Transcript File

Unit 4 Practice Questions
I.
Reactions: balancing, types
Questions 1-3 refer to the following:
(A) 1
(B) 2
(C) 3
Cu + HNO3
Cu(NO3)2 + H2O + NO
(D) 4
(E) 5
1. When the above equation is balanced, what will be
the coefficient of Cu?
2. If 6 moles of Cu reacted according to the above
equation, what will be the number of moles of NO
formed?
3. If Cu(NO3)2 goes into solution as ions, what will be
the number of ions into which it will dissociate?
1
Questions 1-3 refer to the following:
(A)
(B)
(C)
(D)
(E)
H2
NH3
CO2
HCl
O2
1. A gas produced by the reaction of zinc with
hydrochloric acid
2. A gas combustion product that is heavier than air
3. A gas produced by the heating of potassium
chlorate
2
II
I
One mole of NaCl
contains 2 moles of
ions
The reaction in
which HgO is
heated to release
O2 is called
decomposition
BECAUSE
NaCl is a stable salt at room
temperature
BECAUSE
In a decomposition
reaction, the original
compound is broken
apart into equal
numbers of atoms
3
I
When a
hydrocarbon is
combusted in air,
carbon monoxide is
the major product
II
BECAUSE
A piece of zinc placed
in a blue copper
solution will displace
the copper from the
solution, producing
copper metal and a
colorless Zn2+
solution
BECAUSE
Air contains much more
nitrogen than oxygen
Copper is a much more
active metal than zinc
4
I
A wooden splint is
set on fire and blown
out, leaving a hot
glowing end. When
the glowing splint is
inserted into a
sample of purified
CO2 gas, it will
reignite into a flame
II
BECAUSE
CO2 gas contains oxygen
5
I
AgCl is insoluble in
water
Calcium phosphate is
a water-soluble
compound
II
BECAUSE
All chlorides are soluble in
water except for those of
silver, mercury and lead
BECAUSE
All group I ions form
water-soluble salts
6
The reaction of aluminum with dilute H2SO4 can be
classified as
(A)
(B)
(C)
(D)
Synthesis
Decomposition
Single replacement
Double replacement
7
What are the simplest whole-number coefficients
that balance this equation?
___C4H10 + ___O2
(A)
(B)
(C)
(D)
(E)
___CO2 + ___H2O
1,6,4,2
2,13,8,10
1,6,1,5
3,10,16,20
4,26,16,20
8
If the equation for the reaction below is balanced
using the smallest possible whole-number
coefficients, then the coefficient for oxygen gas is
___C2H4 + ___O2
(A)
(B)
(C)
(D)
(E)
___CO2 + ___H2O
1
2
3
4
5
9
When the equation below is balanced using the
lowest whole-number terms, the coefficient of CO2
is
___C4H10 + ___O2
(A)
(B)
(C)
(D)
(E)
___CO2 + ___H2O
2
4
8
10
13
10
When the equation for the reaction below is
balanced, how many moles of NF3 wold be required
to react completely with 6 moles of H2O?
___NF3 + ___H2O
(A)
(B)
(C)
(D)
(E)
___HF + ___NO + ___NO2
0.5 mole
1 mole
2 moles
3 moles
4 moles
11
Which coefficient balances the reaction given below?
2Ca3(PO4)2 + 6SiO2 + 10C
(A)
(B)
(C)
(D)
(E)
10CO + P4 + ___CaSiO3
2
4
5
6
8
12
Which of the following reactions produces a yellow
precipitate?
(A)
(B)
(C)
(D)
(E)
NaOH (s) + HCl (aq)
NaCl(aq) + H2O
2NaOH(aq) + BaCl2 (aq)
Ba(OH)2 (s) + 2NaCl (aq)
Pb(NO3)2 (aq) + 2KI (aq)
2KNO3 (aq) + PbI2 (s)
CuO(s) + Mg(s)
Cu(s) + MgO (s)
4Fe + 3O2
2Fe2O3
13
When the equation for the reaction shown below is
completed and balanced and all coefficients are
reduced to lowest whole-number terms, the
coefficient of O2 is
___Al + ___O2
(A)
(B)
(C)
(D)
(E)
___Al2O3
1
2
3
4
6
14
What is the sum of the coefficients of the following
equation when it is balanced?
___C6H12O6 + ___O2
(A)
(B)
(C)
(D)
(E)
___CO2 + ___H2O
20
38
21
19
18
15
What is the precipitate produced from the double
displacement reaction of an aqueous solution of
lead(II) nitrate and an aqueous solution of potassium
sulfate?
(A)
(B)
(C)
(D)
(E)
PbSO4
KNO3
K2Pb
NO2
SO3
16
The reaction below is classified as a
CH3CO2Na + HClO4
(A)
(B)
(C)
(D)
(E)
CH3CO2H + NaClO4
Double displacement reaction
Synthesis reaction
Decomposition reaction
Single displacement and decomposition reaction
Synthesis and decomposition reaction
17
H2 + Cl2
2HCl
The above reaction is classified as a
(A)
(B)
(C)
(D)
(E)
Decomposition
Double displacement
Neutralization
Oxidation-reduction
Single displacement
18
What is the sum of the coefficients of the products for the
following reaction, after balancing?
__K2Cr2O7 + __HCl
(A)
(B)
(C)
(D)
(E)
__KCl + __CrCl3 + __H2O + __Cl2
10
12
13
14
15
19
Which equation is correctly balanced?
(A)
(B)
(C)
(D)
(E)
Na + Cl2
2NaCl
CH4 + 3O2
CO2 + H2O
2KI + Pb(NO3)2
2KNO3 + PbI2
H2SO4 + KOH
K2SO4 + H2O
C6H12O6 + 6O2
6CO2 + H2O
20
Which of the following can be classified as a precipitation
reaction?
(A)
(B)
(C)
(D)
(E)
HCl (aq) + NaOH (aq)
KBr (aq) + NaCl (aq)
AgNO3(aq) + MgCl2(aq)
CaCl2 (aq) + KI (aq)
NaNO3 (aq) + HC2H3O2 (aq)
21
What would be the stoichiometric coefficient of
hydrochloric acid in the following equation?
___Cl2 + ___H2O
(A)
(B)
(C)
(D)
(E)
___HCl +___HClO3
1
3
5
10
12
22
When the equation
___C2H6 + ___O2
___CO2 +___H2O
Is competely balanced using the lowest whole
number coefficients, the sum of the coefficients will
be
(A)
(B)
(C)
(D)
(E)
4
9.5
19
15.5
11
23
Which reaction between ions does not form a
precipitate?
(A)
(B)
(C)
(D)
(E)
Ag1+ + Cl1Pb2+ + 2I1Ca2+ + CO32Hg2+ + 2Br1Na1+ + OH1-
24
The product formed when oxygen and hydrogen are
mixed in a test tube at room temperature is
(A)
(B)
(C)
(D)
(E)
Hydrogen peroxide
Water
A base
A zwitterion
No reaction takes place
25
If the equation for the reaction below is balanced
with whole-number coefficients, what is the
coefficient for oxygen gas?
___C2H4 + ___O2
(A)
(B)
(C)
(D)
(E)
___CO2 + ___H2O
1
2
3
4
5
26
For a metal atom to replace another kind of metallic
ion in a solution, the metal atom must be
(A) A good oxidizing agent
(B) Higher in the activity series than the metal in
solution
(C) Lower in the electromotive chart than the metal
in solution
(D) Equal in activity to the metal in solution
27
How many atoms are represented in the formula
Ca3(PO4)2?
(A)
(B)
(C)
(D)
(E)
5
8
9
12
13
28
What is the total number of atoms represented in
one molecule of (CH3)2NH?
(A)
(B)
(C)
(D)
(E)
5
8
9
10
12
29
The chemical symbol Ar could stand for
(A)
(B)
(C)
(D)
(E)
One mole of argon
One atom of argon
Both a mole or an atom of argon
Neither a mole or an atom of argon
One molecule of argon
30
Which salt has a solubility that is different from the
other four?
(A)
(B)
(C)
(D)
(E)
AgCl
PbBr2
Ca3(PO4)2
Na2CO3
Al(OH)3
31
The net ionic equation for the reaction between
CaCl2 and Na2CO3 to form calcium carbonate and
sodium chloride would include all of the following
except:
(A)
(B)
(C)
(D)
(E)
Ca2+
CO322Na1+
CaCO3
All of the substances above would be in the net
ionic equation
32
When most fuels burn, the products include carbon
dioxide and
(A)
(B)
(C)
(D)
(E)
Hydrocarbons
Hydrogen
Water
Hydroxide
Hydrogen peroxide
33
Which of the following elements normally exist as
monoatomic molecules?
(A)
(B)
(C)
(D)
(E)
Cl
H
O
N
He
34
In this equation:
Al(OH)3 + H2SO4
Al2(SO4)3 + H2O
The whole number coefficients of the balanced
equation are
(A)
(B)
(C)
(D)
1,3,1,2
2,3,2,6
2,3,1,6
1,3,1,6
35
For the reaction of sodium with water, the balanced
equation using the smallest whole numbers has
which of the following coefficients?
I. 1
II. 2
III. 3
(A)
(B)
(C)
(D)
(E)
I only
III only
I and II only
II and III only
I, II, and III
36
The reaction of zinc metal, Zn, and hydrochloric
acid, HCl, produces which of the following?
I. H2 (g)
II. Cl2 (g)
III. Zn2+ (aq)
(A)
(B)
(C)
(D)
(E)
II only
III only
I and II only
I and III only
I, II, and III
37
Which reactions would form at least one solid
precipitate as a product? Assume aqueous
reactants.
I. AgNO3 + NaCl
NaNO3 + AgCl
II. Pb(NO3)2 + 2KI
PbI2 + 2KNO3
III. 2NaOH + H2SO4
Na2SO4 + 2H2O
(A)
(B)
(C)
(D)
(E)
I only
II only
III only
I and II only
II and III only
38
Which of these equations is/are properly balanced?
I. Cl2 + NaBr
II. 2Na + O2
III. 2K + 2H2O
(A)
(B)
(C)
(D)
(E)
Br2 + 2NaCl
Na2O
H2 + 2KOH
I only
II only
III only
I and III only
I, II and III
39
One reason for a double displacement reaction to
go to completion is that
(A)
(B)
(C)
(D)
A product is soluble
A product is given off as a gas
The products can react with each other
The products are miscible
40
II. % Composition, Empirical and Molecular Formulas
I
The percent
composition of
oxygen in water is
33%
II
BECAUSE
One atom of oxygen makes
up one-third of the mass of
a water molecule
41
Laboratory results showed the composition of a
compound to be 58.81% barium, 13.73% sulfur and
27.46% oxygen. What is the empirical formula?
(A)
(B)
(C)
(D)
(E)
BaSO4
BaS2O
Ba2SO3
BaS2O4
Ba2SO4
42
What is the percent composition of oxygen in
C6H12O6 (molar mass = 180)?
(A)
(B)
(C)
(D)
(E)
25%
33%
40%
53%
75%
43
A compound was analyzed and found to be
composed of 75% carbon and 25% hydrogen. What
is the empirical formula of this compound?
(A)
(B)
(C)
(D)
(E)
C2H4
CH4
CH3
CH2
CH
44
The percent composition by mass of oxygen in
BaSO4 is
(A)
(B)
(C)
(D)
(E)
233.4%
66.7%
27.4%
58.7%
13.7%
45
Which statement is true about the percent
composition by mass in C6H12O6?
(A)
(B)
(C)
(D)
(E)
Carbon is 6.7% by mass
Oxygen is 53.3 % by mass
Hydrogen is 12% by mass
Carbon is 72% by mass
Carbon is 20% by mass
46
What is the approximate percentage composition
by mass of the element oxygen in the compound
HClO4?
(A)
(B)
(C)
(D)
(E)
16%
32%
50%
64%
75%
47
The percent composition of an unknown element X
in CH3X is 32%. Which of the following is element X?
(A)
(B)
(C)
(D)
(E)
H
F
Cl
Na
Li
48
A compound’s composition by mass is 50% S and
50% O. What is the empirical formula of this
compound?
(A)
(B)
(C)
(D)
(E)
SO
SO2
S2O
S2O3
S3O4
49
What percentage of the total mass of KHCO3 is
made up by nonmetallic elements?
(A)
(B)
(C)
(D)
(E)
17%
83%
61%
20%
50%
50
A compound has a composition of 40% sulfur and
60% oxygen by mass. What is the empirical formula
of this compound?
(A)
(B)
(C)
(D)
(E)
SO
S2O3
S2O7
SO3
SO2
51
A hydrocarbon has the empirical formula CH3. A
probable molecular formula for this compound
could be
(A)
(B)
(C)
(D)
(E)
C3H3
C2H6
C3H8
C4H8
C5H10
52
What is the percentage by mass of sulfur in H2SO4?
(A)
(B)
(C)
(D)
(E)
16%
33%
36%
42%
Cannot be determined
53
What is the percent composition by weight of Al in
Al2(SO4)3?
(A)
(B)
(C)
(D)
(E)
7.9%
31.6%
15.8%
12.7%
22.3%
54
What is the molecular formula of a compound with
the empirical formula C3H6O2 and a mass of 148
amu?
(A)
(B)
(C)
(D)
(E)
C6H12O4
C2H6O2
C9H18O6
C2H3O
None of the above
55
What is the percent by mass of silicon in a sample
of silicon dioxide?
(A)
(B)
(C)
(D)
(E)
21%
33%
47%
54%
78%
56
Which of the following could be the molecular
formula for a molecule with an empirical formula of
CH2?
(A)
(B)
(C)
(D)
(E)
CH
CH4
C2H2
C2H6
C3H6
57
Which of the following statements about molecular
and empirical formulas is/are false?
I. a given compound can have the same
molecular and empirical formula
II. The molecular formula is a whole-number
multiple of the empirical formula
III. H2O2 represents the empirical formula of
hydrogen peroxide
(A)
(B)
(C)
(D)
(E)
III only
I and II only
II and III only
I, II, and III
I only
58
What is the percentage composition of calcium in
calcium hydroxide, Ca(OH)2?
(A)
(B)
(C)
(D)
(E)
40%
43%
54%
69%
74%
59
Which of the following compounds contains the
greatest percentage of oxygen by weight?
(A)
(B)
(C)
(D)
(E)
C3H6O5Cl
C3H6O2
C5H10O5
C4H8O3
They are all equal
60
What is the mass of nitrogen in a 50.0 g sample of
sodium nitrite (NaNO2)?
(A)
(B)
(C)
(D)
(E)
20.2 g
16.4 g
10.1 g
8.23 g
23.4 g
61
In the laboratory, a sample of hydrated salt was
heated at 110oC for 30 minutes until all the water
was driven off. The data were as follows:
Mass of hydrate before heating = 250 g
Mass of hydrate after heating = 160 g
From these data, what was the percent of water by
mass in the original sample?
(A)
(B)
(C)
(D)
(E)
26.5
36
47
56
90
62
What is the approximate percentage of oxygen in
the formula mass of Ca(NO3)2?
(A)
(B)
(C)
(D)
(E)
28
42
58
68
84
63
What formulas could represent the empirical
formula and the molecular formula of a given
compound?
(A)
(B)
(C)
(D)
(E)
CH2O and C4H6O4
CHO and C6H12O6
CH4 and C5H12
CH2 and C3H6
CO and CO2
64
Analysis of a gas gave: C = 85.7% and H = 14.3%. If
the formula mass of this gas is 42, what are the
empirical formula and the true formula?
(A)
(B)
(C)
(D)
(E)
CH and C4H4
CH2 and C3H6
CH3 and C3H9
C2H2 and C3H6
C2H4 and C3H6
65
In synthesizing MgO from a Mg strip burned in a
crucible, which of the following is NOT true?
(A) The initial strip of Mg should be cleaned
(B) The lid of the crucible should fit tightly to
exclude oxygen
(C) The heating of the covered crucible should
continue until the Mg is fully reacted
(D) The crucible, lid and contents should be cooled
to room temperature before measuring their
mass
(E) When the Mg appears to be fully reacted, the
crucible lid should be partially removed and
heating continued
66
A compound whose molecular mass is 90.0 grams
contains 40.0% carbon, 6.67% hydrogen, and
53.33% oxygen. What is the true formula of the
compound?
(A)
(B)
(C)
(D)
(E)
C2H2O4
CH2O4
C3H6O
C3HO3
C3H6O3
67
If the simplest formula of a substance is CH2 and its
molecular mass is 56, what is its true formula?
(A)
(B)
(C)
(D)
(E)
CH2
C2H4
C3H4
C4H8
C5H10
68
III. Moles, Conversions and Stoichiometry
Questions 1-4 refer to the following:
(A)
(B)
(C)
(D)
(E)
9.03 x 1023 molecules
44.8 liters
3.5 moles
6.0 grams
3.01 x 1023 atoms
1.
2.
3.
4.
0.25 moles of O2 at STP
3.0 moles of H2 at STP
56 grams of N2 at STP
96.0 grams of SO2 at STP
69
II
I
Two liters of CO2
can be produced by
1 gram of carbon
burning completely
One mole of CO2
has a greater mass
than 1 mole of
H2O
BECAUSE
The amount of gas evolved
in a chemical reaction can
be determined by using the
mole relationship of the
coefficients in the balanced
equation
BECAUSE
The molecular mass of
CO2 is greater than the
molecular mass of H2O
70
II
I
There are 3 moles
of atoms in 18
grams of water
The complete
electrolysis of 45
grams of water
will yield 40 grams
of H2 and 5 grams
of O2
BECAUSE
There are 6 x 1023 atoms in
1 mole
BECAUSE
Water is composed of
hydrogen and oxygen in
a ratio of 8:1 by mass
71
I
II
BECAUSE
When 2 liters of
oxygen gas react with
2 liters of hydrogen
completely, the
limiting factor is the
volume of the oxygen
The coefficients in balanced
equations of gaseous
reactions give the volume
relationships of the gases
If equal masses of
sodium metal and
chlorine gas are
allowed to react,
some sodium will be
leftover after all the
chlorine is used up
The reaction requires
twice as many atoms of
chlorine as sodium
BECAUSE
72
In the following reaction, how many liters of SO2 at
STP will result from the complete burning of pure
sulfur in 8 liters of oxygen?
S + O2
(A)
(B)
(C)
(D)
(E)
SO2
1
4
8
16
32
73
If 80 grams of Al and 80 grams of Fe2O3 are
combined, what is the maximum number of moles
of Fe that can be produced?
2Al + Fe2O3
(A)
(B)
(C)
(D)
(E)
Al2O3 + 2Fe
1
4
8
16
32
74
Acetylene, used as a fuel in welding torches, is
produced in a reaction between calcium carbide
and water:
CaC2 + 2H2O
Ca(OH)2 + C2H2
How many grams of C2H2 are formed from 0.400
moles of CaC2?
(A)
(B)
(C)
(D)
(E)
0.400
0.800
4.00
10.4
26.0
75
Aspirin (C9H8O4) is prepared by reacting salicylic acid
(C7H6O3) and acetic anhydride (C4H6O3)
C7H6O3 + C4H6O3
C9H8O4 + C2H4O2
How many moles of salicylic acid should be used to
prepare six 5-grain aspirin tablets? (1g = 15.5 grains)
(A)
(B)
(C)
(D)
(E)
0.01
0.1
1.0
2.0
31.0
76
Ag(NH3)2+
Ag+ + 2NH3
If 5.8 g of Ag(NH3)2+ yields 1.4 g of ammonia, how
many moles of silver are produced?
(A)
(B)
(C)
(D)
(E)
4.4
5.8
0.041
0.054
7.2
77
How many grams of O2 will it take to oxidize 88 grams
of C3H8 to CO and H2O?
(A)
(B)
(C)
(D)
(E)
32
64
112
166
224
78
How many molecules are in a 36.5 g sample of SF6
gas?
(A)
(B)
(C)
(D)
(E)
1.51 x 1022
1.06 x 1022
1.51 x 1023
1.06 x 1024
1.51 x 10-24
79
What would be the approximate weight of 1.204 x
1024 bromine atoms?
(A)
(B)
(C)
(D)
(E)
80 grams
120 grams
160 grams
180 grams
200 grams
80
Chlorophyll, a green pigment involved in the light
reactions of photosynthesis, consists of 2.4312
percent Mg. If you are given a 100 g sample of
chlorophyll, how many atoms of Mg will it contain?
(A)
(B)
(C)
(D)
(E)
6.02 x 1022 atoms
6.02 x 1023 atoms
6.02 x 1024 atoms
6.02 x 1025 atoms
None of the above
81
Water is formed by the addition of 4.0 g of H2 to an
excess of O2. If 27 g of H2O is recovered, what is the
percent yield for the reaction?
(A)
(B)
(C)
(D)
(E)
25%
50%
75%
100%
Cannot be determined
82
In the reaction 2SO2 + O2
2SO3, 0.25 mole of
sulfur dioxide is mixed with 0.25 mole of oxygen and
allowed to react. What is the maximum number of
moles of SO3 that can be produced?
(A)
(B)
(C)
(D)
(E)
0.0625 mole
0.125 mole
0.25 mole
0.5 mole
1.0 mole
83
The volume of water vapor required to produce
44.8 liters of oxygen by the below reaction is
2H2O
(A)
(B)
(C)
(D)
(E)
2H2 + O2
11.2 L
22.4 L
44.8 L
89.6 L
100.0 L
84
Given this reaction that occurs in plants:
6CO2 + 6H2O
C6H12O6 + 6O2
If 54 grams of water are consumed by the plant,
how many grams C6H12O6 can be made? Assume an
unlimited supply of carbon dioxide for the plant to
consume as well.
(A)
(B)
(C)
(D)
(E)
54 grams
180 grams
540 grams
3 grams
90 grams
85
According to the reaction:
Pb + S
PbS
When 20.7 grams of lead are reacted with 6.4
grams of sulfur
(A) There will be an excess of 20.7 grams of lead
(B) The sulfur will be in excess by 3.2 grams
(C) The lead and sulfur will react completely
without any excess reactants
(D) The sulfur will be the limiting factor in the
reaction
(E) There will be an excess of 10.3 grams of lead
86
Given a 4-gram sample of each H2(g) and He(g), each
in separate containers, which of the following
statements is true? (assume STP)
(A) The sample of hydrogen gas will occupy 44.8 liters
and the sample of helium will contain 6.02 x 1023
molecules
(B) The sample of hydrogen gas will occupy 22.4 liters
and sample of helium will contain 3.02 x 1023
molecules
(C) The sample of hydrogen gas will occupy 44.8 liters
and the sample of helium will contain 1.202 x 1024
molecules
(D) The sample of helium will occupy 44.8 liters and
the sample of hydrogen gas will contain 6.02 x
1023 molecules
(E) None of the above statements is correct.
87
If 48.6 grams of magnesium are placed in a
container with 64 grams of oxygen gas and the
reaction below proceeds to completion, what is the
mass of MgO (s) produced?
2Mg + O2
(A)
(B)
(C)
(D)
(E)
2MgO
15.4 grams
32.0 grams
80.6 grams
96.3 grams
112 grams
88
Given the reaction at STP:
Mg + 2HCl
MgCl2 + H2
How many liters of H2 can be produced from the
reaction of 12.15 grams of Mg with excess HCl?
(A)
(B)
(C)
(D)
(E)
2.0 liters
4.0 liters
11.2 liters
22.4 liters
44.8 liters
89
A sample of a gas at STP contains 3.01 x 1023
molecules and has a mass of 20.0 grams. This gas
would
(A) Have a molar mass of 20.0 grams/mole and
occupy 11.2 liters
(B) Occupy 22.4 liters and have a molar mass of
30.0 grams/mole
(C) Occupy 22.4 liters and have a molar mass of
20.0 grams/mole
(D) Have a molar mass of 40.0 grams/mole and
occupy 33.6 liters
(E) Have a molar mass of 40.0 grams/mole and
occupy 11.2 liters
90
2NO + 2H2
N2 + 2H2O
Which of the following statements is true regarding
the reaction given above?
(A) If 1 mole of H2 is consumed, 0.5 mole of N2 is
produced
(B) If 1 mole of H2 is consumed, 0.5 mole of H2O is
produced
(C) If 0.5 mole of H2 is consumed, 1 mole of N2 is
produced
(D) If 0.5 mole of H2 is consumed, 1 mole of NO is
consumed
(E) If 0.5 mole of H2 iscondsumed, 1 mole of H2O is
produced
91
Propane and oxygen react according to the
equation: C3H8 + 5O2
3CO2 + 4H2O
How many grams of water can be produced from
the complete combustion of 2.0 moles of C3H8?
(A)
(B)
(C)
(D)
(E)
144.0
82.0
8.0
44.8
22.4
92
Carbon and oxygen react to form carbon dioxide
according to the reaction: C + O2
CO2
How much carbon dioxide can be formed from the
reaction of 36 grams of carbon with 64 grams of
oxygen gas?
(A)
(B)
(C)
(D)
(E)
36 grams
64 grams
28 grams
132 grams
88 grams
93
How many grams of Fe2O3 can be formed form the
rusting of 446 grams of Fe according to the
reaction: 4Fe + 3O2
2Fe2O3
(A)
(B)
(C)
(D)
(E)
320 grams
223 grams
159 grams
480 grams
640 grams
94
Sodium and chlorine react according to the
following reaction: 2Na + Cl2
2NaCl
If the reaction starts with 5.0 moles of Na and 3.0
moles of Cl2, then which statement below is true?
(A) Cl2 is the excess reagent and 5.0 moles of NaCl
will be produced
(B) Na is the excess reagent and 2.5 moles of NaCl
will be produced
(C) There will be an excess of 2.0 moles of Na
(D) Na is the limiting reagent and 2.0 moles of NaCl
will be produced
(E) Cl2 is the excess reagent and 2.0 moles of NaCl
will be produced
95
According to the reaction: 3H2 + N2
2NH3
How many grams of hydrogen gas and nitrogen gas
are needed to make exactly 68 grams of ammonia?
(A) 2 grams of hydrogen gas and 28 grams of
nitrogen gas
(B) 3 grams of hydrogen gas and 1 gram of nitrogen
gas
(C) 12 grams of hydrogen gas and 56 grams of
nitrogen gas
(D) 102 grams of hydrogen gas and 34 grams of
nitrogen gas
(E) 6 grams of hydrogen gas and 2 grams of
nitrogen gas
96
What is the mass of 3.0 x 1023 atoms of neon gas?
(A)
(B)
(C)
(D)
(E)
0.50 grams
1.0 grams
5.0 grams
40.0 grams
10.0 grams
97
Which of the following statements is the most
accurate with regard to the significance of
Avogadro’s number, 6.02 x 1023?
(A) It is the conversion factor between grams and
atomic mass units
(B) It is a universal physical constant just as the
speed of light
(C) It is the number of particles that is required to
fill a 1-liter container
(D) It is the inverse diameter of an H atom
(E) It is the number of electrons in the universe
98
In the laboratory a student was determining the
formula for the hydrate of barium chloride, BaCl2. The
student heated the sample in the crucible strongly for
10 minutes. The mass data is provided below:
mass of crucible and cover
31.623 g
mass of crucible, cover and 33.632 g
sample prior to heating
mass of crucible, cover and 33.376 g
sample after heating
After the heating, how many moles of water were
removed from the sample?
(A)
(B)
(C)
(D)
(E)
0.0142 moles
0.0974 moles
0.112 moles
0.256 moles
1.85 moles
99
How many grams of hydrogen gas can be produced
from the following reaction if 65 grams of zinc and
65 grams of HCl are present in the reaction?
Zn + 2HCl
(A)
(B)
(C)
(D)
(E)
ZnCl2 + H2
1.0
1.8
3.6
7.0
58
100
If 60. grams of NO is reacted with sufficient O2 to
form NO2 that is removed during the reaction, how
many grams of NO2 can be produced?
(A)
(B)
(C)
(D)
(E)
46
60.
92
120
180
101
What volume of gas, in liters, would 1.5 moles of
hydrogen occupy at STP?
(A)
(B)
(C)
(D)
(E)
11.2
22.4
33.6
44.8
67.2
102
A gas at STP that contains 6.02 x 1023 atoms and
forms diatomic molecules will occupy
(A)
(B)
(C)
(D)
(E)
11.2 L
22.4 L
33.6 L
67.2 L
1.06 qt
103
5.00 liters of gas at STP have a mass of 12.5 grams.
What is the molar mass of the gas?
(A)
(B)
(C)
(D)
(E)
12.5 g/mol
25.0 g/mol
47.5 g/mol
56.0 g/mol
125 g/mol
104
How many moles of CaO are needed to react with
an excess of water to form 370 grams of calcium
hydroxide?
(A)
(B)
(C)
(D)
(E)
1.0
2.0
3.0
4.0
5.0
105
When 1 mole of chlorine gas reacts completely with
excess KBr solution, as shown below, the products
obtained are
Cl2 + 2Br(A)
(B)
(C)
(D)
(E)
1 mol of Cl- ions and 1 mol of Br1 mol of Cl- ions and 2 mol of Br1 mol of Cl- ions and 1 mol of Br2
2 mol of Cl- ions and 1 mol of Br2
2 mol of Cl- ions and 2 mol of Br2
106
What mass of CaCO3 is needed to produce 11.2
liters of CO2 at STP when the calcium carbonate is
reacted with an excess amount of hydrochloric
acid?
(A)
(B)
(C)
(D)
(E)
25.0 g
44.0 g
50.0 g
100. g
None of the above
107
What is the approximate formula mass of Ca(NO3)2?
(A)
(B)
(C)
(D)
(E)
70
82
102
150
164
108
If 10 liters of CO gas react with sufficient oxygen for
a complete reaction, how many liters of CO2 gas are
formed?
(A)
(B)
(C)
(D)
(E)
5
10
15
20
40
109
If 49 grams of H2SO4 react with 80.0 grams of NaOH,
how much reactant will be left over after the
reaction is complete?
(A)
(B)
(C)
(D)
(E)
24.5 g H2SO4
None of either compound
20. g NaOH
40. g NaOH
60. g NaOH
110
Given one mole of CH4 (g) at STP. Which statements
are true?
I. There are 6.02 x 1023 molecules present
II. The sample will occupy 22.4 L
III. The sample will weigh 16 g
(A)
(B)
(C)
(D)
(E)
I only
II only
I and III only
II and III only
I, II, and III
111
What is the molar mass of Ca3(PO4)2?
(A)
(B)
(C)
(D)
(E)
310 grams/mole
154 grams/mole
67 grams/mole
83 grams/mole
115 grams/mole
112
If the density of a diatomic gas at STP is 1.43 g/L,
what is the gram molecular mass of the gas?
(A)
(B)
(C)
(D)
(E)
14.3 g
32.0 g
48.0 g
64.3 g
224 g
113
From 2 moles of KClO3 how many liters of O2 can be
produced at STP by decomposition of tall the KClO3?
(A)
(B)
(C)
(D)
(E)
11.2
22.4
33.6
44.8
67.2
114
How many atoms are in one mole of water?
(A)
(B)
(C)
(D)
(E)
3
54
6.02x1023
2(6.02x1023)
3(6.02x1023)
115
Four grams of hydrogen gas at STP contain
(A)
(B)
(C)
(D)
(E)
6.02x1023 atoms
12.04x1023 atoms
12.04x1046 atoms
1.2x1023 molecules
12.04x1023 molecules
116
How many liters of O2 can be produced by
completely decomposing 2.00 moles of KClO3?
(A)
(B)
(C)
(D)
(E)
11.2
22.4
33.6
44.8
67.2
117
If the molecular mass of NH3 is 17, what is the
density of this compound at STP?
(A)
(B)
(C)
(D)
(E)
0.25 g/L
0.76 g/L
1.52 g/L
3.04 g/L
9.11 g/L
118
How many grams of sulfur are present in 1 mole of
H2SO4?
(A)
(B)
(C)
(D)
(E)
2
32
49
64
98
119
What is the approximate mass, in grams, of 1 liter of
nitrous oxide, N2O, at STP?
(A)
(B)
(C)
(D)
(E)
1
2
11.2
22
4
120
What is the molar mass of CaCO3?
(A)
(B)
(C)
(D)
(E)
68 g/mol
75 g/mol
82 g/mol
100 g/mol
116 g/mol
121
What volume, in liters, will be occupied at STP by 4
grams of H2?
(A)
(B)
(C)
(D)
(E)
11.2
22.4
33.6
44.8
56.0
122
What volume, in liters, of NH3 is produced when
22.4 liters of N2 are made to combine completely
with a sufficient quantity of H2 under appropriate
conditions?
(A)
(B)
(C)
(D)
(E)
11.2
22.4
44.8
67.2
89.6
123
What volume, in liters, of SO2 will result from the
complete burning of 64 grams of sulfur?
(A)
(B)
(C)
(D)
(E)
2.0
11.2
44.8
126
158
124
How many grams of CO2 can be prepared from 150
grams of calcium carbonate reacting with an excess
of hydrochloric acid solution?
(A)
(B)
(C)
(D)
(E)
11
22
33
44
66
125
What is the mass, in grams, of 1 mole of
KAl(SO4)2 .12H20?
(A)
(B)
(C)
(D)
(E)
132
180
394
474
516
126
What mass of aluminum will be completely oxidized by 2
moles of oxygen at STP?
(A)
(B)
(C)
(D)
(E)
18 g
37.8 g
50.4 g
72.0 g
100.8 g
127
In this reaction:
CaCO3 + 2HCl
CaCl2 + H2O + CO2
If 4.0 moles of HCl are available to the reaction with an
unlimited supply of CaCO3, how many moles of CO2 can
be produced at STP?
(A)
(B)
(C)
(D)
(E)
1.0
1.5
2.0
2.5
3.0
128
The following reaction occurs at STP:
2H2O
2H2 + O2
How many liters of hydrogen gas can be produced by the
breakdown of 72 grams of water?
(A)
(B)
(C)
(D)
(E)
5.6 liters
11.2 liters
22.4 liters
44.8 liters
89.6 liters
129
A sample of a gas at STP contains 3.01 x 1023 molecules
and has a mass of 22.0 grams. This gas is most likely
(A)
(B)
(C)
(D)
(E)
CO2
O2
N2
CO
NO
130
The number of oxygen atoms in 0.50 mole of Al2(CO3)3 is
(A)
(B)
(C)
(D)
(E)
4.5 x 1023
9.0 x 1023
3.6 x 1024
2.7 x 1024
5.4 x 1024
131
4.0 grams of hydrogen are ignited with 4.0 grams of
oxygen. How many grams of water can be formed?
(A)
(B)
(C)
(D)
(E)
0.50
2.5
4.5
8.0
36
132