron reacting with nitric acid to form iron(II) nitrate and
hydrogen gas
E. iron reacting with nickel(II) chloride to form iron(II)
chloride and nickel
F. iron(III) acetate reacting with potassium sulfide to form
iron(III) sulfide and potassium acetate
Question
59
Marks: 1
In which reaction is nitrogen reduced?
Choose one answer.
A. iron(II) chloride reacting with potassium nitrate and
hydrochloric acid to form nitric oxide (NO), iron(III) chloride,
potassium chloride and water
B. nitrogen reacting with hydrogen to form ammonia
C. copper(II) nitrate reacting with potassium sulfide to form the

precipitate copper(II) sulfide and aqueous potassium nitrate
D. nitrous acid reacting with potassium hydroxide to form
potassium nitrite and water
E. iron reacting with nitric acid to form iron(II) nitrate and
hydrogen gas
F. iron(II) nitrate reacting with sodium hydroxide to form
iron(II) hydroxide and sodium nitrate
Question
60
Marks: 1
Which reactions are redox reactions?
Choose at least one answer.
A. hydrochloric acid reacting with nickel metal to form
hydrogen gas and aqueous nickel(II) chloride
B. sodium bromide reacting with chlorine to form sodium
chloride and bromine
C. sodium hydroxide reacting with aluminum chloride to form
solid aluminum hydroxide and sodium chloride
D. sodium hydroxide reacting with hydrochloric acid to form
water and sodium chloride

E. sodium hydroxide reacting with potassium to form potassium
hydroxide and sodium
F. acetic acid reacting with sodium bicarbonate to form carbon
dioxide, water and sodium acetate
61
Marks: 1
Which substance is the strongest oxidizing agent?
Choose one answer.
A. Ag+
B. Sn2+
C. Ni2+
D. Fe2+
E. Cr3+
F. Na+
Question
62
Marks: 1

Which substance is the strongest reducing agent?
Choose one answer.
A. Mg
B. Al
C. Cd
D. Fe
E. Pb
F. H2
Question
63
Marks: 1
How many electrons are transferred in the redox reaction taking
place in acidic solution:
Sn2+(aq) + Cr2O72-(aq) --> Cr3+(aq) + Sn4+(aq)?
Answer:
Question
64
Marks: 1
How many electrons are transferred in the redox reaction taking
place in basic solution:
Cr(s) + ClO4-(aq) --> ClO3-(aq) + Cr3+(aq)?

Answer:
Question
65
Marks: 1
How many electrons are transferred in the redox reaction:
Pb2+(aq) + Ni(s) --> Pb(s) + Ni2+(aq)?
Answer:
Question
66
Marks: 1
How many electrons are transferred in the redox reaction:
Zn(s) + Fe3+(aq) --> Zn2+(aq) + Fe(s)?
Answer:
Question
67
Marks: 1
What is the stoichiometric coefficient for the hydrogen ion in
the balanced redox reaction of:
Cl-(aq) + NO3-(aq) --> NO(g) + Cl2(g) when balanced in acidic
solution?
Answer:
Question
68
Marks: 1
What is the stoichiometric coefficient for the hydrogen ion in
Zn(s) + NO3-(aq) --> NO2(g) + Zn2+(aq) when balanced in
acidic solution?

Answer:
Question
69
Marks: 1
What is the stoichiometric coefficient for the hydroxide ion in
In+(aq) + ClO-(aq) --> Cl-(aq) + In3+(aq) when balanced in
basic solution?
Answer:
Question
70
Marks: 1
Cr(s) + ClO4-(aq) --> ClO3-(aq) + Cr3+(aq) when balanced in
basic solution?
Answer:
Question
71
Marks: 1
Na(s) + H2O(l) --> Na+(aq) + H2(g) when balanced in basic
solution?
Answer:
Question
72
Marks: 1

What is the stoichiometric coefficient for the substance
oxidized (as a reactant) in the balanced redox reaction of:
Fe(s) + MnO4-(aq) --> Mn2+(aq) + Fe3+(aq) when balanced in
acidic solution?
Answer:
Question
73
Marks: 1
What is the stoichiometric coefficient for the substance
oxidized (as a reactant) in the balanced redox reaction of:
Pb(s) + MnO42-(aq) --> MnO2(s) + Pb2+(aq) when balanced in
basic solution?
Answer:
Question
74
Marks: 1
What is the stoichiometric coefficient for the substance reduced
(as a reactant) in the balanced redox reaction of:
Fe(s) + MnO4-(aq) --> Mn2+(aq) + Fe3+(aq) when balanced in
acidic solution?
Answer:
Question
75
Marks: 1
What is the stoichiometric coefficient for the substance reduced
(as a reactant) in the balanced redox reaction of:
Pb(s) + MnO42-(aq) --> MnO2(s) + Pb2+(aq) when balanced in
basic solution?
Answer:

Question
76
Marks: 1
What is the stoichiometric coefficient for water in the balanced
redox reaction of:
In+(aq) + ClO-(aq) --> Cl-(aq) + In3+(aq) when balanced in
basic solution?
Answer:
Question
77
Marks: 1
What is the stoichiometric coefficient for water in the balanced
redox reaction of:
Cr(s) + ClO4-(aq) --> ClO3-(aq) + Cr3+(aq) when balanced in
basic solution?
Answer:
Question
78
A galvanic cell consists of a iron electrode in 1.0 M Fe(NO3)2
and a copper electrode in 1.0 M Cu(NO3)2. What is the standard
cell potential (emf, in V) of this cell at 25oC?
Answer:
Question
79
A galvanic cell consists of a lead electrode in 1.0 M Pb(NO3)2
and a aluminum electrode in 1.0 M Al(NO3)3. What is the
standard cell potential (emf, in V) of this cell at 25oC?
Answer:

Question
80
A galvanic cell consists of a lead electrode in 1.0 M Pb(NO3)2
and a aluminum electrode in 1.0 M Al(NO3)3. What is the
standard Gibbs free energy (in kJ) of this cell at 25oC?
Answer:
81
A galvanic cell consists of a silver electrode in 1.0 M AgNO3
and a chromium electrode in 1.0 M Cr(NO3)3. What is the
standard Gibbs free energy (in kJ) of this cell at 25oC?
Answer:
Question
82
A galvanic cell consists of a tin electrode in 1.0 M Sn(NO3)2
and a cadmium electrode in 1.0 M Cd(NO3)2. What is the
standard cell potential (emf, in V) of this cell at 25oC?
Answer:
Question
83
A galvanic cell consists of a zinc electrode in 1.0 M Zn(NO3)2
and a nickel electrode in 1.0 M Ni(NO3)2. What is the standard
cell potential (emf, in V) of this cell at 25oC?
Answer:
Question
84
For a galvanic cell,
Choose one answer.
a. Eo > 0.

b. Eo = 0.
c. Eo< 0.
d. Eo cannot be approximated.
Question
85
For a galvanic cell, Eo equals
Choose one answer.
a. Eocathode - Eoanode, where each value is the standard
reduction potential
b. Eoanode - Eocathode, where each value is the standard
reduction potential
c. Eocathode + Eoanode, where each value is the standard
reduction potential
d. Eoanode * Eocathode, where each value is the standard
reduction potential
Question
86
What direction do the electrons and the cations flow in a
galvanic cell?

Choose one answer.
a. the electrons flow from the cathode to the anode and the
cations flow from the oxidation half-reaction to the reduction
half-reaction to charge balance
b. the electrons flow from the anode to the cathode and the
cations flow from the oxidation half-reaction to the reduction
c. the electrons flow from the cathode to the anode and the
cations flow from the reduction half-reaction to the oxidation
d. the electrons flow from the anode to the cathode and the
cations flow from the reduction half-reaction to the oxidation
Question
87
What is the standard cell potential (emf, in V) of this cell at
25oC?
Cr |Cr3+ (1.0 M) ǁ H2SO4 (1 M) |SO2 (1 atm) |Pt(s)
Answer:
Question
88
What is the standard cell potential (emf, in V) of this cell at
25oC?
Mn | Mn2+(1.0 M) ǁ H2SO4 (1 M) |SO2 (1 atm) |Pt(s)
Answer:

Question
89
What is the standard Gibbs free energy (in kJ) of this cell at
25oC?
Cr |Cr3+ (1.0 M) ǁ H2SO4 (1 M) |SO2 (1 atm) |Pt(s)
Answer:
Question
90
What is the standard Gibbs free energy (in kJ) of this cell at
25oC?
Mn | Mn2+(1.0 M) ǁ H2SO4 (1 M) |SO2 (1 atm) |Pt(s)
Answer:
Question
91
What occurs at the anode?
Choose one answer.
a. oxidation and electrons are consumed
b. oxidation and electrons are produced
c. reduction and electrons are consumed
d. reduction and electrons are produced
Question

92
What occurs at the cathode?
Choose one answer.
a. oxidation and electrons are consumed
b. oxidation and electrons are produced
c. reduction and electrons are consumed
d. reduction and electrons are produced
Question
93
A galvanic cell consists of a iron electrode in 1 M Fe(NO3)2
and a copper electrode in 1 M Cu(NO3)2. What is the
equilibrium constant for this reaction at 25oC?
Enter you answer with 2 significant digits, using the syntax of
"1.0x10(22)" for "1.0x1022"
Answer:
Question
94
For a galvanic cell,
Choose one answer.
a. Eo > 0 and ΔGo > 0.
b. Eo > 0 and ΔGo< 0.

c. Eo< 0 and ΔGo > 0.
d. Eo< 0 and ΔGo< 0.
Question
95
Which reaction is not spontaneous under standard conditions?
Choose one answer.
a. Co(s) + H2O(l) --> Co2+(aq) + H2(g)
b. Na(s) + H2O(l) --> Na+(aq) + H2(g)
c. Sn(s) + H2O(l) --> Sn2+(aq) + H2(g)
d. Zn(s) + H2O(l) --> Zn2+(aq) + H2(g)
Question
96
A galvanic cell consists of a iron electrode in 0.0412 M
Fe(NO3)2 and a copper electrode in 0.275 M Cu(NO3)2. What
is the cell potential (emf, in V) of this cell at 25oC?
Answer:
Question
97
A galvanic cell consists of a zinc electrode in 0.0270 M
Zn(NO3)2 and a nickel electrode in 0.321 M Ni(NO3)2. What is

the cell potential (emf, in V) of this cell at 25oC?
Answer:
Question
98
What is the cell potential (emf, in V) of this cell at 25oC?
Cu |Cu2+ (0.0359 M) ǁ Br2 |Br- (0.525 M)
Answer:
Question
99
What mass (in g) of aluminum can be electroplated when 0.430
amps are used for 1.021 hours using a solution of aluminum
nitrate?
Answer:
Question
100
What mass (in g) of silver can be electroplated when 0.966
amps are used for 1.079 hours using a solution of silver nitrate?
Answer:

Exam 3 hw 1Marks 1The ___________ is outside of the reg.docx

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