VERSION 1                                                                             PAGE 1  

MULTIPLE CHOICE

  1. What is the volume of a 12.2 g piece of metal with a density of 9.43 g/cm„?
a) 12.2 cm„
b) 1.29 cm„
c) 0.773 cm„
d) 115 cm„
e) none of these

  2. 1 nanometer = ______ picometers
a) 1000
b) 0.1
c) 0.01
d) 1
e) 10

  3. 1 picometer = _____ centimeters
a) 1 † 10�Œ
b) 1 † 10¨�Œ
c) 1 † 10Š
d) 1 † 10¨Š
e) 1 † 10¨�‚

  4. The density of silver is 10.5 g/cm„.  What volume (cm„) would be occupied by a piece of silver with a mass of 61.3 g?
a) 0.171
b) 644
c) 10.5
d) 0.00155
e) 5.84

  5. How many significant figures are there in the number 0.00230?
a) 2
b) 3
c) 5
d) 6
e) 4

  6. How many significant figures should there be in the answer to the following?
23.1 + 0.11 + 140.3 + 52.07 = _____
a) 5
b) 1
c) 2
d) 3
e) 4

  7. How many significant figures should there be in the answer to the following?
(3.15 † 1.06) + (21 † 1.773) = _____
a) 1
b) 2
c) 3
d) 4
e) 5

  8. What is the correct answer (reported to the proper number of significant figures) to the following?
(2115-2101) † (5.11 † 7.72) = _____
a) 552
b) 552.29
c) 552.3
d) 5.5 † 10‚
e) 6 † 10‚

VERSION 1                                                                             PAGE 2  

  9. 12.00 - 0.83747 + 0.001 = __________
a) 11.16353
b) 11.16
c) 11.1635
d) 11
e) 11.163

 10. How many significant figures should there be in the answer to the following computation?

.                      (10.07 + 7.395)
.                      ÄÄÄÄÄÄÄÄÄÄÄÄÄÄÄ
                            2.5
a) 1
b) 2
c) 3
d) 4
e) 5

 11. An atom of the most common isotope of gold, �‹‰Au, has _____ protons, _____ neutrons, and _____ electrons.
a) 197, 79, 118
b) 118, 79, 39 
c) 79, 197, 197
d) 79, 118, 118
e) 79, 118, 79 

 12. The empirical formula of a compound with molecules containing 12 carbon atoms, 14 hydrogen atoms, and 6 oxygen atoms is __________.
a) C�2H�“O•
b) CHO
c) CH2O
d) C•H–O�
e) C2H“O

VERSION 1                                                                             PAGE 3  

 15. What is the coefficient of H2SO“ when the following equation is balanced?

          H2SO“(aq) + NaOH(aq) ¢ Na2SO“(aq) + H2O(l)

a) 1
b) 2
c) 3
d) 4
e) 0.5

 16. The formula weight (amu) of potassium phosphate is __________.
a) 173.17 
b) 251.37 
c) 212.27 
d) 196.27 
e) 86.07 

 17. The formula weight of the ionic compound (NH“)2SO“ is __________ amu.
a) 100 
b) 118 
c) 116 
d) 132 
e) 264

 18. How many sulfur atoms are there in 25 molecules of C“H“S2?
a) 1.5 † 10‚‡
b) 4.8 † 10‚‡
c) 3.0 † 10‚‡
d) 50
e) 6.02 † 10‚„

 19. A compound was found to contain 40.0% carbon, 6.7% hydrogen, and 53.3% oxygen by mass.  What is the empirical formula of the compound?
a) CH2O
b) C•HO—
c) C2H“O2
d) C�H•O
e) C“H–O”�

 20. What mass (g) of oxygen is required to burn 28.8 g of ammonia?  Be sure to balance the reaction.

            NH� + O2 Ä¢ NO2 + H2O

a) 94.9 
b) 54.1 
c) 108 
d) 15.3
e) 28.8 

 21. A sample of nitrogen (9.27 g) reacts completely with magnesium, according to the equation:

        3 Mg + N2 Ä¢ Mg�N2

The mass of Mg consumed is _____ g.
a) 8.04 
b) 24.1 
c) 16.1 
d) 0.92 
e) 13.9

VERSION 1                                                                             PAGE 4  

 22. How many moles of NH� are produced by the complete reaction of 6.0 mol of H2O according to the following equation?

                  Li�N + 3H2O ¢ 3LiOH + NH�

a) 2.0
b) 1.0
c) 6.0
d) 3.0
e) 18

 23. Calcium carbide (CaC2) reacts with water, producing acetylene (C2H2):

             CaC2 + 2H2O ¢ Ca(OH)2 + C2H2

Production of 13g of C2H2 requires __________ g of H2O.

a) 4.5
b) 9.0
c) 18
d) 4.8 † 10‚
e) 4.8 † 10¨‚

 24. How many grams of N2 are required to completely react with 9.3 g of H2 according to the following equation?
                     N2 + 3H2 ¢ 2NH�
a) 1.3 † 10‚
b) 2.0
c) 43
d) 3.9 † 10‚
e) 4.6

         (c) 2000 Prentice-Hall, Inc. All rights reserved.

VERSION 1                                                                             PAGE 1  

ANSWER KEY FOR TEST - UNTITLED

  1. b
                                    Chapter:1       QUESTION: 46

  2. a
                                    Chapter:1       QUESTION: 55

  3. b
                                    Chapter:1       QUESTION: 56

  4. e
                                    Chapter:1       QUESTION: 64

  5. b
                                    Chapter:1       QUESTION: 69

  6. e
                                    Chapter:1       QUESTION: 71

  7. b
                                    Chapter:1       QUESTION: 72

  8. d
                                    Chapter:1       QUESTION: 74

  9. b
                                    Chapter:1       QUESTION: 92

 10. b
                                    Chapter:1       QUESTION: 98

 11. e
                                    Chapter:2       QUESTION: 27

 12. d
                                    Chapter:2       QUESTION: 74

 13. a
                                    Chapter:2       QUESTION: 81

 14. a
                                    Chapter:2       QUESTION: 93

 15. a
                                    Chapter:3       QUESTION: 18

 16. c
                                    Chapter:3       QUESTION: 66

 17. d
                                    Chapter:3       QUESTION: 69

 18. d
                                    Chapter:3       QUESTION: 89

 19. a
                                    Chapter:3       QUESTION:116

 20. a
                                    Chapter:3       QUESTION:142

VERSION 1                                                                             PAGE 2  

 21. b
                                    Chapter:3       QUESTION:141

 22. a
                                    Chapter:3       QUESTION:147

 23. c
                                    Chapter:3       QUESTION:149

 24. c
                                    Chapter:3       QUESTION:152

         (c) 2000 Prentice-Hall, Inc. All rights reserved.

VERSION 2                                                                             PAGE 1  

MULTIPLE CHOICE

  1. A compound was found to contain 40.0% carbon, 6.7% hydrogen, and 53.3% oxygen by mass.  What is the empirical formula of the compound?
a) CH2O
b) C•HO—
c) C2H“O2
d) C�H•O
e) C“H–O”�

  3. How many significant figures should there be in the answer to the following?
(3.15 † 1.06) + (21 † 1.773) = _____
a) 1
b) 2
c) 3
d) 4
e) 5

  4. The empirical formula of a compound with molecules containing 12 carbon atoms, 14 hydrogen atoms, and 6 oxygen atoms is __________.
a) C�2H�“O•
b) CHO
c) CH2O
d) C•H–O�
e) C2H“O

  5. The formula weight (amu) of potassium phosphate is __________.
a) 173.17 
b) 251.37 
c) 212.27 
d) 196.27 
e) 86.07 

  6. The density of silver is 10.5 g/cm„.  What volume (cm„) would be occupied by a piece of silver with a mass of 61.3 g?
a) 0.171
b) 644
c) 10.5
d) 0.00155
e) 5.84

  7. An atom of the most common isotope of gold, �‹‰Au, has _____ protons, _____ neutrons, and _____ electrons.
a) 197, 79, 118
b) 118, 79, 39 
c) 79, 197, 197
d) 79, 118, 118
e) 79, 118, 79 

VERSION 2                                                                             PAGE 2  

  8. What is the coefficient of H2SO“ when the following equation is balanced?

          H2SO“(aq) + NaOH(aq) ¢ Na2SO“(aq) + H2O(l)

a) 1
b) 2
c) 3
d) 4
e) 0.5

  9. What mass (g) of oxygen is required to burn 28.8 g of ammonia?  Be sure to balance the reaction.

            NH� + O2 Ä¢ NO2 + H2O

a) 94.9 
b) 54.1 
c) 108 
d) 15.3
e) 28.8 

 10. How many moles of NH� are produced by the complete reaction of 6.0 mol of H2O according to the following equation?

                  Li�N + 3H2O ¢ 3LiOH + NH�

a) 2.0
b) 1.0
c) 6.0
d) 3.0
e) 18

 11. 1 nanometer = ______ picometers
a) 1000
b) 0.1
c) 0.01
d) 1
e) 10

 12. Calcium carbide (CaC2) reacts with water, producing acetylene (C2H2):

             CaC2 + 2H2O ¢ Ca(OH)2 + C2H2

Production of 13g of C2H2 requires __________ g of H2O.

a) 4.5
b) 9.0
c) 18
d) 4.8 † 10‚
e) 4.8 † 10¨‚

 13. How many significant figures are there in the number 0.00230?
a) 2
b) 3
c) 5
d) 6
e) 4

VERSION 2                                                                             PAGE 3  

 14. A sample of nitrogen (9.27 g) reacts completely with magnesium, according to the equation:

        3 Mg + N2 Ä¢ Mg�N2

The mass of Mg consumed is _____ g.
a) 8.04 
b) 24.1 
c) 16.1 
d) 0.92 
e) 13.9

 15. 1 picometer = _____ centimeters
a) 1 † 10�Œ
b) 1 † 10¨�Œ
c) 1 † 10Š
d) 1 † 10¨Š
e) 1 † 10¨�‚

 16. How many significant figures should there be in the answer to the following?
23.1 + 0.11 + 140.3 + 52.07 = _____
a) 5
b) 1
c) 2
d) 3
e) 4

 17. 12.00 - 0.83747 + 0.001 = __________
a) 11.16353
b) 11.16
c) 11.1635
d) 11
e) 11.163

 18. The formula weight of the ionic compound (NH“)2SO“ is __________ amu.
a) 100 
b) 118 
c) 116 
d) 132 
e) 264

 20. What is the correct answer (reported to the proper number of significant figures) to the following?
(2115-2101) † (5.11 † 7.72) = _____
a) 552
b) 552.29
c) 552.3
d) 5.5 † 10‚
e) 6 † 10‚

VERSION 2                                                                             PAGE 4  

 21. How many sulfur atoms are there in 25 molecules of C“H“S2?
a) 1.5 † 10‚‡
b) 4.8 † 10‚‡
c) 3.0 † 10‚‡
d) 50
e) 6.02 † 10‚„

 23. How many grams of N2 are required to completely react with 9.3 g of H2 according to the following equation?
                     N2 + 3H2 ¢ 2NH�
a) 1.3 † 10‚
b) 2.0
c) 43
d) 3.9 † 10‚
e) 4.6

 24. What is the volume of a 12.2 g piece of metal with a density of 9.43 g/cm„?
a) 12.2 cm„
b) 1.29 cm„
c) 0.773 cm„
d) 115 cm„
e) none of these

         (c) 2000 Prentice-Hall, Inc. All rights reserved.

VERSION 2                                                                             PAGE 1  

ANSWER KEY FOR TEST - UNTITLED

  1. a
                                    Chapter:3       QUESTION:116

  2. b
                                    Chapter:1       QUESTION: 98

  3. b
                                    Chapter:1       QUESTION: 72

  4. d
                                    Chapter:2       QUESTION: 74

  5. c
                                    Chapter:3       QUESTION: 66

  6. e
                                    Chapter:1       QUESTION: 64

  7. e
                                    Chapter:2       QUESTION: 27

  8. a
                                    Chapter:3       QUESTION: 18

  9. a
                                    Chapter:3       QUESTION:142

 10. a
                                    Chapter:3       QUESTION:147

 11. a
                                    Chapter:1       QUESTION: 55

 12. c
                                    Chapter:3       QUESTION:149

 13. b
                                    Chapter:1       QUESTION: 69

 14. b
                                    Chapter:3       QUESTION:141

 15. b
                                    Chapter:1       QUESTION: 56

 16. e
                                    Chapter:1       QUESTION: 71

 17. b
                                    Chapter:1       QUESTION: 92

 18. d
                                    Chapter:3       QUESTION: 69

 19. a
                                    Chapter:2       QUESTION: 81

 20. d
                                    Chapter:1       QUESTION: 74

VERSION 2                                                                             PAGE 2  

 21. d
                                    Chapter:3       QUESTION: 89

 22. a
                                    Chapter:2       QUESTION: 93

 23. c
                                    Chapter:3       QUESTION:152

 24. b
                                    Chapter:1       QUESTION: 46

         (c) 2000 Prentice-Hall, Inc. All rights reserved.