General Chemistry The Essential Concept 7Th Edition Raymond By Chang – Test Bank
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Sample Test
Chapter 03: Stoichiometry
A periodic table will be required to answer some of these
questions.
1. An
atom of helium has a mass about four times greater than that of an atom of
hydrogen. Which choice makes the correct comparison of the relative numbers of
helium and hydrogen atoms in equal masses of the two elements?
2. A)
There are about four times as many helium atoms as hydrogen atoms.
3. B)
There are about two times as many helium atoms as hydrogen atoms.
4. C)
The number of helium and hydrogen atoms is the same.
5. D)
There are about half as many helium atoms as hydrogen atoms.
6. E)
There are about one-fourth as many helium atoms as hydrogen atoms.
Ans: E
Category: Easy Section: 3.1
2. There
are two stable isotopes of chlorine: chlorine-35, with a mass of 34.968853 amu;
and chlorine-37, with a mass of 36.965903. Given that the average atomic mass
of a chlorine atom is 35.45 amu, which of the following statements is true?
3. A)
Chlorine contains almost exclusively of Cl, with very little
4. B)
Chlorine contains more Cl than
5. C)
Chlorine contains roughly equal amounts of Cl and
6. D)
Chlorine contains more Cl than
7. E)
Chlorine contains almost exclusively of Cl, with very little
Ans: B
Category: Easy Section: 3.1
3. An
atom of bromine has a mass about four times greater than that of an atom of
neon. Which choice makes the correct comparison of the relative numbers
of bromine and neon atoms in 1,000 g of each element?
4. A)
The number of bromine and neon atoms is the same.
5. B)
There are one thousand times as many bromine atoms as neon atoms.
6. C)
There are one thousand times as many neon atoms as bromine atoms.
7. D)
There are four times as many neon atoms as bromine atoms.
8. E)
There are four times as many bromine atoms as neon atoms.
Ans: D
Category: Easy
Section: 3.1
4. An
atom of bromine has a mass about four times greater than that of an atom of
neon. How many grams of neon will contain the same number of atoms as
1,000 g of bromine?
5. A) 4
g Ne B) 250 g Ne C) 400 g Ne
D) 1,000 g Ne E) 4,000 g Ne
Ans: B
Category: Medium Section: 3.1
5. An
average atom of uranium (U) is approximately how many times heavier than an
atom of potassium?
6. A) 1
times B) 4.8 times C) 2.4
times D) 12.5 times E) 7.7
times
Ans: A
Category: Easy Section: 3.1
6. Boron
obtained from borax deposits in Death Valley consists of two isotopes.
They are boron-10 and boron-11 with atomic masses of 10.013 amu and 11.009 amu,
respectively. The atomic mass of boron is 10.81 amu (see periodic table).
Which isotope of boron is more abundant, boron-10 or boron-11?
7. A)
Cannot be determined from data given
8. B)
Neither, their abundances are the same.
9. C)
Boron-10
10.
D) Boron-11
Ans: D
Category: Medium Section: 3.1
7. The
element oxygen consists of three naturally occuring isotopes: 16O, 17O,
and 18O. The atomic mass of oxygen is 16.0 amu. What can be
implied about the relative abundances of these isotopes?
8. A)
More than 50% of all O atoms are 17
9. B)
Almost all O atoms are 18
10.
C) Almost all O atoms are 17
11.
D) The isotopes all have the same abundance, i.e. 33.3%.
12.
E) The abundances of 17O
and 18O are very small.
Ans: E Category: Medium
Section: 3.1
8. What
is the average mass, in grams, of one potassium atom?
9. A) 14
´ 10–23 g
D) 31.0 g
10.
B) 49 ´ 10–23 g
E) 39.1 g
11.
C) 02 ´ 10–18 g
Ans: B Category: Easy
Section: 3.2
9. What
is the average mass, in grams, of one atom of iron?
10.
A) 02 ´ 1023 g
D) 55.85 g
11.
B) 66 ´ 10–24 g
E) 55.85 ´ 10 –23 g
12.
C) 28 ´ 10–23 g
Ans: C
Category: Easy Section: 3.2
10.
What is the average mass, in grams, of one arsenic atom?
11.
A) 48 ´ 10–23 g
B) 33.0 g C) 74.9 g D)
1.24 ´ 10–22 g E) 8.04 ´ 1021 g
Ans: D
Category: Easy Section: 3.2
11.
The mass of 1.21 ´ 1020 atoms
of sulfur is
12.
A) 88 ´ 1021 g.
B) 2.00 mg. C) 32.06 g.
D) 6.44 mg. E) 2.00 ´ 10–4 g.
Ans: D
Category: Medium Section: 3.2
12.
The mass of 1.63 ´ 1021 silicon
atoms is
13.
A) 71 ´ 10–23 g.
D) 1.04 ´ 104 g.
14.
B) 58 ´ 1022 g.
E) 7.60 ´ 10–2 g.
15.
C) 08 g.
Ans: E
Category: Medium Section: 3.2
13.
What is the mass of 7.80 ´ 1018 carbon
atoms?
14.
A) 30 ´ 10 –5 g
D) 1.56 ´ 10 –4 g
15.
B) 43 ´ 103 g
E) 12.01 g
16.
C) 80 ´ 1018 g
Ans: D Category: Medium
Section: 3.2
14.
If 0.274 moles of a substance weighs 62.5 g, what is the molar
mass of the substance, in units of g/mol?
15.
A) 28 ´ 102 g/mol
D) 2.17 ´ 102 g/mol
16.
B) 71 ´ 101 g/mol
E) none of these
17.
C) 38 ´ 10 –3 g/mol
Ans: A
Category: Easy Section: 3.2
15.
One mole of iron
16.
A) is heavier than one mole of lead (Pb).
D) weighs the same as one mole of lead.
17.
B) is 77.0 g of iron.
E) None of the above.
18.
C) is 26.0 g of iron.
Ans: E
Category: Medium Section: 3.2
16.
Which one of the following does not represent 1.00 mol of the
indicated substance?
17.
A) 02 ´ 1023 C
atoms
D) 65.4 g Zn
18.
B) 0 g
Fe
E) 6.02 ´ 1023 Fe
atoms
19.
C) 01 g C
Ans: B
Category: Medium Section: 3.2
17.
One nanogram does not seem like a very large number. How
many magnesium atoms are there in 1.00 ng of magnesium?
18.
A) 11 ´ 10–11 atoms
D) 6.02 ´ 1014 atoms
19.
B) 48 ´ 1013 atoms
E) 1.46 ´ 1034 atoms
20.
C) 83 ´ 10–35 atoms
Ans: B Category: Medium
Section: 3.2
18.
How many silicon atoms are there in 1.00 g of silicon?
19.
A) 1
atom
D) 14 ´ 1022 atoms
20.
B) 0356
atoms
E) 1.75 ´ 1025 atoms
21.
C) 57 ´ 1023 atoms
Ans: D
Category: Medium Section: 3.2
19.
Determine the number of moles of aluminum in 96.7 g of Al.
20.
A) 279 mol B) 3.58 mol
C) 7.43 mol D) 4.21 mol
E) 6.02 ´ 1023 mol
Ans: B
Category: Easy Section: 3.2
20.
Calculate the number of moles of xenon in 12.0 g of xenon.
21.
A) 00
mol
D) 7.62 ´ 10–3 mol
22.
B) 0457
mol
E) 0.0914 mol
23.
C) 183 mol
Ans: E
Category: Easy Section: 3.2
21.
A gold wire has a diameter of 1.00 mm. What length of this
wire contains exactly 1.00 mol of gold? (density of Au = 17.0 g/cm3)
22.
A) 2630 m B) 69 m
C) 251 m D) 14.8 m E)
62.7 m
Ans: D Category: Difficult
Section: 3.2
22.
A silver wire has a diameter of 0.500 mm. What length of
this wire contains exactly 1.00 mol of silver? (density of Ag = 10.5 g/cm3)
23.
A) 3 m B) 222 m
C) 13.1 m D) 2.01 m E)
890 m
Ans: A Category: Difficult
Section: 3.2
23.
A copper wire has a diameter of 2.00 mm. What length of
this wire contains exactly 1.00 mol of copper? (density of Cu = 8.92 g/cm3)
24.
A) 178 m B) 0.567 m
C) 180 m D) 45.1 m E)
2.27 m
Ans: E
Category: Difficult Section: 3.2
24.
How many atoms are in 5.54 g of F2?
25.
A) 02 ´ 1023 atoms
D) 8.78 ´ 1022 atoms
26.
B) 146
atoms
E) 1.76 ´ 1023 atoms
27.
C) 292 atoms
Ans: E
Category: Medium Section: 3.3
25.
How many atoms are in 4.39 g of CO2?
26.
A) 80 ´ 1023 atoms
D) 6.04 ´ 1024 atoms
27.
B) 01 ´ 1022 atoms
E) 1.81 ´ 1025 atoms
28.
C) 16 ´ 1026 atoms
Ans: A
Category: Medium Section: 3.3
26.
How many atoms are in 0.0728 g of PCl3?
27.
A) 28 ´ 1021 atoms
D) 3.19 ´ 1020 atoms
28.
B) 38 ´ 1022 atoms
E) 6.02 ´ 1024 atoms
29.
C) 39 ´ 1021 atoms
Ans: A
Category: Medium Section: 3.3
27.
How many moles of CF4 are
there in 171 g of CF4?
28.
A) 51 mol B) 1.94 mol
C) 4.07 mol D) 88.0 mol
E) 171 mol
Ans: B
Category: Easy Section: 3.3
28.
How many moles of NH3 are
there in 77.5 g of NH3?
29.
A) 220
mol
D) 1.31 ´ 103 mol
30.
B) 55
mol
E) None of the above.
31.
C) 0 mol
Ans: B
Category: Easy Section: 3.3
29.
Calculate the number of moles of cesium in 50.0 g of cesium.
30.
A) 376 mol B) 0.357
mol C) 2.66 mol D) 2.80
mol E) 0.0200 mol
Ans: A
Category: Easy Section: 3.2
30.
Which of the following samples contains the greatest number of atoms?
31.
A) 100 g of
Pb
D) 5 g of He
32.
B) 0 mole of
Ar
E) 20 million O2 molecules
33.
C) 1 mole of Fe
Ans: B
Category: Medium Section: 3.2
31.
Calculate the molecular mass of potassium permanganate, KMnO4.
32.
A) 52 amu B) 70 amu
C) 110 amu D) 158 amu E)
176 amu
Ans: D
Category: Easy Section: 3.3
32.
Calculate the molecular mass of menthol, C10H20O.
33.
A) 156 amu B) 140 amu
C) 29 amu D) 146 amu E)
136 amu
Ans: A
Category: Easy Section: 3.3
33.
What is the molar mass of acetaminophen, C8H9NO2?
34.
A) 43 g/mol B) 76
g/mol C) 151 g/mol D) 162
g/mol E) 125 g/mol
Ans: C
Category: Easy Section: 3.3
34.
What is the molar mass of nicotine, C10H14N2?
35.
A) 134 g/mol B) 148
g/mol C) 158 g/mol D) 210
g/mol E) 162 g/mol
Ans: E
Category: Easy Section: 3.3
35.
What is the mass of 0.0250 mol of P2O5?
36.
A) 5 g B) 5676 g C)
0.0250 g D) 1.51 ´ 1022 g
E) 3.55 g
Ans: E
Category: Easy Section: 3.3
36.
Calculate the mass of 3.00 moles of CF2Cl2.
37.
A) 00 g B) 174 g
C) 363 g D) 1.81 ´ 1024 g
E) 40.3 g
Ans: C Category: Easy
Section: 3.3
37.
The molecular formula of aspirin is C9H8O4.
How many aspirin molecules are present in one 500-milligram tablet?
38.
A) 77
molecules
D) 1.67 ´ 1021 molecules
39.
B) 77 ´ 10–3 molecules
E) None of these is correct.
40.
C) 67 ´ 1024 molecules
Ans: D
Category: Medium Section: 3.3
38.
Formaldehyde has the formula CH2O.
How many molecules are there in 0.11 g of formaldehyde?
39.
A) 1 ´ 10 –27
B) 3.7 ´ 10 –3 C)
4 D) 2.2 ´ 1021
E) 6.6 ´ 1022
Ans: D
Category: Medium Section: 3.3
39.
How many molecules are there in 8.0 g of ozone, O3?
40.
A) 3
molecules
D) 0 ´ 1023 molecules
41.
B) 6 ´ 1024 molecules
E) 6.0 ´ 1023 molecules
42.
C) 0 ´ 1023 molecules
Ans: C
Category: Medium Section: 3.3
40.
How many moles of HCl are represented by 1.0 ´ 1019 HCl
molecules?
41.
A) 7 ´ 10–5 mol
D) 36.5 mol
42.
B) 5 ´ 10–3 mol
E) 6.02 ´ 104 mol
43.
C) 0 ´ 1019 mol
Ans: A
Category: Easy Section: 3.2
41.
How many sodium atoms are there in 6.0 g of Na3N?
42.
A) 6 ´ 1024 atoms
D) 0.217 atoms
43.
B) 6 ´ 1022 atoms
E) 0.072 atoms
44.
C) 3 ´ 1023 atoms
Ans: C
Category: Medium Section: 3.3
42.
How many moles of oxygen atoms are there in 10 moles of KClO3?
43.
A) 3 mol B) 3 mol
C) 10 mol D) 30 mol E)
6.02 ´ 1024 mol
Ans: D
Category: Easy Section: 3.3
43.
How many sulfur atoms are there in 21.0 g of Al2S3?
44.
A) 42 ´ 1022 atoms
D) 6.02 ´ 1023 atoms
45.
B) 53 ´ 1023 atoms
E) 6.30 ´ 1026 atoms
46.
C) 14 ´ 1023 atoms
Ans: B
Category: Medium Section: 3.3
44.
How many sulfur atoms are present in 25.6 g of Al2(S2O3)3?
45.
A) 393 B) 6 C)
3.95 ´ 1022 D) 7.90 ´ 1022
E) 2.37 ´ 1023
Ans: E
Category: Medium Section: 3.3
45.
How many fluorine atoms are there in 65 g of CF4?
46.
A) 74
atoms
D) 1.8 ´ 1024 atoms
47.
B) 0
atoms
E) 2.4 ´ 1023 atoms
48.
C) 5 ´ 1023 atoms
Ans: D
Category: Medium Section: 3.3
46.
How many moles of O atoms are in 25.7 g of CaSO4?
47.
A) 189 mol
D) 1.14 ´ 1023 mol
48.
B) 755
mol
E) 4.55 ´ 1023 mol
49.
C) 00 mol
Ans: B
Category: Medium Section: 3.3
47.
How many O atoms are there in 51.4 g CaSO4?
48.
A) 4 B) 40 ´ 1024
C) 1.13 D) 9.09 ´ 1023
E) 2.28 ´ 1023
Ans: D
Category: Medium Section: 3.3
48.
How many moles of Cl atoms are there in 65.2 g CHCl3?
49.
A) 548 mol B) 1.09 mol
C) 3.3 ´ 1023 mol D) 1.64 mol
E) 3.0 mol
Ans: D
Category: Medium
Section: 3.3
49.
How many carbon atoms are there in 10 lbs of sugar, C12H22O11?
50.
A) 6 ´ 1025 atoms
D) 4.21 atoms
51.
B) 0 ´ 1024 atoms
E) 342 atoms
52.
C) 159 atoms
Ans: A
Category: Medium Section: 3.3
50.
How many grams of sulfur are there in 6.0 g of Fe2(SO4)3?
51.
A) 40 g B) 0.48 g
C) 6.00 g D) 0.92 g E)
1.44 g
Ans: E
Category: Medium Section: 3.3
51.
How many grams of sodium are there in 10. g of sodium sulfate,
Na2SO4?
52.
A) 16 g B) 0.32 g
C) 3.2 g D) 1.6 g E) 142
g
Ans: C
Category: Medium Section: 3.3
52.
How many grams of nitrogen are there in 7.5 g of Ca(NO3)2?
53.
A) 64 g B) 1.3 g
C) 0.15 g D) 1.15 g E)
2.3 g
Ans: B
Category: Medium Section: 3.3
53.
The mass of four moles of molecular bromine (Br2) is
54.
A) 80 g. B) 320 g.
C) 640 g. D) 140 g. E) 24
´ 1023
Ans: C
Category: Easy Section: 3.3
54.
Calculate the mass of 4.50 moles of chlorine gas, Cl2.
55.
A) 34 ´ 10 –2 g
B) 4.5 g C) 15.7 g D) 160
g E) 319 g
Ans: E
Category: Easy Section: 3.3
55.
What is the mass of 3.00 moles of ethanol, C2H6O?
56.
A) 99 ´ 10–24 g
B) 138 g C) 6.52 ´ 10–2 g
D) 50 g E) 1.81 ´ 1024 g
Ans: B
Category: Easy Section: 3.3
56.
What is the mass of 0.20 mole of C2H6O
(ethanol)?
57.
A) 230 g B) 46 g
C) 23 g D) 6 g E) None of
these.
Ans: E
Category: Easy Section: 3.3
57.
What is the mass of 8.25 ´ 1019 UF6 molecules?
58.
A) 352 g B) 0482 g
C) 1.37 ´ 10–4 g D) 2.90 ´ 1022 g
E) 8.25 ´ 1019 g
Ans: B
Category: Medium Section: 3.3
58.
A mass spectrometer works by ionizing atoms or molecules, and
then accelerating them past oppositely charged plates. The mass is obtained by
59.
A) measuring the force of impact on a detecting screen, and then
calculating the mass using force = mass ´
60.
B) suspending the ions in an applied electric field, and then
calculating mass by setting the downward gravitational force equal to the
upward electrostatic force.
61.
C) measuring the magnitude of deflection as the ions pass
through a magnetic field to obtain the charge-to-mass ratio, and then
calculating the mass from that ratio.
62.
D) measuring the time it takes for the ions to hit the detector
at a known distance to calculate the acceleration, and then calculating mass
from force = mass ´
Ans: C
Category: Medium Section: 3.4
59.
The empirical formula of a compound of uranium and fluorine that
is composed of 67.6% uranium and 32.4% fluorine is
60.
A) U2 B) U3F4.
C) UF4. D) UF6.
E) UF8.
Ans: D
Category: Medium Section: 3.6
60.
The percent composition by mass of a compound is 76.0% C, 12.8%
H, and 11.2% O. The molar mass of this compound is 284.5 g/mol. What is the
molecular formula of the compound?
61.
A) C10H6O B) C9H18O
C) C16H28O4 D) C20H12O2
E) C18H36O2
Ans: E
Category: Medium Section: 3.6
61.
A compound was discovered whose composition by mass is 85.6% C
and 14.4% H. Which of the following could be the molecular formula of this
compound?
62.
A) CH4 B) C2H4
C) C3H4 D) C2H6
E) C3H8
Ans: B
Category: Medium Section: 3.6
62.
An organic thiol compound is 38.66% C, 9.73% H, and 51.61% S by
mass. What is the empirical formula of this compound?
63.
A) C2H6S B) C3H8S
C) C4H10S D) C4H12S
E) C5H14S
Ans: A Category: Medium
Section: 3.6
63.
The percent composition by mass of an unknown chlorinated
hydrocarbon was found to be 37.83% C, 6.35% H, and 55.83% Cl by mass. What is
the empirical formula of this compound?
64.
A) C2H4Cl B) C3H7Cl
C) C3H6Cl2 D) C4H9Cl
E) C5H11Cl
Ans: A
Category: Medium Section: 3.6
64.
Which one of the following chemical reactions is balanced?
65.
A) HCl + KMnO4
® Cl2 + MnO2 + H2O +
KCl
66.
B) HCl + KMnO4
® Cl2 + MnO2 + 2H2O +
KCl
67.
C) 2HCl + 2KMnO4
® Cl2 + MnO2 + 2H2O +
2KCl
68.
D) 6HCl + 2KMnO4
® 2Cl2 + 2MnO2 +
4H2O + 2KCl
69.
E) 8HCl + 2KMnO4
® 3Cl2 + 2MnO2 +
4H2O + 2KCl
Ans: E
Category: Medium Section: 3.6
65.
What is the coefficient of H2O
when the following equation is properly balanced with the smallest set of whole
numbers?
___ Na + ___ H2O ®
___ NaOH + ___ H2
1. A)
1 B) 2 C) 3
D) 4 E) 5
Ans: B
Category: Medium Section: 3.7
66.
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
1. A)
3 B) 4 C) 6
D) 12 E) 24
Ans: D
Category: Medium Section: 3.7
67.
When balanced with smallest set of whole numbers, the
coefficient of O2 in the following equation is
__ C2H4 + __ O2 ®
__ CO2 + __ H2O
1. A)
B) 2. C) 3.
D) 4. E) 6.
Ans: C
Category: Medium Section: 3.7
68.
When a chemical equation is balanced, it will have a set of
whole number coefficients that cannot be reduced to smaller whole numbers.
What is the coefficient for O2 when
the following combustion reaction of a hydrocarbon is balanced?
___ C7H14 + ___ O2
® ___ CO2 + ___ H2O
1. A)
42 B) 21 C)
11 D) 10 E) none of these
Ans: B
Category: Medium Section: 3.7
69.
What is the coefficient preceding O2 when
the following combustion reaction of a fatty acid is properly balanced using
the smallest set of whole numbers?
__ C18H36O2 + __ O2 ®
__ CO2 + __ H2O
1. A)
1 B) 8 C) 9
D) 26 E) 27
Ans: D Category: Medium
Section: 3.7
70.
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
1. A)
3 B) 8 C) 10
D) 11 E) none of these
Ans: A
Category: Medium Section: 3.7
71.
Balance the equation below using the smallest set of whole
numbers. What is the coefficient of H2O?
___ PCl3(l) + ___ H2O(l)
® ___ H3PO3(aq) + ___ HCl(aq)
1. A)
1 B) 2 C) 3
D) 5 E) none of these
Ans: C
Category: Medium Section: 3.7
72.
What is the coefficient of O2 when
the following equation is properly balanced with the smallest set of whole
numbers?
___ CH3OH + ___ O2
® ___ CO2 + ___ H2O
1. A)
1 B) 2 C) 3
D) 7 E) none of these
Ans: C
Category: Medium Section: 3.7
73.
Balance the following equation using the smallest set of whole
numbers, then add together the coefficients. Do not forget to count
coefficients of one. The sum of the coefficients is
__ SF4 + __ H2O
® __ H2SO3 + __ HF
4. A)
B) 6. C) 7.
D) 9. E) none of these.
Ans: D
Category: Medium Section: 3.7
74.
Balance the following equation using the smallest set of whole
numbers, then add together the coefficients. Don’t forget to count coefficients
of one. The sum of the coefficients is
___ Cr + ___ H2SO4 ®
___ Cr2(SO4)3 + ___ H2
4. A)
B) 9. C) 11.
D) 13. E) 15.
Ans: B
Category: Medium Section: 3.7
75.
Balance the following equation using the smallest set of whole
numbers, then add together the coefficients. Do not forget to count
coefficients of one. The sum of the coefficients is
___ Al + ___ H2SO4 ®
___ Al2(SO4)3 + ___ H2
3. A)
B) 5. C) 6.
D) 9. E) 12.
Ans: D
Category: Medium Section: 3.7
76.
Balance the following equation using the smallest set of whole
numbers, then add together the coefficients. Do not forget to count
coefficients of one. The sum of the coefficients is
___ CH4 + ___ Cl2 ®
___ CCl4 + ___ HCl
4. A)
B) 6. C) 8.
D) 10. E) 12.
Ans: D
Category: Medium Section: 3.7
77.
Ammonia reacts with diatomic oxygen to form nitric oxide and
water vapor:
4NH3 + 5O2 ® 4NO +
6H2O
When 40.0 g NH3 and
50.0 g O2 are allowed to react, which is the limiting reagent?
1. A) NH3
B) O2 C) NO D) H2O
E) No reagent is limiting.
Ans: B
Category: Medium Section: 3.9
78.
Ammonia reacts with diatomic oxygen to form nitric oxide and
water vapor:
4NH3 + 5O2 ® 4NO +
6H2O
When 20.0 g NH3 and
50.0 g O2 are allowed to react, which is the limiting reagent?
1. A) NH3
B) O2 C) NO D) H2O
E) No reagent is limiting.
Ans: A
Category: Medium Section: 3.9
79.
When 22.0 g NaCl and 21.0 g H2SO4 are
mixed and react according to the equation below, which is the limiting reagent?
2NaCl + H2SO4
® Na2SO4 + 2HCl
1. A)
NaCl B) H2SO4
C) Na2SO4 D) HCl E) No
reagent is limiting.
Ans: A
Category: Medium Section: 3.9
80.
Vanadium(V) oxide reacts with calcium according to the chemical
equation below. When 10.0 moles of V2O5 are
mixed with 10.0 moles of Ca, which is the limiting reagent?
V2O5(s) + 5Ca(l) ® 2V(l) + 5CaO(s)
1. A) V2O5
B) Ca C) V D)
CaO E) No reagent is limiting.
Ans: B Category: Medium
Section: 3.9
81.
Chlorine gas can be made from the reaction of manganese dioxide
with hydrochloric acid.
MnO2(s) + 4HCl(aq) ® MnCl2(aq)
+ 2H2O(l) + Cl2(g)
According to the above reaction, which is the limiting reagent
when 28 g of MnO2 are reacted with 42 g of HCl?
1. A)
MnO2 B) HCl C) MnCl2
D) Cl2 E) No reagent is limiting.
Ans: B
Category: Medium Section: 3.9
82.
How many grams of Cl2 can
be prepared from the reaction of 16.0 g of MnO2 and
30.0 g of HCl according to the following chemical equation?
MnO2 + 4HCl ® MnCl2 +
Cl2 + 2H2O
1. A) 82
g B) 5.8 g C) 13.0
g D) 14.6 g E) 58.4 g
Ans: C
Category: Medium Section: 3.9
83.
Hydrogen chloride gas can be prepared by the following reaction:
2NaCl(s) + H2SO4(aq)
® 2HCl(g) + Na2SO4(s)
How many grams of HCl can be prepared from 2.00 mol H2SO4 and
150 g NaCl?
7. A) 30
g B) 93.5 g C) 146
g D) 150 g E) 196 g
Ans: B
Category: Medium Section: 3.9
84.
Calculate the mass of FeS formed when 9.42 g of iron reacts with
8.50 g of sulfur according to the following reaction.
Fe(s) + S(s) ® FeS(s)
17.
A) 9 g B) 87.9 g
C) 26.0 g D) 14.8 g E)
1.91 ´ 10–3 g
Ans: D
Category: Medium Section: 3.9
85.
What is the theoretical yield of chromium that can be produced
by the reaction of 40.0 g of Cr2O3 with
8.00 g of aluminum according to the chemical equation below?
2Al + Cr2O3 ®
Al2O3 + 2Cr
7. A) 7
g B) 15.4 g C) 27.3
g D) 30.8 g E) 49.9 g
Ans: B Category: Medium
Section: 3.9
86.
Calculate the mass of excess reagent remaining at the end of the
reaction in which 90.0 g of SO2 are
mixed with 100.0 g of O2.
2SO2 + O2 ® 2SO3
11.
A) 5 g B) 22.5 g
C) 67.5 g D) 77.5 g E)
400 g
Ans: D Category: Medium
Section: 3.9
87.
What is the maximum number of grams of ammonia, NH3,
that can be obtained from the reaction of 10.0 g of H2 and
80.0 g of N2?
N2 + 3H2 ® 2NH3
28.
A) 4 g B) 48.6 g
C) 56.7 g D) 90.0 g E)
97.1 g
Ans: C Category: Medium
Section: 3.9
88.
How many grams of water could be made from 5.0 mol H2 and
3.0 mol O2?
89.
A) g B) 36 g C)
42 g D) 45 g E) 108 g
Ans: A
Category: Medium Section: 3.9
89.
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 NH3 and
50.0 g O2 are mixed and allowed to react?
1. A) 30
mol B) 1.57 mol C) 1.87
mol D) 3.53 mol E) None of
these.
Ans: C
Category: Medium Section: 3.9
90.
What is the theoretical yield of vanadium, in moles, that can be
produced by the reaction of 2.0 mole of V2O5 with
6.0 mole of calcium based on the following chemical reaction?
V2O5(s) + 5Ca(l) ® 2V(l) + 5CaO(s)
1. A) 0
mol B) 1.6 mol C) 2.0
mol D) 2.4 mol E) 4.0 mol
Ans: D
Category: Medium Section: 3.9
91.
What is the theoretical yield of vanadium, in moles, that can be
produced by the reaction of 1.0 mole of V2O5 with
4.0 mole of calcium based on the following chemical reaction?
V2O5(s) + 5Ca(l) ® 2V(l) + 5CaO(s)
1. A) 0
mol B) 1.6 mol C) 2.0
mol D) 0.80 mol E) None of
these
Ans: B
Category: Medium Section: 3.9
92.
What is the theoretical yield of vanadium that can be produced
by the reaction of 40.0 g of V2O5 with
40.0 g of calcium based on the following chemical reaction?
V2O5(s) + 5Ca(l) ® 2V(l) + 5CaO(s)
11.
A) 2 g B) 5.6 g
C) 22.4 g D) 40.0 g E)
20.3 g
Ans: E Category: Medium
Section: 3.9
93.
How many grams of Cr can be produced by the reaction of 44.1 g
of Cr2O3 with 35.0 g of Al according to the following chemical
reaction?
2Al + Cr2O3
® Al2O3 + 2Cr
7. A) 56
g B) 30.2 g C) 67.4
g D) 104 g E) None of these.
Ans: B
Category: Medium Section: 3.9
94.
What is the theoretical yield of aluminum that can be produced
by the reaction of 60.0 g of aluminum oxide with 30.0 g of carbon according to
the following chemical reaction?
Al2O3 + 3C ® 2Al + 3CO
30.
A) 0 g B) 7.9 g
C) 101.2 g D) 45.0 g E)
31.8 g
Ans: E
Category: Medium Section: 3.9
95.
A 1.375 g sample of mannitol, a sugar found in seaweed, is
burned completely in oxygen to give 1.993 g of carbon dioxide and 0.9519 g of
water. The empirical formula of mannitol is
96.
A) B) CH7O3.
C) C3H2O. D) C3H7O3.
E) CH2O.
Ans: D
Category: Difficult Section: 3.6
96.
A 0.8715 g sample of sorbic acid, a compound first obtained from
the berries of a certain ash tree, is burned completely in oxygen to give 2.053
g of carbon dioxide and 0.5601 g of water. The empirical formula of sorbic acid
is
97.
A) CH2 B) C3H4O.
C) CH4O3. D) C3H4O2.
E) C2H4O2.
Ans: B
Category: Difficult Section: 3.6
97.
An oxyhydrocarbon produced in a chemical reaction was determined
to have a molecular mass of 120.20 g/mol. Which of the following is a possible
empirical formula for this compound?
98.
A) CH4O B) C2H6O
C) C3H8O D) C3H8O2
E) C4H10O2
Ans: C
Category: Easy Section: 3.6
98.
Washing soda is a hydrate of sodium carbonate. Elemental
analysis of a sample of washing soda gave 4.20% C and 7.05% H. What is the
formula for washing soda?
99.
A) Na2CO3×2H2O
D) Na2CO3×8H2O
100.
B) Na2CO3×4H2O
E) Na2CO3×10H2O
101.
C) Na2CO3×6H2O
Ans: E
Category: Difficult Section: 3.6
99.
The first step in the Ostwald process for producing nitric acid
is
4NH3(g) + 5O2(g) ® 4NO(g) + 6H2O(g).
If the reaction of 150. g of ammonia with 150. g of oxygen gas
yields 87. g of nitric oxide (NO), what is the percent yield of this reaction?
1. A)
100% B) 49% C)
77% D) 33% E) 62%
Ans: C
Category: Difficult Section: 3.10
100.
One way of obtaining pure sodium carbonate is through the
decomposition of the mineral trona, Na5(CO3)2(HCO3)×2H2O, as
shown in the following reaction:
2Na3(CO3)(HCO3)×2H2O(s) ® 3Na2CO3(s) +
CO2(g) + 5H2O(g)
When 15 metric ton (1 ´ 103 kg)
of trona is decomposed, 11 metric ton of Na2CO3 is
recovered. What is the percent yield of this reaction? (1 metric ton = 103 kg)
1. A)
95% B) 73% C)
65% D) 42% E) 13%
Ans: A
Category: Difficult Section: 3.10
101.
When octane (C8H18) is
burned in a particular internal combustion engine, the yield of products
(carbon dioxide and water) is 93%. What mass of carbon dioxide will be
produced in this engine when 15.0 g of octane is burned with 15.0 g of oxygen
gas?
102.
A) g B) 12. g C)
21. g D) 54. g E) 43. g
Ans: B
Category: Difficult Section: 3.10
102.
The Hall process for the production of aluminum involves the
reaction of aluminum oxide with elemental carbon to give aluminum metal and
carbon monoxide. If the yield of this reaction is 75%, what mass of
aluminum metal can be produced from the reaction of 1.65 ´ 106 of
aluminum oxide with 1.50 ´ 106 g
of carbon?
103.
A) 6 ´ 105 g
D) 8.7 ´ 105 g
104.
B) 3 ´ 105 g
E) 1.7 ´ 106 g
105.
C) 6 ´ 105 g
Ans: C
Category: Difficult Section: 3.10
103.
The Hall process for the production of aluminum involves the
reaction of aluminum oxide with elemental carbon to give aluminum metal and
carbon monoxide. If the yield of this reaction is 82% and aluminum ore is
71% by mass aluminum oxide, what mass of aluminum ore must be mined in order to
produce 1.0 ´ 103 kg (1 metric ton) of aluminum metal by the Hall process?
104.
A) 8 ´ 103 kg
D) 1.6 ´ 103 kg
105.
B) 2 ´ 103 kg
E) 3.3 ´ 103 kg
106.
C) 1 ´ 103 kg
Ans: E
Category: Difficult Section: 3.10
104.
A method for producing pure copper metal involves the reaction
of copper(I) sulfide with oxygen gas to give copper metal and sulfur
dioxide. Suppose the yield of this reaction is 87%. What mass of a copper
ore consisting of 46% copper(I) sulfide must be mined in order to produce 1.0 ´
103 kg (1.0 metric ton) of copper metal?
105.
A) 4 ´ 103 kg
D) 1.5 ´ 103 kg
106.
B) 2 ´ 103 kg
E) 8.0 ´ 103 kg
107.
C) 3 ´ 103 kg
Ans: B
Category: Difficult Section: 3.10
105.
Solid sodium hydrogen carbonate (also known as sodium
bicarbonate) can be decomposed to form solid sodium carbonate, gaseous carbon
dioxide, and water vapor. When the balanced chemical reaction for this
process is written such that the coefficient of water is 1, what is the
coefficient of carbon dioxide?
106.
A) 0 B) 1 C)
2 D) E) cannot be
determined
Ans: B
Category: Medium Section: 3.7
106.
Aluminum hydroxide reacts with nitric acid to form aluminum
nitrate and water. What mass of water can be formed by the reaction of
15.0 g of aluminum hydroxide with excess nitric acid?
107.
A) 15 g B) 3.46 g
C) 45.0 g D) 6.14 g E)
10.4 g
Ans: E
Category: Medium Section: 3.8
107.
Liquid hexane, C6H14,
burns in oxygen gas to yield carbon dioxide and water. What is the
minimum mass of oxygen required for the complete reaction of 10.0 mL of hexane?
(density of hexane = 0.660 g/mL)
108.
A) 71 g B) 2.45 g
C) 23.3 g D) 46.6 g E)
35.3 g
Ans: C
Category: Medium Section: 3.8
108.
Liquid heptane, C7H16 ,
burns in oxygen gas to yield carbon dioxide and water. What mass of
carbon dioxide is produced when 15.0 mL of heptane burns completely? (density
of heptane = 0.6838 g/mL)
109.
A) 1 g B) 71.8 g
C) 4.49 g D) 6.59 g E)
31.5 g
Ans: E
Category: Medium Section: 3.8
109.
Liquid heptane, C7H16,
burns in oxygen gas to yield carbon dioxide and water. What mass of water
is produced when 15.0 mL of heptane burns completely? (density of heptane =
0.6838 g/mL)
110.
A) 8 g B) 2.70 g
C) 31.6 g D) 1.85 g E)
21.6 g
Ans: A
Category: Medium Section: 3.8
110.
Liquid heptane, C7H16,
burns in oxygen gas to yield carbon dioxide and water. What is the
minimum mass of oxygen required for the complete reaction of 25.5 mL of
heptane? (density of heptane = 0.6838 g/mL)
111.
A) 14 g B) 89.6 g
C) 61.3 g D) 30.6 g E)
5.57 g
Ans: C
Category: Medium Section: 3.8
111.
Which of the following statements are true about a sample of
sulfur and a sample of oxygen if the two samples are of equal mass?
112.
The number of electrons in the two samples is about the same.
113.
The number of protons in the two samples is about the same.
III. The number of atoms in the two samples is about the same.
1. There
are roughly twice as many sulfur atoms as oxygen atoms.
2. There
are roughly twice as many oxygen atoms as sulfur atoms.
Ans: I, II, and V
Category: Difficult
Section: 3.1
112.
Nickel has a lower atomic mass than cobalt, even though it has a
higher atomic number. One possible explanation is that one of the average
atomic masses was miscalculated. In the case of cobalt, there is only one
isotope: 100% 59Co at a mass of 58.9332 amu. For nickel, however, there are five
isotopes as given in the table.
|
isotope |
mass (amu) |
abundance |
|
58Ni |
57.9354 |
67.76% |
|
60Ni |
59.9308 |
26.16% |
|
61Ni |
60.9311 |
1.25% |
|
62Ni |
61.9283 |
3.66% |
|
64Ni |
63.9280 |
1.16% |
1. Using
the data in the table, calculate the average atomic mass for nickel.
2. Is
the atomic mass for nickel in your periodic table correct?
3. Regardless
of your answer to part B, how else could you explain the observation that the
atomic mass of nickel is less than the mass of cobalt, even though it has the
higher atomic number?
Ans: A. 58.70 amu
1. yes
2. Cobalt
has 27 protons and 32 neutrons per atom. While nickel has one more proton than
cobalt, it has on average greater enough fewer neutrons than cobalt to lower
the average atomic mass of nickel to be less than that of cobalt.
Category: Difficult
Section: 3.1
113.
How many moles of aluminum are present in an Al cylinder with a
mass of 15 g?
Ans: 0.56 mole
Category: Easy
Section: 3.2
114.
How many moles of iron are present in an iron cylinder that
weighs 25 g?
Ans: 0.45 mole
Category: Easy Section: 3.2
115.
Calculate the molecular mass, in g/mol, of H2SO4.
Ans: 98.09 g/mol
Category: Easy
Section: 3.3
116.
Calculate the molecular mass, in g/mol, of P4O10.
Ans: 283.9 g/mol
Category: Easy
Section: 3.3
117.
Calculate the molecular mass, in g/mol, of C6H12O6.
Ans: 180.2 g/mol
Category: Easy
Section: 3.3
118.
How many ICl3 molecules
are present in 1.75 kg of ICl3?
Ans: 4.52 ´ 1024
Category: Medium
Section: 3.3
119.
How many Mg atoms are present in 170 g of Mg?
Ans: 4.2 ´ 1024
Category: Easy
Section: 3.2
120.
Calculate the mass of 3.7 moles of Br2.
Ans: 590 g
Category: Easy
Section: 3.3
121.
Calculate the volume of 0.15 mole of Br2. The
density of Br2 is 3.12 g/mL.
Ans: 7.7 mL
Category: Medium
Section: 3.3
122.
A chemistry student determined the empirical formula for
titanium sulfide (TixSy). To do so, she reacted titanium with excess sulfur in a crucible,
and recorded the following data:
Weight of
crucible
11.120 g
Weight of
titanium
8.820 g
Weight of crucible and product 31.700 g
What is the empirical formula of titanium sulfide?
Ans: TiS2
Category: Medium Section: 3.6
123.
A chemistry student determined the empirical formula for
tungsten oxide (WxOy). To do so, he heated tungsten with oxygen in a crucible. The
data that he recorded are shown below:
Weight of
crucible
11.120 g
Weight of tungsten
8.820 g
Weight of crucible and product 22.998 g
What is the empirical formula of tungsten oxide?
Ans: WO4
Category: Medium
Section: 3.6
124.
A compound with a percent composition by mass of 87.5% N and
12.5% H was recently discovered. What is the empirical formula for this
compound?
Ans: NH2
Category: Medium
Section: 3.6
125.
Define a mole.
Ans: An Avogadro’s number of a specific entity, such as an
atom or molecule
Category: Easy
Section: 3.2
126.
If 0.66 mole of a substance has a mass of 99 g, what is the
molecular mass of the substance?
Ans: 150 g
Category: Medium
Section: 3.2
127.
Calculate the molecular mass of ethylene glycol, C2H6O2, a
compound frequently used as automobile antifreeze.
Ans: 62.1 g
Category: Easy
Section: 3.3
128.
Calculate the percent composition by mass of sodium in Na2CO3.
Ans: 43.4%
Category: Medium
Section: 3.5
129.
Calculate the percent composition by mass of carbon in Na2CO3.
Ans: 11.3%
Category: Medium
Section: 3.5
130.
Calculate the percent composition by mass of oxygen in Na2CO3.
Ans: 45.3%
Category: Medium
Section: 3.5
131.
A 0.600 g sample of a compound of arsenic and oxygen was found
to contain 0.454 g of arsenic. What is the empirical formula of the compound?
Ans: As2O3
Category: Medium
Section: 3.6
132.
A sample of unknown ore was analyzed and found to contain 12.7%
Al, 19.7% N, and 67.6% O. What is the empirical formula of this ore?
Ans: AlN3O9
Category: Medium
Section: 3.6
133.
Phosgene, a poisonous gas used during WWI, is composed of 12.1%
C, 16.2% O, and 71.1% Cl. What is the empirical formula of phosgene?
Ans: COCl2
Category: Medium
Section: 3.6
134.
What percent by mass of oxygen is present in carbon monoxide,
CO?
Ans: 57%
Category: Medium
Section: 3.5
135.
Balance the following chemical equation:
NaNO3 ® NaNO2 +
O2
Ans: 2NaNO3 ®
2NaNO2 + O2
Category: Medium
Section: 3.7
136.
Balance the following chemical equation:
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