Name: __________________________ Date: _____________
1. The diameter of an atom is approximately 1  10– 8 cm. What is this diameter when
expressed in nanometers?
A) 1  10– 19 nm
B) 1  10– 15 nm
C) 1  101 nm
D) 1  10– 10 nm
E) 1  10– 1 nm
2. How many milliliters is 0.005 L?
A) 0.5 mL
B) 5 mL
C) 0.50 mL
D) 0.000005 mL
E) 200 mL
3. The SI prefixes giga and micro represent, respectively:
A) 10– 9 and 10– 6.
B) 106 and 10– 3.
C) 103 and 10– 3.
D) 109 and 10– 6.
E) 10– 9 and 10– 3.
4. The SI prefixes kilo and centi represent, respectively:
A) 103 and 10– 2.
B) 106 and 10 1.
C) 10 3 and 10– 2.
D) 10– 6 and 102.
E) 102 and 10– 3.
5. Ammonia boils at –33.4ºC. What temperature is this in ºF?
A) – 60.1ºF
B) – 92.1ºF
C) – 28.1ºF
D) – 18.5ºF
E) +13.5ºF
Page 1
6. Which of the following represents the largest mass?
A) 2.0  102 mg
B) 0.0010 kg
C) 1.0  105 µg
D) 2.0  102 cg
E) 10.0 dg
7. The highest temperature ever recorded in Phoenix, Arizona, was 122ºF. Express this
temperature in ºC.
A) 50ºC
B) 64ºC
C) 67ºC
D) 162ºC
E) 219ºC
8. How many significant figures does the result of the following sum contain?
8.52010  7.9
A) 2
B) 3
C) 4
D) 5
E) 6
9. How many significant figures does the difference 218.7201 – 218.63 contain?
A) 1
B) 2
C) 3
D) 5
E) 7
10. How many cubic inches are in 1.00 liter?
A) 61.0 in3
B) 155 in3
C) 394 in3
D) 1.64  104 in3
E) none of them
Page 2
11. How many cubic centimeters are there in exactly one cubic meter?
A) 1  10–6 cm3
B) 1  10–3 cm3
C) 1  10–2 cm3
D) 1  104 cm3
E) 1  106 cm3
12. If the price of gasoline is $1.14 per U.S. gallon, what is the cost per liter? (1 L = 1.06
qt)
A) $0.0434 /L
B) $4.83 /L
C) $0.302 /L
D) $0.269 /L
E) $1.07 /L
13. Bromine is a red liquid at 25ºC. Its density is 3.12 g/cm3. What is the volume of 28.1 g
of liquid bromine?
A) 87.7 cm3
B) 0.111 cm3
C) 9.01 cm3
D) 28.1 cm3
E) None of the above.
14. Which of the following speeds is the greatest?
A) 40 mi/h
B) 2.0  105 mm/min
C) 40 km/h
D) 0.74 km/min
E) 400 m/min
15. The diameter of Earth is 12.7 Mm. Express this diameter in centimeters.
A) 1.27  105 cm
B) 1.27  106 cm
C) 1.27  107 cm
D) 1.27  108 cm
E) 1.27  109 cm
Page 3
16. The city of Los Angeles is now approximately 2400 miles south of Alaska. It is moving
slowly northward as the San Andreas fault slides along. If Los Angeles is to arrive near
Anchorage, Alaska, in 76 million years, at what average rate will it have to move in mm
per month?
A) 2.0  10 – 10 mm/mo.
B) 6.6  10 – 6 mm/mo.
C) 4.2 mm/mo.
D) 9.5 mm/mo.
E) 51 mm/mo.
18. Americans combined drive about 4.0 109 miles per day and their vehicles get an
average of 20.0 miles per gallon of fuel used. For each 1 kg of gasoline that is burned,
about 3.0 kg of carbon dioxide are produced. How many kilograms of CO2 are emitted
into the atmosphere each day by cars in the U.S.? One gallon of gas weighs about 3.5
kg.
A) 2.1  109 kg
B) 8.4  1011 kg
C) 1.7  108 kg
D) 93 kg
E) none of these
19. A magnesium ion, Mg2+, has
A) 12 protons and 13 electrons.
B) 24 protons and 26 electrons.
C) 12 protons and 10 electrons.
D) 24 protons and 22 electrons.
E) 12 protons and 14 electrons.
20. A sulfide ion, S2– , has:
A) 16 protons and 16 electrons
B) 32 protons and 16 electrons
C) 16 protons and 14 electrons
D) 16 protons and 18 electrons
E) 32 protons and 18 electrons
Page 4
21. What is the formula for the ionic compound formed by calcium and selenium?
A) CaSe
B) Ca2Se
C) CaSe2
D) Ca3Se
E) CaSe3
22. Which of the following scientists developed the nuclear model of the atom?
A) John Dalton
B) Robert Millikan
C) J. J. Thomson
D) Henry Moseley
E) Ernest Rutherford
23. The chemical name for ClO2– is chlorite ion. Therefore, the name of HClO2 is
A) hydrochloric acid
B) chloroform
C) hydrogen dioxychloride
D) chlorous acid
E) chloric acid
24. The formula for sodium sulfide is
A) SNa.
B) K2S.
C) NaS2.
D) Na2S.
E) SeS.
25. The correct name for Ba(OH)2 is
A) barium hydrogen oxide.
B) boron hydroxide.
C) barium hydrate.
D) beryllium hydroxide.
E) barium hydroxide.
Page 5
26. The Stock system name for As2S5 is
A) arsenic(V) sulfide.
B) diarsenic pentasulfide.
C) arsenic(III) sulfide.
D) arsenic(V) sulfate.
E) diarsenic sulfate.
27. The Stock system name for CrO3 is:
A) chromium oxide
B) chromium(II) oxide
C) chromium(III) trioxide
D) chromium(III) oxide
E) chromium(VI) oxide
28. The mineral manganosite is a compound of manganese-55 and oxygen-16. If 77% of
the mass of manganosite is due to manganese, what is the empirical formula of
manganosite?
A) MnO
B) Mn2O
C) Mn2O2
D) MnO2
E) none of these
29. The mineral hausmannite is a compound of manganese-55 and oxygen-16. If 72% of
the mass of hausmannite is due to manganese, what is the empirical formula of
hausmannite?
A) MnO
B) Mn3O
C) Mn3O4
D) Mn4O3
E) MnO3
30. The chemical formula for iron(II) nitrate is
A) Fe2(NO3)3
B) Ir(NO2)2
C) Fe2N3
D) Fe(NO3)2
E) Fe(NO2)2
Page 6
31. What is the formula for the ionic compound formed by magnesium and iodine?
A) MgI
B) Mg2I
C) MgI2
D) MgI3
E) Mg3I
32. What is the formula for the binary compound formed by potassium and nitrogen?
A) KN
B) K2N
C) NK2
D) K3N
E) NK3
33. What is the average mass, in grams, of one atom of iron?
A) 6.02  1023 g
B) 1.66  10–24 g
C) 9.28  10–23 g
D) 55.85 g
E) 55.85  10 –23 g
34. The mass of 1.21  1020 atoms of sulfur is
A) 3.88  1021 g.
B) 2.00 mg.
C) 32.06 g.
D) 6.44 mg.
E) 2.00  10–4 g.
35. What is the mass of 7.80  1018 carbon atoms?
A) 1.30  10 –5 g
B) 6.43  103 g
C) 7.80  1018 g
D) 1.56  10 –4 g
E) 12.01 g
Page 7
36. How many moles of NH3 are there in 77.5 g of NH3?
A) 0.220 mol
B) 4.55 mol
C) 14.0 mol
D) 1.31  103 mol
E) None of the above.
37. Calculate the molecular mass of menthol, C10H20O.
A) 156 amu
B) 140 amu
C) 29 amu
D) 146 amu
E) 136 amu
38. What is the molar mass of nicotine, C10H14N2?
A) 134 g/mol
B) 148 g/mol
C) 158 g/mol
D) 210 g/mol
E) 162 g/mol
39. The molecular formula of aspirin is C9H8O4. How many aspirin molecules are present
in one 500-milligram tablet?
A) 2.77 molecules
B) 2.77  103 molecules
C) 1.67  1024 molecules
D) 1.67  1021 molecules
E) None of these is correct.
40. How many sodium atoms are there in 6.0 g of Na3N?
A) 3.6  1024 atoms
B) 4.6  1022 atoms
C) 1.3  1023 atoms
D) 0.217 atoms
E) 0.072 atoms
Page 8
41. How many sulfur atoms are present in 25.6 g of Al2(S2O3)3?
A) 0.393
B) 6
C) 3.95  1022
D) 7.90  1022
E) 2.37  1023
42. How many grams of nitrogen are there in 7.5 g of Ca(NO3)2?
A) 0.64 g
B) 1.3 g
C) 0.15 g
D) 1.15 g
E) 2.3 g
43. Calculate the mass of 4.50 moles of chlorine gas, Cl2.
A) 6.34  10 –2 g
B) 4.5 g
C) 15.7 g
D) 160 g
E) 319 g
44. 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?
A) Cannot be determined from data given
B) Neither, their abundances are the same.
C) Boron-10
D) Boron-11
45. 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?
A) C10H6O
B) C9H18O
C) C16H28O4
D) C20H12O2
E) C18H36O2
Page 9
46. When balanced with smallest set of whole numbers, the coefficient of O2 in the
following equation is
__ C2H4 + __ O2  __ CO2 + __ H2O
A) 1.
B) 2.
C) 3.
D) 4.
E) 6.
47. 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) 3
B) 8
C) 10
D) 11
E) none of these
48. 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?
A) NH3
B) O2
C) Neither reagent is limiting.
49. Chlorine gas can be made from the reaction of manganese dioxide with hydrochloric
acid. Which is the limiting reagent when 28 g of MnO2 are mixed with 42 g of HCl?
MnO2(s) + 4HCl(aq)  MnCl2(aq) + 2H2O(l) + Cl2(g)
A) MnO2
B) HCl
C) MnCl2
D) Cl2
E) No reagent is limiting.
Page 10
50. 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?
A) 1.30 mol
B) 1.57 mol
C) 1.87 mol
D) 3.53 mol
E) None of these.
51. 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
A) CH2O
B) C3H4O
C) CH4O3
D) C3H4O2
E) C2H4O2
52. 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?
A) 1.6  105 g
B) 3.3  105 g
C) 6.6  105 g
D) 8.7  105 g
E) 1.7  106 g
53. Which of the following compounds is a strong electrolyte?
A) H2O
B) N2
C) CH3COOH (acetic acid)
D) C2H6O (ethanol)
E) KOH
Page 11
54. Which of the following compounds is a weak electrolyte?
A) HCl
B) NH3
C) C6H12O6 (glucose)
D) N2
E) KCl
55. Which of the following compounds is a nonelectrolyte?
A) NaOH
B) HNO3
C) C2H6O (ethanol)
D) KF
E) CH3COOH (acetic acid)
56. Based on the solubility rules, which one of the following compounds should be
insoluble in water?
A) NaCl
B) MgBr2
C) FeCl2
D) AgBr
E) ZnCl2
57. Based on the solubility rules, which one of the following compounds should be
insoluble in water?
A) CaCO3
B) (NH4)2CO3
C) Na2CO3
D) K2CO3
E) KNO3
58. Based on the solubility rules, which one of the following should be soluble in water?
A) AgBr
B) AgCl
C) Ag2CO3
D) AgNO3
E) Ag2S
Page 12
59. Based on the solubility rules, which one of the following should be soluble in water?
A) (NH4)3PO4
B) Ca3(PO4)2
C) AlPO4
D) Ag3PO4
E) Mg3(PO4)2
60. Based on the solubility rules, which of the following will occur when a solution
containing about 0.1 g of Pb(NO3)2(aq) is mixed with a solution containing 0.1 g of
KI(aq) /100 mL?
A) KNO3 will precipitate; Pb2+ and I– are spectator ions.
B) No precipitate will form.
C) Pb(NO3)2 will precipitate; K+ and I– are spectator ions.
D) PbI2 will precipitate; K+ and NO3– are spectator ions.
E) Pb2+ and I– are spectator ions, and PbI2 will precipitate.
61. Which of the following is the correct net ionic equation for the reaction that occurs
when solutions of Pb(NO3)2 and NH4Cl are mixed?
A) Pb(NO3)2(aq) + 2NH4Cl(aq)  NH4NO3(aq) + PbCl2(s)
B) Pb2+(aq) + 2Cl–(aq)  PbCl2(s)


C)
Pb2+(aq) + 2NO3– (aq) + 2NH 4 (aq) + 2Cl–(aq)  2NH 4 (aq) + 2NO3– (aq) +
PbCl2(s)
D) NH4+(aq)+ NO3– (aq)  2NH4NO3(s)
E) No reaction occurs when the solutions are mixed.
62. What is the chemical formula of the salt produced by the neutralization of hydrobromic
acid with magnesium hydroxide?
A) MgBr
B) Mg2Br3
C) Mg3Br2
D) Mg2Br
E) MgBr2
63. The oxidation number of Mn in KMnO4 is
A) +8
B) +7
C) +5
D) 7
E) 8
Page 13
64. The oxidation number of N in N2H4 is
A) +4
B) 4
C) +2
D) 2
E) 0
65. Which one of the following is a redox reaction?
A) 2Al(s) + 3H2SO4(aq)  Al2(SO4)3(aq) + 3H2(g)
B) 2KBr(aq) + Pb(NO3)2(aq)  2KNO3(aq) + PbBr2(s)
C) CaBr2(aq) + H2SO4(aq)  CaSO4(s) + 2HBr(g)
D) H+(aq) + OH (aq)  H2O(l)
E) CO32 (aq) + HSO4(aq)  HCO3 (aq) + SO42 (aq)
66. In the following chemical reaction the oxidizing agent is
5S + 6KNO3 + 2CaCO3  3K2SO4 + 2CaSO4 + CO2 + 3N2
A) S
B) N2
C) KNO3
D) CaSO4
E) CaCO3
67. Identify the reducing agent in the following chemical reaction.
5Fe2+(aq) + MnO4(aq) + 8H+(aq)  5Fe3+(aq) + Mn2+(aq) + 4H2O(l)
A) Fe2+
B) MnO4
C) H+
D) Mn2+
E) Fe3+
68. What element is oxidized in the following chemical reaction?
H2SO4 + Cd(OH)2  2H2O + CdSO4
A) H
B) S
C) O
D) Cd
E) this is not a redox reaction
Page 14
69. What element is reduced in the following chemical reaction?
Cu + 2H2SO4  CuSO4 + SO2 + 2H2O
A) Cu
B) H
C) S
D) O
E) H2O
70. Predict the products of the following single replacement reaction.
Fe(s) + CuSO4(aq) 
A) Cu(s) + FeSO4(aq)
B) Fe(s) + Cu(s) + SO4(aq)
C) CuS(s) + Fe2SO4(aq)
D) FeCuSO4(aq)
E) FeO(s) + CuSO3(aq)
71. Which of the following represents a halogen displacement reaction?
A) 2KBr(aq) + Cl2(g)  2KCl(aq) + Br2(l)
B) 2Na(s) + 2H2O(l)  2NaOH(aq) + H2(g)
C) CaBr2(aq) + H2SO4(aq)  CaSO4(s) + 2HBr(g)
D) 2KNO3(s)  2KNO2(s) + O2(g)
E) 2LiOH(aq) + H2SO4(aq)  Li2SO4(aq) + 2H2O(l)
72. Which of the following represents a hydrogen displacement reaction?
A) 2C2H6(g) + 7O2(g)  4CO2(g) + 6H2O(l)
B) 2KBr(aq) + Cl2(g)  2KCl(aq) + Br2(l)
C) N2(g) + 3H2(g)  2NH3(g)
D) CaBr2(aq) + H2SO4(aq)  CaSO4(s) + 2HBr(g)
E) 2Al(s) + 3H2SO4(aq)  Al2(SO4)3(aq) + 3H2(g)
73. What mass of Na2SO4 is needed to prepare 350. mL of a solution having a sodium ion
concentration of 0.125 M?
A) 3.11 g
B) 24.9 g
C) 12.4 g
D) 6.21 g
E) 8.88 g
Page 15
74. A 50.0 mL sample of 0.436 M NH4NO3 is diluted with water to a total volume of 250.0
mL. What is the ammonium nitrate concentration in the resulting solution?
A) 21.8 M
B) 0.459 M
C) 2.18  102 M
D) 8.72  102 M
E) 0.109 M
75. 35.0 mL of 0.255 M nitric acid is added to 45.0 mL of 0.328 M Mg(NO3)2. What is the
concentration of nitrate ion in the final solution?
A) 0.481 M
B) 0.296 M
C) 0.854 M
D) 1.10 M
E) 0.0295 M
76. 34.62 mL of 0.1510 M NaOH was needed to neutralize 50.0 mL of an H2SO4 solution.
What is the concentration of the original sulfuric acid solution?
A) 0.0229 M
B) 0.218 M
C) 0.0523 M
D) 0.209 M
E) 0.105 M
77. One method of determining the concentration of hydrogen peroxide (H2O2) in a solution
is through titration with iodide ion. The net ionic equation for this reaction is
H2O2 + 2I +2H+  I2 + 2H2O
A 50.00 mL sample of a hydrogen peroxide solution is found to react completely with
37.12 mL of a 0.1500 M KI solution. What is the concentration of hydrogen peroxide in
the sample?
A) 5.568  102 M
B) 0.2227 M
C) 0.1010 M
D) 0.4041 M
E) 0.1114 M
Page 16
78. A sample of a gas occupies 1.40  103 mL at 25ºC and 760 mmHg. What volume will it
occupy at the same temperature and 380 mmHg?
A) 2,800 mL
B) 2,100 mL
C) 1,400 mL
D) 1,050 mL
E) 700 mL
79. The gas pressure in an aerosol can is 1.80 atm at 25°C. If the gas is an ideal gas, what
pressure would develop in the can if it were heated to 475°C?
A) 0.095 atm
B) 0.717 atm
C) 3.26 atm
D) 4.52 atm
E) 34.2 atm
80. At what temperature will a fixed amount of gas with a volume of 175 L at 15°C and
760. mmHg occupy a volume of 198 L at a pressure of 640. mm Hg?
A) 274°C
B) 214°C
C) 114°C
D) 1°C
E) 59°C
81. At what temperature will a fixed mass of gas with a volume of 125 L at 15°C and 750.
mmHg occupy a volume of 101 L at a pressure of 645 mm Hg?
A) 73°C
B) 10.4°C
C) 2°C
D) 34°C
E) 200°C
82. A gas evolved during the fermentation of sugar was collected at 22.5°C and 702 mmHg.
After purification its volume was found to be 25.0 L. How many moles of gas were
collected?
A) 0.950 mol
B) 1.05 mol
C) 12.5 mol
D) 22.4 mol
E) 724 mol
Page 17
83. Calculate the mass, in grams, of 2.74 L of CO gas measured at 33°C and 945 mmHg.
A) 0.263 g
B) 2.46 g
C) 3.80 g
D) 35.2 g
E) 206 g
84. Calculate the density, in g/L, of CO2 gas at 27°C and 0.500 atm pressure.
A) 0.893 g/L
B) 1.12 g/L
C) 9.93 g/L
D) 46.0 g/L
E) 2.17 kg/L
85. Which of the following gases will have the greatest density at the same specified
temperature and pressure?
A) H2
B) CClF3
C) CO2
D) C2H6
E) CF4
86. Determine the molar mass of chloroform gas if a sample weighing 0.389 g is collected
in a flask with a volume of 102 cm3 at 97°C. The pressure of the chloroform is 728
mmHg.
A) 187 g/mol
B) 121 g/mol
C) 112 g/mol
D) 31.6 g/mol
E) 8.28  10-3 g/mol
87. Determine the molar mass of Freon-11 gas if a sample weighing 0.597 g occupies 100.
cm3 at 95°C, and 1,000. mmHg.
A) 0.19 g/mol
B) 35.3 g/mol
C) 70.9 g/mol
D) 137 g/mol
E) 384 g/mol
Page 18
88. A gaseous compound is 30.4% nitrogen and 69.6% oxygen by mass. A 5.25-g sample
of the gas occupies a volume of 1.00 L and exerts a pressure of 1.26 atm at 4.0°C.
Which of the following is its molecular formula?
A) NO
B) NO2
C) N3O6
D) N2O4
E) N2O5
89. A sample of hydrogen gas was collected over water at 21°C and 685 mmHg. The
volume of the container was 7.80 L. Calculate the mass of H2(g) collected. (Vapor
pressure of water = 18.6 mmHg at 21°C.)
A) 0.283 g
B) 0.570 g
C) 0.589 g
D) 7.14 g
E) 435 g
90. How many liters of chlorine gas at 25°C and 0.950 atm can be produced by the reaction
of 12.0 g of MnO2?
MnO2(s) + 4HCl(aq)  MnCl2(aq) + 2H2O(l) + Cl2(g)
A) 5.36  10-3 L
B) 0.138 L
C) 0.282 L
D) 3.09 L
E) 3.55 L
91. Complete this sentence: The molecules of different samples of an ideal gas have the
same average kinetic energies, at the same ________.
A) pressure
B) temperature
C) volume
D) density
92. Which of the following gas molecules have the highest average kinetic energy at 25°C?
A) H2
B) O2
C) N2
D) Cl2
E) All the gases have the same average kinetic energy at 25°C.
Page 19
93. Deviations from the ideal gas law are greater at
A) low temperatures and low pressures.
B) low temperatures and high pressures.
C) high temperatures and high pressures.
D) high temperatures and low pressures.
94. A method of removing CO2 from a spacecraft is to allow the CO2 to react with sodium
hydroxide. (The products of the reaction are sodium carbonate and water.) What
volume of carbon dioxide at 25°C and 749 mmHg can be removed per kilogram of
sodium hydroxide that reacts?
A) 301 L
B) 284 L
C) 276 L
D) 310 L
E) 620 L
Page 20
Answer Key
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
23.
24.
25.
26.
27.
28.
29.
30.
31.
32.
33.
34.
35.
36.
37.
38.
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40.
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43.
44.
E
B
D
A
C
D
A
A
A
A
E
C
C
A
E
C
B
A
C
D
A
E
D
D
E
A
E
A
C
D
C
D
C
D
D
B
A
E
D
C
E
B
E
D
Page 21
45.
46.
47.
48.
49.
50.
51.
52.
53.
54.
55.
56.
57.
58.
59.
60.
61.
62.
63.
64.
65.
66.
67.
68.
69.
70.
71.
72.
73.
74.
75.
76.
77.
78.
79.
80.
81.
82.
83.
84.
85.
86.
87.
88.
89.
90.
E
C
A
B
B
C
B
C
E
B
C
D
A
D
A
D
B
E
B
D
A
C
A
E
C
A
A
E
A
D
A
C
A
A
D
D
A
A
C
A
B
B
D
D
B
E
Page 22
91.
92.
93.
94.
B
E
B
D
Page 23