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CHM1045_Study_Guide_Chapters_3_4
1
...
Calculate its
formula mass
...
118
...
99
...
78
...
59
...
50
...


Calculate the molecular mass of tetraphosphorus decaoxide, P4O10, a corrosive substance which can be
used as a drying agent
...
469
...
283
...
190
...
139
...
94
...


Calculate the molecular or formula mass of rubidium carbonate, Rb2CO3
...
340
...
255
...
230
...
145
...
113
...


Calculate the molecular or formula mass of (NH4)3AsO4
...
417
...
193
...
165
...
156
...
108
...


Aluminum sulfate, Al2(SO4)3, is used in tanning leather, purifying water, and manufacture of
antiperspirants
...

A
...
06 g/mol
B
...
15 g/mol
C
...
15 g/mol
D
...
02 g/mol
E
...
98 g/mol

6
...

A
...
87 g/mol
B
...
79 g/mol
C
...
79 g/mol
D
...
89 g/mol
E
...
71 g/mol

7
...

A
...
70 g/mol
C
...
158 g/mol
E
...


Calculate the molecular mass of menthol, C10H20O
...
156 g/mol
B
...
29 g/mol
D
...
136 g/mol

9
...
43 g/mol
B
...
151 g/mol
D
...
125 g/mol

10
...
134 g/mol
B
...
158 g/mol
D
...
162 g/mol
11
...
What is the % of carbon in sucrose, by
mass?
A
...
7%
B
...
3%
C
...
4%
D
...
1%
E
...
8%
12
...
13%
B
...
35%
D
...
52%
13
...
43
...
11
...
45
...
27
...
23%
14
...
28%
B
...
24%
D
...
42%

15
...
B O (s) + 6HF(l) → 2BF (g) + 3H O(l)
2 3
3
2
B
...
B O (s) + 2HF(l) → 2BF (g) + H O(l)
2 3
3
2
D
...
B O (s) + 6HF(l) → 2BF (g) + 6H O(l)
2 3
3
2
16
...
UO (s) + 2HF(l) → UF (s) + H O(l)
2

4

2

B
...
UO (s) + H F (l) → UF (s) + H O (l)
2

4 4

4

4 2

D
...
UO (s) + 8HF(l) → 2UF (s) + 4H O(l)
2

4

2

17
...
C H (l) + 9O (g) → 3H O(g) + 6CO (g)
6 6
2
2
2
B
...
2C H (l) + 15O (g) → 6H O(g) + 12CO (g)
6 6
2
2
2
D
...
2C H (l) + 9O (g) → 6H O(g) + 12CO (g)
6 6
2
2
2
18
...
C H O (l) + 8O (g) → 9H O(g) + 8CO (g)
8 18 3
2
2
2
B
...
2C H O (l) + 22O (g) → 9H O(g) + 16CO (g
8 18 3
2
2
2
D
...
2C H O (l) + 17O (g) → 18H O(g) + 16CO (g)
8 18 3
2
2
2
19
...
Ca (PO ) (s) + 3SiO (s) + 8C(s) → 3CaSiO (s) + 8CO(g) + P (s)
3
4 2
2
3
4
B
...
Ca (PO ) (s) + 3SiO (s) + 8C(s) → 3CaSiO (s) + 8CO(g) + 2P (s)
3
4 2
2
3
4
D
...
2Ca (PO ) (s) + 6SiO (s) + 10C(s) → 6CaSiO (s) + 10CO(g) + 4P (s)
3

4 2

2

3

4

20
...
1
B
...
3
D
...
5
21
...
3
B
...
6
D
...
24
22
...
1
B
...
3
D
...
6
23
...
What is the coefficient for O2 when the following combustion
reaction of a hydrocarbon is balanced?
___ C7H14 + ___ O2 → ___ CO2 + ___ H2O
A
...
21
C
...
10
E
...

24
...
1
B
...
9
D
...
27
25
...
3
B
...
10
D
...
None of the answers is correct
...
Balance the equation below using the smallest set of whole numbers
...
1
B
...
3
D
...
None of the answers is correct
...
What is the coefficient of O2 when the following equation is properly balanced with the smallest set of
whole numbers?
___ CH3OH + ___ O2 → ___ CO2 + ___ H2O
A
...
2
C
...
7
E
...

28
...
Don't forget to count coefficients of one
...
4
B
...
7
D
...
None of the answers is correct
...
Balance the following equation using the smallest set of whole numbers, then add together the
coefficients
...
The sum of the coefficients is:
___ Cr + ___ H2SO4 → ___ Cr2(SO4)3 + ___ H2
A
...
9
C
...
13
E
...
Balance the following equation using the smallest set of whole numbers, then add together the
coefficients
...
The sum of the coefficients is:
___ Al + ___ H2SO4 → ___ Al2(SO4)3 + ___ H2
A
...
5
C
...
9
E
...
Balance the following equation using the smallest set of whole numbers, then add together the
coefficients
...
The sum of the coefficients is:
___ CH4 + ___ Cl2 → ___ CCl4 + ___ HCl
A
...
6
C
...
10
E
...
What is the average mass, in grams, of one atom of iron (NA = 6
...
6
...
1
...
9
...
55
...
55
...
What is the mass, in grams, of one arsenic atom (NA = 6
...
5
...
33
...
74
...
1
...
8
...
What is the mass of one copper atom (NA = 6
...
1
...
63
...
1 amu
D
...
66 × 10-24 g
E
...
476 × 1021 g
35
...
21 × 1020 atoms of sulfur (NA = 6
...
3
...
2
...
32
...
6
...
2
...
The mass of 1
...
022 × 1023 mol-1) is:
A
...
71 × 10-23 g
B
...
58 × 1022 g
C
...
08 g
D
...
04 × 104 g
E
...
60 × 10-2 g
37
...
85 g of ammonia (NA = 6
...

A
...
92 x 1023
B
...
73 x 10-25
C
...
24 x 1023
D
...
83 x 10-24
E
...
71 x 1023
38
...
80 × 1018 carbon atoms (NA = 6
...
1
...
6
...
7
...
1
...
12
...
What is the mass in grams of 0
...
4
...
25
...
17
...
4
...
2
...
Calculate the number of moles in 17
...

A
...
28 mol
B
...
32 mol
C
...
431 mol
D
...
305 mol
E
...
200 mol
41
...
Calculate the number of moles in 38
...

A
...
38 mol
B
...
55 mol
C
...
583 mol
D
...
282 mol
E
...
186 mol
42
...
Calculate the number of moles in 47
...

A
...
377 mol
B
...
146 mol
C
...
105 mol
D
...
4660 mol
E
...
4207 mol
43
...

Calculate the mass in grams of 3
...

A
...
06 × 10-4 g
B
...
91 × 10-2 g
C
...
85 × 10-2 g
D
...
6 g
E
...
Calculate the mass in grams of 8
...

A
...
0217 g
B
...
139 g
C
...
21 g
D
...
7 g
E
...
0 g
45
...
050 mol of C3H8O3 is:
A
...
0 × 1022 H atoms
B
...
2 × 1023 H atoms
C
...
4 × 1023 H atoms
D
...
8 × 1023 H atoms
E
...

46
...
0250 mol of P2O5?
A
...
5 g
B
...
0
...
1
...
3
...
Calculate the mass of 3
...

A
...
00 g
B
...
363 g
D
...
81 × 1024 g
E
...
3

48
...
76 mass %
Gd
...

A
...
Gd3O2
C
...
Gd4O3
E
...
Hydroxylamine nitrate contains 29
...
20 mass % H, and 66
...
Determine its
empirical formula
...
HNO
B
...
HN6O16
D
...
H2NO3
50
...
17 mass % N, 4
...
63 mass O
...
NH2O5
B
...
N3H3O3
D
...
N2H2O4
51
...
The compound contains 58
...
Determine its
empirical formula
...
BrF
B
...
Br2F3
D
...
BrF3
52
...
52 mass percent chromium
...

A
...
Cr2Si3
C
...
Cr3Si2
E
...
The empirical formula of a compound of uranium and fluorine that is composed of 67
...
4% fluorine is:
A
...
U3F4
C
...
UF6
E
...
The percent composition by mass of a compound is 76
...
8% H, and 11
...
5 g/mol
...
C10H6O
B
...
C16H28O4
D
...
C18H36O2

55
...
6% C and 14
...
Which of these
choices could be the molecular formula of this compound?
A
...
C2H4
C
...
C2H6
E
...
Terephthalic acid, used in the production of polyester fibers and films, is composed of carbon, hydrogen,
and oxygen
...
6943 g of terephthalic acid was subjected to combustion analysis it produced 1
...
226 g H2O
...
C2H3O4
B
...
C4H3O2
D
...
C2H2O
57
...

SO2(g) + 2Cl2(g) → SOCl2(g) + Cl2O(g)
If 0
...
0
...
0
...
0
...
0
...
0
...
Aluminum will react with bromine to form aluminum bromide (used as an acid catalyst in organic
synthesis)
...
43 mol of Al2Br6?
A
...
29 mol
B
...
86 mol
C
...
43 mol
D
...
62 mol
E
...
22 mol
59
...

2NH3(g) + 5F2(g) → N2F4(g) + 6HF(g)
How many moles of NH3 are needed to react completely with 13
...
34
...
27
...
6
...
5
...
2
...
How many grams of ammonia are formed when 5
...
3
...
0
...
13
...
17
...
6
...
How many grams of nitrogen are required to react with 2
...
25
...
13
...
78
...
38
...
77
...
How many grams of nitrogen are required to react with hydrogen to produce 13
...
11
...
0
...
22
...
16
...
44
...
What mass, in grams, of sodium carbonate is required for complete reaction with 8
...
28
...
14
...
4
...
7
...
400
...
How many grams of lead (II) chloride are produced when 13
...
5
...
1
...
0
...
11
...
16
...
How many grams of calcium are required to react with 7
...
8
...
34
...
4
...
3
...
17
...
How many grams of oxygen are required to react with calcium to produce 44
...
12
...
25
...
6
...
0
...
51
...
How many grams of sodium fluoride (used in water fluoridation and manufacture of insecticides) are
needed to form 485 g of sulfur tetrafluoride?
3SCl2(l) + 4NaF(s) → SF4(g) + S2Cl2(l) + 4NaCl(s)
A
...
1510 g
C
...
205 g
E
...
3 g

68
...

PH3(g) + O2(g) → P4O10(s) + H2O(g)
Calculate the mass of P4O10(s) formed when 225 g of PH3 reacts with excess oxygen
...
1880 g
B
...
g
C
...
g
D
...
56
...
Potassium chlorate (used in fireworks, flares and safety matches) forms oxygen and potassium chloride
when heated
...
4 g of potassium chlorate is heated?
A
...
99
...
10
...
6
...
4
...
Aluminum metal reacts with chlorine gas to form solid aluminum trichloride
...
214 g
B
...
321 g
D
...
643 g
71
...
It will also react with hydrogen peroxide to form
lead (II) sulfate and water
...
151 g
B
...
50
...
37
...
9
...
How many grams of Cl2 can be prepared from the reaction of 16
...
0 g of HCl
according to the following chemical equation?
MnO2 + 4HCl → MnCl2 + Cl2 + 2H2O
A
...
82 g
B
...
8 g
C
...
0 g
D
...
6 g
E
...
4 g

73
...
00 mol H2SO4 and 150 g NaCl?
A
...
30 g
B
...
5 g
C
...
150 g
E
...
Calculate the mass of FeS formed when 9
...
50 g of S
...
17
...
87
...
26
...
14
...
1
...
What is the limiting reactant when 3
...
79 g of hydrogen to produce ammonia
and how many grams of ammonia are produced?
A
...
22 g of ammonia are produced
...
Nitrogen is the limiting reactant and 2
...

C
...
15 g of ammonia are produced
...
Hydrogen is the limiting reactant and 23
...

E
...
8 g of ammonia are produced
...
What is the limiting reactant when 13
...
7 g of calcium to produce calcium
oxide and how many grams of calcium oxide are produced?
A
...
1 g of calcium oxide are produced
...
Oxygen is the limiting reactant and 24
...

C
...
1 g of calcium dioxide are produced
...
Oxygen is the limiting reactant and 48
...

E
...
6 g of calcium oxide are produced
...
What is the limiting reactant when 31
...
3 g of chlorine, and 25
...
Manganese (II) chloride is the limiting reactant and 8
...

B
...
21 g of hydrochloric acid is produced
...
Chlorine is the limiting reactant and 24
...

D
...
3 g of hydrochloric acid is produced
...
Water is the limiting reactant and 52 g of hydrochloric acid is produced
...
Aluminum reacts with oxygen to produce aluminum oxide which can be used as an adsorbent, desiccant
or catalyst for organic reactions
...
49 g of aluminum and 117
...
Identify the limiting reactant and determine the mass of the excess reactant present in the vessel
when the reaction is complete
...
Oxygen is the limiting reactant; 19
...

B
...
16 g of aluminum remain
...
Aluminum is the limiting reactant; 16
...

D
...
16 g of oxygen remain
...
Aluminum is the limiting reactant; 44
...


79
...
A mixture of 41
...

Identify the limiting reactant and determine the mass of the excess reactant present in the vessel when the
reaction is complete
...
Limiting reactant is Mg; 67 g of FeCl3 remain
...
Limiting reactant is Mg; 134 g of FeCl3 remain
...
Limiting reactant is Mg; 104 g of FeCl3 remain
...
Limiting reactant is FeCl3; 2 g of Mg remain
...
Limiting reactant is FeCl3; 87 g of Mg remain
...
Potassium chloride is used as a substitute for sodium chloride for individuals with high blood pressure
...
00 g of
chlorine gas reacts with 5
...

A
...
47 g of chlorine remain
...
Potassium is the limiting reactant; 7
...

C
...
64 g of potassium remain
...
Chlorine is the limiting reactant; 2
...

E
...

81
...
If a mixture of 75
...
7 g of oxygen produce 43
...
57
...
48
...
38
...
32
...
16
...
What is the percent yield for the reaction
PCl3(g) + Cl2(g) → PCl5(g)
if 119
...
3 g of Cl2 react with excess PCl3?
A
...
85
...
66
...
51
...
43
...
Methanol (CH4O) is converted to bromomethane (CH3Br) as follows:
CH4O + HBr → CH3Br + H2O
If 12
...
00 g of methanol is reacted with excess HBr, what is
the percentage yield?
A
...
9%
B
...
6%
C
...
%
D
...
245%

84
...
If the reaction of 150
...
g of oxygen gas
yields 87
...
100%
B
...
77%
D
...
62%
85
...

2Na5(CO3)2(HCO3)·2H2O(s) → 5Na2CO3(s) + CO2(g) + 3H2O(g)
When 1
...
74 metric ton of Na2CO3 is recovered
...
93%
B
...
22%
D
...
17%
86
...
0 g of Cr2O3 with
8
...
7
...
15
...
27
...
30
...
49
...
Calculate the mass of excess reagent remaining at the end of the reaction in which 90
...
0 g of O2
...
11
...
22
...
67
...
77
...
400 g
88
...
0 g of H2 and 80
...
28
...
48
...
56
...
90
...
97
...
How many grams of water could be made from 5
...
0 mol O2?
A
...
36 g
C
...
45 g
E
...
Ammonia reacts with diatomic oxygen to form nitric oxide and water vapor:
4NH3 + 5O2 → 4NO + 6H2O
What is the theoretical yield of water, in moles, when 40
...
0 g O2 are mixed and allowed to
react?
A
...
30 mol
B
...
57 mol
C
...
87 mol
D
...
53 mol
E
...
87 mol
91
...
0 mole of
V2O5 with 6
...
1
...
1
...
2
...
2
...
4
...
What is the theoretical yield of vanadium, in moles, that can be produced by the reaction of 1
...
0 mole of calcium based on the following chemical equation?
V2O5(s) + 5Ca(l) → 2V(l) + 5CaO(s)
A
...
0 mol
B
...
6 mol
C
...
0 mol
D
...
80 mol
E
...
2 mol
93
...
0g of V2O5 with
40
...
11
...
5
...
22
...
40
...
20
...
How many grams of Cr can be produced by the reaction of 44
...
0 g of Al according
to the following chemical equation?
2Al + Cr2O3 → Al2O3 + 2Cr
A
...
56 g
B
...
2 g
C
...
4 g
D
...
60
...
What is the theoretical yield of aluminum that can be produced by the reaction of 60
...
0 g of carbon according to the following chemical equation?
Al2O3 + 3C → 2Al + 3CO
A
...
0 g
B
...
9 g
C
...
2 g
D
...
0 g
E
...
81 g

96
...
What mass of carbon dioxide will be produced in this engine when 15
...
0 g of oxygen gas?
A
...
g
B
...
g
C
...
54
...
43
...
One mole of oxygen has a mass of 16
...

True False
98
...

True False
99
...

True False
100
...

True False
101
...

True False
102
...
A heterogeneous mixture of 2 or more substances
B
...
May be gaseous, solid, or liquid
D
...
A homogeneous mixture of 2 or more substances that may be gaseous, solid, or liquid
103
...
salute
B
...
solvent
D
...
solute
104
...
salute
B
...
solvent
D
...
solute
105
...
contain molecules
...
conduct electricity
...
react with other solutions
...
always contain acids
...
conduct heat
...
What accurately characterizes all nonelectrolyte solutions?
A
...
conduct electricity
C
...
do not conduct electricity
E
...
Which process defines how ionic compounds break apart into their constituent ions upon dissolution?
A
...
dissociation
C
...
dissolution
E
...
Which process defines how molecular compounds form ions upon dissolution?
A
...
composition
C
...
dissolution
E
...
Which of these compounds is a strong electrolyte?
A
...
O2
C
...
C6H12O6 (glucose)
E
...
Which of these compounds is a strong electrolyte?
A
...
N2
C
...
C2H6O (ethanol)
E
...
Which of these compounds is a weak electrolyte?
A
...
CH3COOH (acetic acid)
C
...
O2
E
...
Which of these compounds is a weak electrolyte?
A
...
NH3
C
...
N2
E
...
Which of these compounds is a nonelectrolyte?
A
...
HNO3
C
...
NaOH
E
...
Which of these compounds is a nonelectrolyte?
A
...
HNO3
C
...
KF
E
...
Which one of the following substances is the best electrolyte?
A
...
CH3Cl
C
...
C2H5OH
E
...
The distinguishing characteristic of all nonelectrolyte solutions is that they
A
...

B
...

C
...

D
...

E
...

117
...
NaCl
B
...
FeCl2
D
...
ZnCl2
118
...
Na2SO4
B
...
CuSO4
D
...
Rb2SO4
119
...
Hg2Cl2
B
...
Ag2CO3
D
...
BaSO4
120
...
AgBr
B
...
Ag2CO3
D
...
Ag2S
121
...
CaSO4
B
...
PbSO4
D
...
AgC

122
...
CuCl2 will precipitate; Ba2+ and SO42- are spectator ions
...
CuSO4 will precipitate; Ba2+ and Cl- are spectator ions
...
BaSO4 will precipitate; Cu2+ and Cl- are spectator ions
...
BaCl2 will precipitate; Cu2+ and SO42- are spectator ions
...
No precipitate will form
...
Based on the solubility rules, which of these processes will occur when solutions of ZnSO4(aq) and
MgCl2(aq) are mixed?
A
...

B
...

C
...

D
...

E
...

124
...
Pb2+(aq), Cl-(aq)
B
...
Pb2+(aq), NO3-(aq)
D
...
There are no spectator ions
...
Select the precipitate that forms when the following reactants are mixed
...
Ba2CO3
B
...
NaCl
D
...
BaO
126
...

Mg(CH3COO)2(aq) + LiOH(aq) →
A
...
Li(CH3COO)2
C
...
Mg(OH)2
E
...
Select the precipitate that forms when aqueous ammonium sulfide reacts with aqueous copper (II)
nitrate
...
CuS
B
...
NH4NO3
D
...
CuSO4
128
...

A
...
Na2NO3
C
...
Pb2SO4
E
...
Select the net ionic equation for the reaction between sodium chloride and mercury (I) nitrate
...
Na+(aq) + NO -(aq) → NaNO (aq)
3

3

B
...
NaCl(aq) → Na+(aq) + Cl-(aq)
D
...
Hg 2+(aq) → Hg (s)
2
2
130
...

Ba(OH)2(aq) + HNO3(aq) →
A
...
Ba(NO3)2(aq) + H2O(l)
C
...
Ba2O(s) + NO2(g) + H2O(l)
E
...

131
...
Pb(NO ) (aq) + 2NH Cl(aq) → NH NO (aq) + PbCl (s)
3 2

4

4

3

2

B
...
Pb2+(aq) + 2NO - (aq) + 2NH + (aq) + 2Cl-(aq) → 2NH + (aq) + 2NO - (aq) + PbCl (s)
3
4
4
3
2
D
...
No reaction occurs when the solutions are mixed
...
The common constituent in all acid solutions is:
A
...
H+
C
...
H2SO4
E
...
Identify the major ions present in an aqueous LiOH solution
...
Li2+, O-, HB
...
LiO-, H+
D
...
Li-, OH+
134
...

A
...
OH-, NO3C
...
H+, N3-, O2E
...
What is the correct formula of the salt formed in the neutralization reaction of hydrochloric acid with
calcium hydroxide?
A
...
CaCl
C
...
CaCl2
E
...
What is the chemical formula of the salt produced by the neutralization of hydrobromic acid with
magnesium hydroxide?
A
...
Mg2Br3
C
...
Mg3Br2
E
...
What is the chemical formula of the salt produced by the neutralization of nitric acid with calcium
hydroxide?
A
...
Ca2(NO3)3
C
...
Ca2NO3
E
...
What is the chemical formula of the salt produced by the neutralization of sodium hydroxide with sulfuric
acid?
A
...
Na2(SO4)3
C
...
NaSO3
E
...
What is the chemical formula of the salt produced by the neutralization of potassium hydroxide with
sulfuric acid?
A
...
K2(SO4)3
C
...
K(SO4)2
E
...
Which of the following is a weak acid?
A
...
HNO3
C
...
HBr
E
...
Which of the following is a strong acid?
A
...
HNO3
C
...
CH3COOH
E
...
Which of the following is a strong base?
A
...
Ca(OH)2
C
...
B(OH)3
E
...
Which of the following is a weak base?
A
...
Ca(OH)2
C
...
NaOH
E
...
Complete the following reaction and identify the Bronsted acid:
NaOH(aq) + HCl(aq) →
A
...
NaCl(aq) + OH-(aq); HCl is the acid
C
...
H2O(l) + NaCl(aq); HCl is the acid
E
...
Complete the following reaction and identify the Bronsted base:
NaOH(aq) + HCl(aq) →
A
...
NaCl(aq) + OH-(aq); HCl is the base
C
...
H2O(l) + NaCl(aq); HCl is the base
E
...
Select the net ionic equation for the reaction between lithium hydroxide and hydrobromic acid:
LiOH(aq) + HBr(aq) → H2O(l) + LiBr(aq)
A
...
HBr(aq) → H+(aq) + Br-(aq)
C
...
Li+(aq) + Br-(aq) → LiBr(aq)
E
...
Which of the following is oxidized in the following reaction?
Fe + Ag2O → FeO + 2Ag
A
...
Ag2O
C
...
FeO
E
...
Which of the following is reduced in the following reaction?
Cu(NO3)2 + Zn → Zn(NO3)2 + Cu
A
...
N
C
...
Zn
E
...
Which of the following is the oxidizing agent in the following reaction?
5Fe2+(aq) + MnO4-(aq) + 8H+(aq) → 5Fe3+(aq) + Mn2+(aq) + 4H2O(l)
...
Fe2+
B
...
H+
D
...
Fe3+

150
...

A
...
NiO2
C
...
Mg(OH)2
E
...
What is the oxidation number for oxygen in KMnO4?
A
...
-8
C
...
-2
E
...
What is the oxidation number for sulfur in sulfuric acid?
A
...
+6
C
...
-4
E
...
What is the oxidation number for N in K3Fe(CN)6
A
...
-3
C
...
-5
E
...
The oxidation number of Cr in Cr2O72- is:
A
...
-7
C
...
+6
E
...
Select the compound in which sulfur has its highest possible oxidation number
...
H2S
B
...
SCl2
D
...
Na2SO4
156
...
+1
B
...
-2
D
...
-1
157
...
+4
B
...
-2
D
...
0

158
...

A
...
0
C
...
+7
E
...
Which one of these equations describes a redox reaction?
A
...
2KBr(aq) + Pb(NO ) (aq) → 2KNO (aq) + PbBr (s)
3 2
3
2
C
...
H+(aq) + OH- (aq) → H O(l)
2
E
...
Which one of the following is not a redox reaction?
A
...
Zn(s) + H SO (aq) → ZnSO (aq) + H (g)
2
4
4
2
C
...
6FeSO (aq) + K Cr O (aq) + 7H SO (aq) →
4
2 2 7
2
4
Cr2(SO4)3(aq) + 3Fe2(SO4)3(aq) + K2SO4(aq) + 7H2O(l)
E
...
Which of these equations does not represent an oxidation-reduction reaction?
A
...
2H O → 2H + O
2
2
2
C
...
2NaI + Br → 2NaBr + I
2

2

E
...
In the chemical reaction 5H O + 2MnO - + 6H+ → 2Mn2+ + 8H O + 5O , the oxidizing agent is:
2 2
4
2
2
A
...
MnO4C
...
Mn2+
E
...
Identify the oxidizing agent in the chemical reaction
2MnO4- + 5H2SO3 → 2Mn2+ + 5SO42- + 4H+ + 3H2O
...
MnO4B
...
Mn2+
D
...
H+
164
...

A
...
MnO4C
...
Mn2+
E
...
Identify the reducing agent in the chemical reaction
Cd + NiO2 + 2H2O → Cd(OH)2 + Ni(OH)2
...
Cd
B
...
H2O
D
...
Ni(OH)2
166
...
H
B
...
O
D
...
This is not a redox reaction
...
What element is reduced in the chemical reaction
Cu + 2H2SO4 → CuSO4 + SO2 + 2H2O?
A
...
H
C
...
O
E
...
Identify all the spectator ions in the following reaction
...
only K+
B
...
only K+ and SO42D
...
only K+, SO42-, Fe2+ and Mn2+
169
...
2C H (g) + 7O (g) → 4CO (g) + 6H O(l)
2 6

2

2

2

B
...
2H O (aq) → 2H O(l) + O (g)
2 2

2

2

D
...
2Al(s) + 3H SO (aq) → Al (SO ) (aq) + 3H (g)
2
4
2
4 3
2
170
...
2NaN (s) → 2Na(s) + 3N (g)
3

2

B
...
3NO (g) + H O(l) → 2HNO (aq) + NO(g)
2

2

3

D
...
2ZnS(s) + 3O (g) → 2ZnO(s) + 2SO (g)
2
2

171
...
2KBr(aq) + Cl (g) → 2KCl(aq) + Br (l)
2

2

B
...
CaBr (aq) + H SO (aq) → CaSO (s) + 2HBr(g)
2

2

4

4

D
...
2LiOH(aq) + H SO (aq) → Li SO (aq) + 2H O(l)
2
4
2
4
2
172
...
2H (g) + O (g) → 2H O(l)
2

2

2

B
...
2KNO (s) → 2KNO (s) + O (g)
3

2

2

D
...
2Al(s) + 3H SO (aq) → Al (SO ) (aq) + 3H (g)
2
4
2
4 3
2
173
...
2Al(s) + 3H SO (aq) → Al (SO ) (aq) + 3H (g)
2

4

2

4 3

2

B
...
LiOH(aq) + HNO (aq) → LiNO (aq) + H O(l)
3
3
2
D
...
CaBr (aq) + H SO (aq) → CaSO (s) + 2HBr(g)
2
2
4
4
174
...
2C H (g) + 7O (g) → 4CO (g) + 6H O(l)
2 6

2

2

2

B
...
N (g) + 3H (g) → 2NH (g)
2

2

3

D
...
2Al(s) + 3H SO (aq) → Al (SO ) (aq) + 3H (g)
2
4
2
4 3
2
175
...
2C H (g) + 7O (g) → 4CO (g) + 6H O(l)
2 6

2

2

2

B
...
N (g) + 3H (g) → 2NH (g)
2

2

3

D
...
2Al(s) + 3H SO (aq) → Al (SO ) (aq) + 3H (g)
2
4
2
4 3
2
176
...
mL of a solution having a lithium ion
concentration of 0
...
6
...
10
...
19
...
30
...
2
...
A 50
...
436 M NH4NO3 is diluted with water to a total volume of 250
...
What is the
ammonium nitrate concentration in the resulting solution?
A
...
8 M
B
...
459 M
C
...
18 × 10-2 M
D
...
72 × 10-2 M
E
...
109 M
178
...
682 g sample of KClO3 is dissolved in enough water to give 375
...
What is the
chlorate ion concentration in this solution?
A
...
00 × 10-2 M
B
...
41 × 10-2 M
C
...
118 M
D
...
65 × 10-2 M
E
...
01 × 10-2 M
179
...
691 g sample of MgCl2 is dissolved in enough water to give 750
...
What is the
magnesium ion concentration in this solution?
A
...
70 × 10-2 M
B
...
05 × 10-2 M
C
...
57 × 10-2 M
D
...
93 × 10-2 M
E
...
131 M
180
...
0 mL of 0
...
0 mL of 0
...
What is the concentration of
nitrate ion in the final solution?
A
...
481 M
B
...
296 M
C
...
854 M
D
...
10 M
E
...
0295 M
181
...
0 mL of 0
...
mL of a solution of PbI2, a precipitate of PbSO4
forms
...
If the recovered PbSO4 is found
to have a mass of 0
...
3
...
1
...
6
...
3
...
1
...
How many moles of H+(aq) ions are present in 750 mL of 0
...
1
...
0
...
0
...
0
...
0
...
How many sodium ions are present in 325 mL of 0
...
1
...
3
...
4
...
6
...
1
...
A standard solution of 0
...
If 46
...
00 mL of the acid, what is the molar
concentration of the acid?
A
...
0524 M
B
...
888 M
C
...
13 M
D
...
26 M
E
...
43 M
185
...
0 M H2SO4 as an electrolyte
...
20 M NaOH will be needed to
neutralize 225 mL of battery acid?
H2SO4(aq) + 2NaOH(aq) → 2H2O(l) + Na2SO4(aq)
A
...
045 L
B
...
28 L
C
...
56 L
D
...
90 L
E
...
1 L
186
...
A 5
...
10 mL of 0
...
What is the percent by weight of acetic acid in the vinegar?
A
...
184%
B
...
63%
C
...
26%
D
...
43%
E
...
23%
187
...
mL sample of 0
...
0120 M Ca(OH)2
...

A
...
210 M
B
...
00632 M
C
...
203 M
D
...
0240 M
E
...
197 M
188
...
mL sample of 0
...
mL of 0
...
Find the concentration of hydrochloric acid in the resulting solution
...
0
...
0
...
0
...
0
...
0
...
Zinc dissolves in hydrochloric acid to yield hydrogen gas: Zn(s) + 2HCl(aq) → ZnCl (aq) + H (g) What
2
2
mass of hydrogen gas is produced when a 7
...
mL of 1
...
0
...
0
...
0
...
0
...
0
...
A 34
...
1510 M NaOH was needed to neutralize 50
...
What is the
concentration of the original sulfuric acid solution?
A
...
0229 M
B
...
218 M
C
...
0523 M
D
...
209 M
E
...
105 M

191
...
cm3
...
32
...
22
...
11
...
16
...
8
...
An electrolyte is a substance that dissolves in water to yield a solution that conducts electricity
...
Ammonium carbonate is not water soluble
...
Sodium hydroxide is water soluble
...
H3PO4 is a strong acid
...
The oxidation number for oxygen is zero
...
The following reaction will occur Na(s) + AgCl(aq) → Ag(s) + NaCl(aq)
...


Calcium fluoride, CaF2, is a source of fluorine and is used to fluoridate drinking water
...

A
...
15 g/mol
B
...
15 g/mol
C
...
07 g/mol
D
...
08 g/mol
E
...
01 g/mol

2
...

A
...
73 g/mol
B
...
89 g/mol
C
...
97 g/mol
D
...
88 g/mol
E
...
97 g/mol

3
...

A
...
43 g/mol
B
...
00 g/mol
C
...
94 g/mol
D
...
47 g/mol
E
...
48 g/mol

4
...

A
...
80 g/mol
B
...
03 g/mol
C
...
02 g/mol
D
...
96 g/mol
E
...
96 g/mol

5
...
Calculate its molecular or formula mass
...
450
...
342
...
315
...
278
...
74
...


Calculate the molar mass of Ca(BO2)2·6H2O
...
273
...
233
...
183
...
174
...
143
...
#1

Burdge - 003 Chapter
...
#3

Burdge - 003 Chapter
...
#5

Burdge - 003 Chapter
...


Calculate the molecular mass of potassium permanganate, KMnO4
...
52 g/mol
B
...
110 g/mol
D
...
176 g/mol

8
...

A
...
140 g/mol
C
...
146 g/mol
E
...


What is the molecular mass of acetaminophen, C8H9NO2?
A
...
76 g/mol
C
...
162 g/mol
E
...


What is the molar mass of nicotine, C10H14N2?
A
...
148 g/mol
C
...
210 g/mol
E
...


Household sugar, sucrose, has the molecular formula C12H22O11
...
26
...
33
...
41
...
42
...
52
...


What is the percent carbon in CH3CH2OH?
A
...
24%
C
...
46%
E
...


What is the percent sodium in sodium carbonate?
A
...
4%
B
...
3%
C
...
3%
D
...
7%
E
...
#7

Burdge - 003 Chapter
...
#9

Burdge - 003 Chapter
...
#11

Burdge - 003 Chapter
...
#13

14
...
28%
B
...
24%
D
...
42%

15
...
#14

B2O3(s) + HF(l) → BF3(g) + H2O(l)
A
...
B O (s) + H F (l) → B F (g) + H O (l)
2 3

6 6

2 6

6 3

C
...
B O (s) + 3HF(l) → 2BF (g) + 3H O(l)
2 3

3

2

E
...
#15

16
...
UO (s) + 2HF(l) → UF (s) + H O(l)
2

4

2

B
...
UO (s) + H F (l) → UF (s) + H O (l)
2

4 4

4

4 2

D
...
UO (s) + 8HF(l) → 2UF (s) + 4H O(l)
2
4
2
Burdge - 003 Chapter
...


Balance the following equation for the combustion of benzene:
C6H6(l) + O2(g) → H2O(g) + CO2(g)
A
...
C H (l) + 9O (g) → 6H O(g) + 6CO (g)
6 6

2

2

2

C
...
C H (l) + 15O (g) → 3H O(g) + 6CO (g)
6 6

2

2

2

E
...
#17

18
...
C H O (l) + 8O (g) → 9H O(g) + 8CO (g)
8 18 3
2
2
2
B
...
2C H O (l) + 22O (g) → 9H O(g) + 16CO (g
8 18 3
2
2
2
D
...
2C H O (l) + 17O (g) → 18H O(g) + 16CO (g)
8 18 3
2
2
2
Burdge - 003 Chapter
...


Balance the following equation:
Ca3(PO4)2(s) + SiO2(s) + C(s) → CaSiO3(s) + CO(g) + P4(s)
A
...
Ca (PO ) (s) + 3SiO (s) + 14C(s) → 3CaSiO (s) + 14CO(g) + P (s)
3

4 2

2

3

4

C
...
2Ca (PO ) (s) + 6SiO (s) + 10C(s) → 6CaSiO (s) + 10CO(g) + P (s)
3
4 2
2
3
4
E
...
#19

20
...
1
B
...
3
D
...
5
Burdge - 003 Chapter
...


What is the coefficient of H2O when the following equation is properly balanced with smallest set of
whole numbers?
___ Al4C3 + ___ H2O → ___ Al(OH)3 + ___ CH4
A
...
4
C
...
12
E
...
#21

22
...
1
B
...
3
D
...
6
Burdge - 003 Chapter
...


When a chemical equation is balanced, it will have a set of whole number coefficients that cannot be
reduced to smaller whole numbers
...
42
B
...
11
D
...
None of the answers is correct
...
#23

24
...
1
B
...
9
D
...
27
Burdge - 003 Chapter
...


What is the coefficient of H2SO4 when the following equation is properly balanced with the smallest
set of whole numbers?
___ Ca3(PO4)2 + ___ H2SO4 → ___ CaSO4 + ___ H3PO4
A
...
8
C
...
11
E
...

Burdge - 003 Chapter
...


Balance the equation below using the smallest set of whole numbers
...
1
B
...
3
D
...
None of the answers is correct
...
#26

27
...
1
B
...
3
D
...
None of the answers is correct
...
#27

28
...
Don't forget to count coefficients of one
...
4
B
...
7
D
...
None of the answers is correct
...
#28

29
...
Don't forget to count coefficients of one
...
4
B
...
11
D
...
15
Burdge - 003 Chapter
...


Balance the following equation using the smallest set of whole numbers, then add together the
coefficients
...
The sum of the coefficients is:
___ Al + ___ H2SO4 → ___ Al2(SO4)3 + ___ H2
A
...
5
C
...
9
E
...
#30

31
...
Don't forget to count coefficients of one
...
4
B
...
8
D
...
12
Burdge - 003 Chapter
...


What is the average mass, in grams, of one atom of iron (NA = 6
...
6
...
1
...
9
...
55
...
55
...


What is the mass, in grams, of one arsenic atom (NA = 6
...
5
...
33
...
74
...
1
...
8
...


What is the mass of one copper atom (NA = 6
...
1
...
63
...
1 amu
D
...
66 × 10-24 g
E
...
476 × 1021 g

35
...
21 × 1020 atoms of sulfur (NA = 6
...
3
...
2
...
32
...
6
...
2
...


The mass of 1
...
022 × 1023 mol-1) is:
A
...
71 × 10-23 g
B
...
58 × 1022 g
C
...
08 g
D
...
04 × 104 g
E
...
60 × 10-2 g

Burdge - 003 Chapter
...
#33

Burdge - 003 Chapter
...
#35

Burdge - 003 Chapter
...


Determine the number of ammonia molecules in 4
...
022 × 1023 mol-1)
...
2
...
4
...
1
...
5
...
1
...


What is the mass of 7
...
022 × 1023 mol-1)?
A
...
30 × 10 -5 g
B
...
43 × 103 g
C
...
80 × 1018 g
D
...
56 × 10 -4 g
E
...
01 g

39
...
250 mol of the common antacid calcium carbonate?
A
...
00 × 102 g
B
...
0 g
C
...
0 g
D
...
00 × 10-2 g
E
...
50 × 10-3 g

40
...
8 g of the antacid magnesium hydroxide, Mg(OH)2
...
3
...
2
...
0
...
0
...
0
...


Phosphorus pentachloride, a white solid that has a pungent, unpleasant odor, is used as a catalyst for
certain organic reactions
...
7 g of phosphorus pentachloride
...
5
...
3
...
0
...
0
...
0
...


Aluminum oxide, Al2O3, is used as a filler for paints and varnishes as well as in the manufacture of
electrical insulators
...
51 g of Al2O3
...
2
...
2
...
1
...
0
...
0
...


Sulfur trioxide can react with atmospheric water vapor to form sulfuric acid that falls as acid rain
...
65 × 1020 molecules of sulfur trioxide
...
6
...
2
...
4
...
20
...
1650 g

Burdge - 003 Chapter
...
#38

Burdge - 003 Chapter
...
#40

Burdge - 003 Chapter
...
#42

Burdge - 003 Chapter
...


Calculate the mass in grams of 8
...

A
...
0217 g
B
...
139 g
C
...
21 g
D
...
7 g
E
...
0 g

45
...
050 mol of C3H8O3 is:
A
...
0 × 1022 H atoms
B
...
2 × 1023 H atoms
C
...
4 × 1023 H atoms
D
...
8 × 1023 H atoms
E
...


46
...
0250 mol of P2O5?
A
...
5 g
B
...
0
...
1
...
3
...


Calculate the mass of 3
...

A
...
00 g
B
...
363 g
D
...
81 × 1024 g
E
...
3

48
...
76
mass % Gd
...

A
...
Gd3O2
C
...
Gd4O3
E
...


Hydroxylamine nitrate contains 29
...
20 mass % H, and 66
...
Determine its
empirical formula
...
HNO
B
...
HN6O16
D
...
H2NO3

50
...
17 mass % N, 4
...
63 mass O
...
NH2O5
B
...
N3H3O3
D
...
N2H2O4

Burdge - 003 Chapter
...
#45

Burdge - 003 Chapter
...
#47

Burdge - 003 Chapter
...
#49

Burdge - 003 Chapter
...


A compound of bromine and fluorine is used to make UF6, which is an important chemical in
processing and reprocessing of nuclear fuel
...
37 mass percent bromine
...

A
...
BrF2
C
...
Br3F
E
...


A compound containing chromium and silicon contains 73
...
Determine its
empirical formula
...
CrSi3
B
...
Cr3Si
D
...
Cr2S

53
...
6% uranium
and 32
...
U2F
B
...
UF4
D
...
UF8

54
...
0% C, 12
...
2% O The molar mass
of this compound is 284
...
What is the molecular formula of the compound?
A
...
C9H18O
C
...
C20H12O2
E
...


A compound was discovered whose composition by mass is 85
...
4% H
...
CH4
B
...
C3H4
D
...
C3H8

56
...
When 0
...
471 g CO2 and 0
...
What is its empirical formula?
A
...
C3H4O2
C
...
C5H12O4
E
...
#51

Burdge - 003 Chapter
...
#53

Burdge - 003 Chapter
...
#55

Burdge - 003 Chapter
...


Sulfur dioxide reacts with chlorine to produce thionyl chloride (used as a drying agent for inorganic
halides) and dichlorine oxide (used as a bleach for wood pulp and textiles)
...
400 mol of Cl2 reacts with excess SO2, how many moles of Cl2O are formed?
A
...
800 mol
B
...
400 mol
C
...
200 mol
D
...
100 mol
E
...
0500 mol
Burdge - 003 Chapter
...


Aluminum will react with bromine to form aluminum bromide (used as an acid catalyst in organic
synthesis)
...
43 mol of Al2Br6?
A
...
29 mol
B
...
86 mol
C
...
43 mol
D
...
62 mol
E
...
22 mol
Burdge - 003 Chapter
...


Ammonia will react with fluorine to produce dinitrogen tetrafluoride and hydrogen fluoride (used in
production of aluminum, in uranium processing, and in frosting of light bulbs)
...
6 mol of F2?
A
...
0 mol
B
...
2 mol
C
...
80 mol
D
...
44 mol
E
...
27 mol
Burdge - 003 Chapter
...


How many grams of ammonia are formed when 5
...
3
...
0
...
13
...
17
...
6
...


How many grams of nitrogen are required to react with 2
...
25
...
13
...
78
...
38
...
77
...
#60

Burdge - 003 Chapter
...


How many grams of nitrogen are required to react with hydrogen to produce 13
...
11
...
0
...
22
...
16
...
44
...


What mass, in grams, of sodium carbonate is required for complete reaction with 8
...
28
...
14
...
4
...
7
...
400
...


How many grams of lead (II) chloride are produced when 13
...
5
...
1
...
0
...
11
...
16
...


How many grams of calcium are required to react with 7
...
8
...
34
...
4
...
3
...
17
...


How many grams of oxygen are required to react with calcium to produce 44
...
12
...
25
...
6
...
0
...
51
...


How many grams of sodium fluoride (used in water fluoridation and manufacture of insecticides) are
needed to form 485 g of sulfur tetrafluoride?

Burdge - 003 Chapter
...
#63

Burdge - 003 Chapter
...
#65

Burdge - 003 Chapter
...
1940 g
B
...
754 g
D
...
51
...
#67

68
...

PH3(g) + O2(g) → P4O10(s) + H2O(g)
Calculate the mass of P4O10(s) formed when 225 g of PH3 reacts with excess oxygen
...
1880 g
B
...
g
C
...
g
D
...
56
...
#68

69
...

KClO3(s) → KCl(s) + O2(g)
How many grams of oxygen are formed when 26
...
223 g
B
...
1 g
C
...
3 g
D
...
86 g
E
...
60 g
Burdge - 003 Chapter
...


Aluminum metal reacts with chlorine gas to form solid aluminum trichloride
...
214 g
B
...
321 g
D
...
643 g

71
...
It will also react with hydrogen peroxide
to form lead (II) sulfate and water
...
151 g
B
...
50
...
37
...
9
...


How many grams of Cl2 can be prepared from the reaction of 16
...
0 g of HCl
according to the following chemical equation?

Burdge - 003 Chapter
...
#71

MnO2 + 4HCl → MnCl2 + Cl2 + 2H2O
A
...
82 g
B
...
8 g
C
...
0 g
D
...
6 g
E
...
4 g
Burdge - 003 Chapter
...


Hydrochloric acid can be prepared by the following reaction:
2NaCl(s) + H2SO4(aq) → 2HCl(g) + Na2SO4(s)
How many grams of HCl can be prepared from 2
...
7
...
93
...
146 g
D
...
196 g
Burdge - 003 Chapter
...


Calculate the mass of FeS formed when 9
...
50 g of S
...
17
...
87
...
26
...
14
...
1
...
#74

75
...
41 g of nitrogen react with 2
...
Hydrogen is the limiting reactant and 0
...

B
...
07 g of ammonia are produced
...
Nitrogen is the limiting reactant and 4
...

D
...
5 g of ammonia are produced
...
Hydrogen is the limiting reactant and 15
...


76
...
9 g of oxygen react with 33
...
Calcium is the limiting reactant and 47
...

B
...
4 g of calcium oxide are produced
...
Calcium is the limiting reactant and 47
...

D
...
7 g of calcium oxide are produced
...
Calcium is the limiting reactant and 23
...


77
...
3 g of manganese (II) chloride, 48
...
7 g of
water react to produce manganese (IV) oxide and how much hydrochloric acid is produced?
A
...
40 g of hydrochloric acid is produced
...
Chlorine is the limiting reactant and 6
...

C
...
8 g of hydrochloric acid is produced
...
Manganese (II) chloride is the limiting reactant and 36
...

E
...


78
...
A mixture of 82
...
65 g of oxygen
is allowed to react
...

A
...
81 g of aluminum remain
...
Oxygen is the limiting reactant; 35
...

C
...
70 g of oxygen remain
...
Aluminum is the limiting reactant; 35
...

E
...
24 g of oxygen remain
...
#75

Burdge - 003 Chapter
...
#77

Burdge - 003 Chapter
...


Magnesium (used in the manufacture of light alloys) reacts with iron (III) chloride to form magnesium
chloride and iron
...
0 g of magnesium and 175 g of iron (III) chloride is allowed to
react
...

A
...

B
...

C
...

D
...

E
...


80
...
Identify the limiting reactant and determine the mass of the excess reactant remaining when
7
...
00 g of potassium to form potassium chloride
...
Potassium is the limiting reactant; 2
...

B
...
23 g of chlorine remain
...
Chlorine is the limiting reactant; 4
...

D
...
70 g of potassium remain
...
No limiting reagent: the reactants are present in the correct stoichiometric ratio
...


Tetraphosphorus hexaoxide is formed by the reaction of phosphorus with oxygen gas
...
3 g of phosphorus and 38
...
3 g of P4O6, what is the percent yield for the
reaction?
A
...
5%
B
...
8%
C
...
0%
D
...
4%
E
...
3%

82
...
#79

Burdge - 003 Chapter
...
#81

PCl3(g) + Cl2(g) → PCl5(g)
if 119
...
3 g of Cl2 react with excess PCl3?
A
...
85
...
66
...
51
...
43
...
#82

83
...
23 g of bromomethane are produced when 5
...
40
...
82
...
100
...
121%
E
...
#83

84
...
If the reaction of 150
...
g of oxygen
gas yields 87
...
100%
B
...
77%
D
...
62%
Burdge - 003 Chapter
...


One way of obtaining pure sodium carbonate is through the decomposition of the mineral trona,
Na5(CO3)2(HCO3)·2H2O
...
00 metric ton (1 × 103 kg) of trona is decomposed, 0
...

What is the percent yield of this reaction?
A
...
43%
C
...
83%
E
...
#85

86
...
0 g of Cr2O3
with 8
...
7
...
15
...
27
...
30
...
49
...
#86

87
...
0 g of SO2 are
mixed with 100
...

2SO2 + O2 → 2SO3
A
...
5 g
B
...
5 g
C
...
5 g
D
...
5 g
E
...
#87

88
...
0 g of H2 and 80
...
28
...
48
...
56
...
90
...
97
...
#88

89
...
0 mol H2 and 3
...
90 g
B
...
42 g
D
...
108 g

90
...
#89

4NH3 + 5O2 → 4NO + 6H2O
What is the theoretical yield of water, in moles, when 40
...
0 g O2 are mixed and
allowed to react?
A
...
30 mol
B
...
57 mol
C
...
87 mol
D
...
53 mol
E
...
87 mol
Burdge - 003 Chapter
...


What is the theoretical yield of vanadium, in moles, that can be produced by the reaction of 2
...
0 mole of calcium based on the following chemical equation?
V2O5(s) + 5Ca(l) → 2V(l) + 5CaO(s)
A
...
0 mol
B
...
6 mol
C
...
0 mol
D
...
4 mol
E
...
0 mol
Burdge - 003 Chapter
...


What is the theoretical yield of vanadium, in moles, that can be produced by the reaction of 1
...
0 mole of calcium based on the following chemical equation?
V2O5(s) + 5Ca(l) → 2V(l) + 5CaO(s)
A
...
0 mol
B
...
6 mol
C
...
0 mol
D
...
80 mol
E
...
2 mol
Burdge - 003 Chapter
...


What is the theoretical yield of vanadium that can be produced by the reaction of 40
...
0g of calcium based on the following chemical equation?
V2O5(s) + 5Ca(l) → 2V(l) + 5CaO(s)
A
...
2 g
B
...
6 g
C
...
4 g
D
...
0 g
E
...
3 g
Burdge - 003 Chapter
...


How many grams of Cr can be produced by the reaction of 44
...
0 g of Al
according to the following chemical equation?
2Al + Cr2O3 → Al2O3 + 2Cr
A
...
56 g
B
...
2 g
C
...
4 g
D
...
60
...
#94

95
...
0 g of aluminum
oxide with 30
...
30
...
7
...
101
...
45
...
31
...
#95

96
...
What mass of carbon dioxide will be produced in this engine when
15
...
0 g of oxygen gas?
A
...
g
B
...
g
C
...
54
...
43
...


One mole of oxygen has a mass of 16
...

FALSE

98
...

TRUE

99
...

FALSE

100
...

FALSE

101
...

TRUE

102
...
A heterogeneous mixture of 2 or more substances
B
...
May be gaseous, solid, or liquid
D
...
A homogeneous mixture of 2 or more substances that may be gaseous, solid, or liquid

103
...
salute
B
...
solvent
D
...
solute

Burdge - 003 Chapter
...
#97

Burdge - 003 Chapter
...
#99

Burdge - 003 Chapter
...
#101

Burdge - 004 Chapter
...
#2

104
...
salute
B
...
solvent
D
...
solute

105
...
contain molecules
...
conduct electricity
...
react with other solutions
...
always contain acids
...
conduct heat
...


What accurately characterizes all nonelectrolyte solutions?
A
...
conduct electricity
C
...
do not conduct electricity
E
...


Which process defines how ionic compounds break apart into their constituent ions upon dissolution?

Burdge - 004 Chapter
...
#4

Burdge - 004 Chapter
...

B
...

D
...


electrolysis
dissociation
division
dissolution
decomposition
Burdge - 004 Chapter
...


Which process defines how molecular compounds form ions upon dissolution?
A
...
composition
C
...
dissolution
E
...


Which of these compounds is a strong electrolyte?
A
...
O2
C
...
C6H12O6 (glucose)
E
...


Which of these compounds is a strong electrolyte?
A
...
N2
C
...
C2H6O (ethanol)
E
...
#7

Burdge - 004 Chapter
...
#9

111
...
HCl
B
...
C6H12O6 (glucose)
D
...
NaCl

112
...
HCl
B
...
C6H12O6 (glucose)
D
...
KCl

113
...
NaF
B
...
CH3COOH (acetic acid)
D
...
C6H12O6 (glucose)

114
...
NaOH
B
...
C2H6O (ethanol)
D
...
CH3COOH (acetic acid)

115
...
CO
B
...
CH4
D
...
HCl

116
...
contain ions
...
do not conduct electricity
...
react with other solutions
...
always contain acids
...
conducts heat
...


Based on the solubility rules, which one of these compounds should be insoluble in water?
A
...
MgBr2
C
...
AgBr
E
...
#10

Burdge - 004 Chapter
...
#12

Burdge - 004 Chapter
...
#14

Burdge - 004 Chapter
...
#16

118
...
Na2SO4
B
...
CuSO4
D
...
Rb2SO4

119
...
Hg2Cl2
B
...
Ag2CO3
D
...
BaSO4

120
...
AgBr
B
...
Ag2CO3
D
...
Ag2S

121
...
CaSO4
B
...
PbSO4
D
...
AgC

122
...
CuCl2 will precipitate; Ba2+ and SO42- are spectator ions
...
CuSO4 will precipitate; Ba2+ and Cl- are spectator ions
...
BaSO4 will precipitate; Cu2+ and Cl- are spectator ions
...
BaCl2 will precipitate; Cu2+ and SO42- are spectator ions
...
No precipitate will form
...


Based on the solubility rules, which of these processes will occur when solutions of ZnSO4(aq) and
MgCl2(aq) are mixed?
A
...

B
...

C
...

D
...

E
...


124
...
#17

Burdge - 004 Chapter
...
#19

Burdge - 004 Chapter
...
#21

Burdge - 004 Chapter
...
Pb2+(aq), Cl-(aq)
B
...
Pb2+(aq), NO3-(aq)
D
...
There are no spectator ions
...
#23

125
...

Na2CO3(aq) + BaCl2(aq) →
A
...
BaCO3
C
...
NaCl2
E
...
#24

126
...

Mg(CH3COO)2(aq) + LiOH(aq) →
A
...
Li(CH3COO)2
C
...
Mg(OH)2
E
...
#25

127
...

A
...
Cu2S
C
...
NH4(NO3)2
E
...


Select the precipitate that forms when aqueous lead (II) nitrate reacts with aqueous sodium sulfate
...
NaNO3
B
...
PbSO4
D
...
PbS

129
...


Burdge - 004 Chapter
...
#27

2NaCl(aq) + Hg2(NO3)2(aq) → NaNO3(aq) + Hg2Cl2(s)
A
...
Hg 2+(aq) + 2Cl-(aq) → Hg Cl (s)
2
2 2
C
...
Hg (NO ) (aq) → Hg 2+(aq) + 2NO -(aq)
2
3 2
2
3
E
...
#28

130
...

Ba(OH)2(aq) + HNO3(aq) →
A
...
Ba(NO3)2(aq) + H2O(l)
C
...
Ba2O(s) + NO2(g) + H2O(l)
E
...

Burdge - 004 Chapter
...


Which of these choices is the correct net ionic equation for the reaction that occurs when solutions of
Pb(NO3)2 and NH4Cl are mixed?
A
...
Pb2+(aq) + 2Cl-(aq) → PbCl (s)
2
C
...
NH +(aq)+ NO - (aq) → 2NH NO (s)
4

3

4

3

E
...

Burdge - 004 Chapter
...


The common constituent in all acid solutions is:
A
...
H+
C
...
H2SO4
E
...


Identify the major ions present in an aqueous LiOH solution
...
Li2+, O-, HB
...
LiO-, H+
D
...
Li-, OH+

134
...

A
...
OH-, NO3C
...
H+, N3-, O2E
...


What is the correct formula of the salt formed in the neutralization reaction of hydrochloric acid with
calcium hydroxide?
A
...
CaCl
C
...
CaCl2
E
...


What is the chemical formula of the salt produced by the neutralization of hydrobromic acid with
magnesium hydroxide?
A
...
Mg2Br3
C
...
Mg3Br2
E
...


What is the chemical formula of the salt produced by the neutralization of nitric acid with calcium
hydroxide?
A
...
Ca2(NO3)3
C
...
Ca2NO3
E
...
#31

Burdge - 004 Chapter
...
#33

Burdge - 004 Chapter
...
#35

Burdge - 004 Chapter
...


What is the chemical formula of the salt produced by the neutralization of sodium hydroxide with
sulfuric acid?
A
...
Na2(SO4)3
C
...
NaSO3
E
...


What is the chemical formula of the salt produced by the neutralization of potassium hydroxide with
sulfuric acid?
A
...
K2(SO4)3
C
...
K(SO4)2
E
...


Which of the following is a weak acid?
A
...
HNO3
C
...
HBr
E
...


Which of the following is a strong acid?
A
...
HNO3
C
...
CH3COOH
E
...


Which of the following is a strong base?
A
...
Ca(OH)2
C
...
B(OH)3
E
...


Which of the following is a weak base?
A
...
Ca(OH)2
C
...
NaOH
E
...


Complete the following reaction and identify the Bronsted acid:

Burdge - 004 Chapter
...
#38

Burdge - 004 Chapter
...
#40

Burdge - 004 Chapter
...
#42

NaOH(aq) + HCl(aq) →
A
...
NaCl(aq) + OH-(aq); HCl is the acid
C
...
H2O(l) + NaCl(aq); HCl is the acid
E
...
#43

145
...
Na(aq) + HOCl(aq); NaOH is the base
B
...
NaCl(aq) + OH-(aq); NaOH is the base
D
...
NaCl(aq) + H2O(l); NaOH is the base
Burdge - 004 Chapter
...


Select the net ionic equation for the reaction between lithium hydroxide and hydrobromic acid:
LiOH(aq) + HBr(aq) → H2O(l) + LiBr(aq)
A
...
HBr(aq) → H+(aq) + Br-(aq)
C
...
Li+(aq) + Br-(aq) → LiBr(aq)
E
...
#45

147
...
Ag
B
...
Fe
D
...
2Ag
Burdge - 004 Chapter
...


Which of the following is reduced in the following reaction?
Cu(NO3)2 + Zn → Zn(NO3)2 + Cu
A
...

C
...

E
...
#47

149
...

A
...
MnO4C
...
Mn2+
E
...
#48

150
...

A
...
NiO2
C
...
Mg(OH)2
E
...
#49

151
...
+1
B
...
+5
D
...
+3

152
...
+1
B
...
-2
D
...
+4

153
...
+3
B
...
+4
D
...
+1

154
...
-12
B
...
-2
D
...
+7

155
...

A
...
SO2
C
...
H2SO3
E
...


What is the oxidation number for oxygen in hydrogen peroxide?
A
...
0
C
...
+2
E
...


The oxidation number of N in N2H4 is:
A
...
+2
C
...
-4
E
...
#50

Burdge - 004 Chapter
...
#52

Burdge - 004 Chapter
...
#54

Burdge - 004 Chapter
...
#56

158
...

A
...
0
C
...
+7
E
...


Which one of these equations describes a redox reaction?
A
...
#57

2

4

2

4 3

2

B
...
CaBr (aq) + H SO (aq) → CaSO (s) + 2HBr(g)
2

2

4

4

D
...
CO 2- (aq) + HSO -(aq) → HCO - (aq) + SO 2- (aq)
3
4
3
4
Burdge - 004 Chapter
...


Which one of the following is not a redox reaction?
A
...
Zn(s) + H SO (aq) → ZnSO (aq) + H (g)
2
4
4
2
C
...
6FeSO (aq) + K Cr O (aq) + 7H SO (aq) →
4
2 2 7
2
4
Cr2(SO4)3(aq) + 3Fe2(SO4)3(aq) + K2SO4(aq) + 7H2O(l)
E
...
#59

161
...
3Al + 6HCl → 3H + AlCl
2

3

B
...
2NaCl + Pb(NO ) → PbCl + 3NaNO
3 2
2
3
D
...
Cu(NO ) + Zn → Zn(NO ) + Cu
3 2
3 2
Burdge - 004 Chapter
...


In the chemical reaction 5H2O2 + 2MnO4 +
A
...
MnO4C
...
Mn2+
E
...


Identify the oxidizing agent in the chemical reaction

-

6H+

→

2Mn2+

+ 8H2O + 5O2, the oxidizing agent is:

Burdge - 004 Chapter
...

A
...
H2SO3
C
...
SO42E
...
#62

164
...

A
...
MnO4C
...
Mn2+
E
...
#63

165
...

A
...
NiO2
C
...
Cd(OH)2
E
...
#64

166
...
H
B
...
O
D
...
This is not a redox reaction
...
#65

167
...
Cu
B
...
S
D
...
H2O
Burdge - 004 Chapter
...


Identify all the spectator ions in the following reaction
...
only K+
B
...
only K+ and SO42D
...
only K+, SO42-, Fe2+ and Mn2+
Burdge - 004 Chapter
...


Which of these chemical equations describes a disproportionation reaction?
A
...
2KBr(aq) + Cl (g) → 2KCl(aq) + Br (l)
2
2
C
...
CaBr (aq) + H SO (aq) → CaSO (s) + 2HBr(g)
2
2
4
4
E
...
#68

170
...
2NaN (s) → 2Na(s) + 3N (g)
3

2

B
...
3NO (g) + H O(l) → 2HNO (aq) + NO(g)
2
2
3
D
...
2ZnS(s) + 3O (g) → 2ZnO(s) + 2SO (g)
2
2
Burdge - 004 Chapter
...


Which of these chemical equations describes a halogen displacement reaction?
A
...
2Na(s) + 2H O(l) → 2NaOH(aq) + H (g)
2
2
C
...
2KNO (s) → 2KNO (s) + O (g)
3
2
2
E
...
#70

172
...
2H (g) + O (g) → 2H O(l)
2

2

2

B
...
2KNO (s) → 2KNO (s) + O (g)
3

2

2

D
...
2Al(s) + 3H SO (aq) → Al (SO ) (aq) + 3H (g)
2
4
2
4 3
2
Burdge - 004 Chapter
...


Which of these chemical equations describes an acid-base neutralization reaction?
A
...
SO (g) + H O(l) → H SO (g)
2
2
2
3
C
...
2KBr(aq) + Cl (g) → 2KCl(aq) + Br (l)
2

2

E
...
#72

174
...
2C H (g) + 7O (g) → 4CO (g) + 6H O(l)
2 6

2

2

2

B
...
N (g) + 3H (g) → 2NH (g)
2

2

3

D
...
2Al(s) + 3H SO (aq) → Al (SO ) (aq) + 3H (g)
2

4

2

4 3

2

Burdge - 004 Chapter
...


Which of these chemical equations describes a combustion reaction?
A
...
LiOH(aq) + HNO (aq) → LiNO (aq) + H O(l)
3
3
2
C
...
2Na(s) + 2H O(l) → 2NaOH(aq) + H (g)
2
2
E
...
#74

176
...
mL of a solution having a lithium ion
concentration of 0
...
6
...
10
...
19
...
30
...
2
...


A 50
...
436 M NH4NO3 is diluted with water to a total volume of 250
...
What is
the ammonium nitrate concentration in the resulting solution?
A
...
8 M
B
...
459 M
C
...
18 × 10-2 M
D
...
72 × 10-2 M
E
...
109 M

178
...
682 g sample of KClO3 is dissolved in enough water to give 375
...
What is the
chlorate ion concentration in this solution?
A
...
00 × 10-2 M
B
...
41 × 10-2 M
C
...
118 M
D
...
65 × 10-2 M
E
...
01 × 10-2 M

179
...
691 g sample of MgCl2 is dissolved in enough water to give 750
...
What is the
magnesium ion concentration in this solution?
A
...
70 × 10-2 M
B
...
05 × 10-2 M
C
...
57 × 10-2 M
D
...
93 × 10-2 M
E
...
131 M

180
...
0 mL of 0
...
0 mL of 0
...
What is the concentration
of nitrate ion in the final solution?
A
...
481 M
B
...
296 M
C
...
854 M
D
...
10 M
E
...
0295 M

181
...
0 mL of 0
...
mL of a solution of PbI2, a precipitate of PbSO4
forms
...
If the recovered PbSO4 is
found to have a mass of 0
...
#75

Burdge - 004 Chapter
...
#77

Burdge - 004 Chapter
...
#79

A
...

C
...

E
...
10 × 10-4 M
1
...
20 × 10-3 M
3
...
55 × 10-3 M
Burdge - 004 Chapter
...


How many moles of H+(aq) ions are present in 750 mL of 0
...
1
...
0
...
0
...
0
...
0
...


How many sodium ions are present in 325 mL of 0
...
1
...
3
...
4
...
6
...
1
...


A standard solution of 0
...
If 46
...
00 mL of the acid, what is the molar
concentration of the acid?
A
...
0524 M
B
...
888 M
C
...
13 M
D
...
26 M
E
...
43 M

185
...
0 M H2SO4 as an electrolyte
...
20 M NaOH will be needed to
neutralize 225 mL of battery acid?

Burdge - 004 Chapter
...
#82

Burdge - 004 Chapter
...
0
...
0
...
0
...
0
...
1
...
#84

186
...
A 5
...
10 mL of 0
...
What is the percent by weight of acetic acid in the
vinegar?
A
...
184%
B
...
63%
C
...
26%
D
...
43%
E
...
23%

187
...
mL sample of 0
...
0120 M Ca(OH)2
...

A
...
210 M
B
...
00632 M
C
...
203 M
D
...
0240 M
E
...
197 M

Burdge - 004 Chapter
...
#86

188
...
mL sample of 0
...
mL of 0
...
Find the concentration of hydrochloric acid in the resulting solution
...
0
...
0
...
0
...
0
...
0
...
#87

189
...
35 g chunk of zinc dissolves in 500
...
200M
HCl?
A
...
605 g
B
...
113 g
C
...
302 g
D
...
453 g
E
...
226 g

190
...
62 mL of 0
...
0 mL of an H2SO4 solution
...
0
...
0
...
0
...
0
...
0
...


Calcium nitrate tetrahydrate dissolves in cold water to the extent of 266 g per 100
...
What is the
concentration of nitrate ions in this solution?
A
...
4 M
B
...
5 M
C
...
3 M
D
...
2 M
E
...
10 M

192
...

TRUE

193
...

FALSE

194
...

TRUE

195
...

FALSE

196
...

TRUE

Burdge - 004 Chapter
...
#89

Burdge - 004 Chapter
...
#91

Burdge - 004 Chapter
...
#93

Burdge - 004 Chapter
...
#95

197
...

TRUE
Burdge - 004 Chapter
...

Burdge - 004 Chapter

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