Basic Chemistry 4e Chapter 7 Chemical Quantities Karen

Basic Chemistry, 4/e Chapter 7: Chemical Quantities Karen Timberlake © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 1. How much does Avogadro’s number of sulfur atoms weigh? A. 16 g B. 32 g C. 16 amu D. 6. 02 × 1023 g © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 1. How much does Avogadro’s number of sulfur atoms weigh? A. 16 g B. 32 g C. 16 amu D. 6. 02 × 1023 g © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 2. How many atoms are there in two moles of helium? A. 2 × 1023 B. 6. 02 × 1023 C. 1. 204 × 1024 D. 6. 02 × 1046 © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 2. How many atoms are there in two moles of helium? A. 2 × 1023 B. 6. 02 × 1023 C. 1. 204 × 1024 D. 6. 02 × 1046 © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 3. How many molecules of water are in 9 g of H 2 O? A. 18 × 1023 B. 9 × 1023 C. 6 × 1023 D. 3 × 1023 © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 3. How many molecules of water are in 9 g of H 2 O? A. 18 × 1023 B. 9 × 1023 C. 6 × 1023 D. 3 × 1023 © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 4. How many molecules of aspirin, C 9 H 8 O 4, are present in 1. 5 mol of aspirin? A. 9. 03 × 1022 molecules aspirin B. 9. 03 × 1023 molecules aspirin C. 9. 03 × 1024 molecules aspirin D. 9. 03 × 1025 molecules aspirin © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 4. How many molecules of aspirin, C 9 H 8 O 4, are present in 1. 5 mol of aspirin? A. 9. 03 × 1022 molecules aspirin B. 9. 03 × 1023 molecules aspirin C. 9. 03 × 1024 molecules aspirin D. 9. 03 × 1025 molecules aspirin © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 5. What is the formula mass for aspirin, C 9 H 8 O 4? A. 144. 13 g B. 179. 15 g C. 180. 16 g D. 181. 17 g © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 5. What is the formula mass for aspirin, C 9 H 8 O 4? A. 144. 13 g B. 179. 15 g C. 180. 16 g D. 181. 17 g © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 6. Calculate the molar mass for isopropyl alcohol, C 3 H 7 OH. A. 59. 09 g B. 60. 00 g C. 60. 10 g D. 61. 10 g © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 6. Calculate the molar mass for isopropyl alcohol, C 3 H 7 OH. A. 59. 09 g B. 60. 00 g C. 60. 10 g D. 61. 10 g © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 7. How many moles of lactic acid, C 3 H 6 O 3, are present in 175. 0 g of lactic acid? A. 1. 67 mol B. 1. 76 mol C. 1. 85 mol D. 1. 94 mol © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 7. How many moles of lactic acid, C 3 H 6 O 3, are present in 175. 0 g of lactic acid? A. 1. 67 mol B. 1. 76 mol C. 1. 85 mol D. 1. 94 mol © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 8. Calculate the molar mass for butane, C 4 H 10. A. 34. 00 g B. 48. 00 g C. 58. 00 g D. 64. 00 g © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 8. Calculate the molar mass for butane, C 4 H 10. A. 34. 00 g B. 48. 00 g C. 58. 00 g D. 64. 00 g © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 9. Calculate the formula mass of Be(NO 3)2. A. 117 g/mol B. 117 g C. 133 g/mol D. 133 g © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 9. Calculate the formula mass of Be(NO 3)2. A. 117 g/mol B. 117 g C. 133 g/mol D. 133 g © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 10. Calculate the molecular mass of pentanol, CH 3(CH 2)3 CH 2 OH. A. 63 g B. 88 g C. 63 g/mol D. 88 g/mol © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 10. Calculate the molecular mass of pentanol, CH 3(CH 2)3 CH 2 OH. A. 63 g B. 88 g C. 63 g/mol D. 88 g/mol © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 11. How many moles are there in 120 g of glucose (C 6 H 12 O 6)? A. 0. 5 moles B. 0. 67 moles C. 1. 0 moles D. 1. 2 moles © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 11. How many moles are there in 120 g of glucose (C 6 H 12 O 6)? A. 0. 5 moles B. 0. 67 moles C. 1. 0 moles D. 1. 2 moles © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 12. Calculate the percent composition by mass for glucose, C 6 H 12 O 6. A. 40. 00% C, 6. 15% H, 53. 84% O B. 40. 00% C, 6. 71% H, 53. 28% O C. 40. 00% C, 7. 27% H, 52. 72% O D. 40. 00% C, 7. 83% H, 52. 16% O © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 12. Calculate the percent composition by mass for glucose, C 6 H 12 O 6. A. 40. 00% C, 6. 15% H, 53. 84% O B. 40. 00% C, 6. 71% H, 53. 28% O C. 40. 00% C, 7. 27% H, 52. 72% O D. 40. 00% C, 7. 83% H, 52. 16% O © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 13. What is the percent carbon in ethanol, C 2 H 5 OH? A. 24% B. 26% C. 52% D. 54% © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 13. What is the percent carbon in ethanol, C 2 H 5 OH? A. 24% B. 26% C. 52% D. 54% © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 14. What is the best empirical formula for magnesium oxide? A. Mg. O B. Mg. O 2 C. Mg 2 O D. Mg 2 O 2 © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 14. What is the best empirical formula for magnesium oxide? A. Mg. O B. Mg. O 2 C. Mg 2 O D. Mg 2 O 2 © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 15. What is the correct molecular formula for a compound of aluminum and oxygen? A. Al. O B. Al 3 O C. Al. O 3 D. Al 2 O 3 © 2014 Pearson Education, Inc.

Chapter 7 – Chemical Quantities 15. What is the correct molecular formula for a compound of aluminum and oxygen? A. Al. O B. Al 3 O C. Al. O 3 D. Al 2 O 3 © 2014 Pearson Education, Inc.