© 2014 Pearson Education, Inc. Basic Chemistry, 4/e Chapter 9: Chemical Quantities in Reactions Karen Timberlake.

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Presentation transcript:

© 2014 Pearson Education, Inc. Basic Chemistry, 4/e Chapter 9: Chemical Quantities in Reactions Karen Timberlake

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 1.Calculate the total mass of the reactants for the following equation. 3H 2 (g) + N 2 (g)  2NH 3 (g) A g B g C g D g

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 1.Calculate the total mass of the reactants for the following equation. 3H 2 (g) + N 2 (g)  2NH 3 (g) A g B g C g D g

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 2. Water is produced by the reaction of hydrogen and oxygen: 2H 2 (g) + O 2 (g)  2H 2 O (l). How many moles of water form when 3 mol O 2 react? A.2 mol B.4 mol C.6 mol D.8 mol

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 2. Water is produced by the reaction of hydrogen and oxygen: 2H 2 (g) + O 2 (g)  2H 2 O (l). How many moles of water form when 3 mol O 2 react? A.2 mol B.4 mol C.6 mol D.8 mol

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 3.How many grams of water are produced from 1.00 g of glucose, C 6 H 12 O 6 ? C 6 H 12 O 6 (s) + 6O 2 (g)  6CO 2 (g) + 6H 2 O (l) A.0.06 g B.0.60 g C.6.00 g D g

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 3.How many grams of water are produced from 1.00 g of glucose, C 6 H 12 O 6 ? C 6 H 12 O 6 (s) + 6O 2 (g)  6CO 2 (g) + 6H 2 O (l) A.0.06 g B.0.60 g C.6.00 g D g

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 4. Hydrogen and oxygen react to form water: 2H 2 (g) + O 2 (g)  2H 2 O (l). If you have 5.0 mol H 2 and 3.0 mol O 2, determine the number of moles of O 2 needed to react with all the H 2. A. 1.5 mol B. 2.0 mol C. 2.5 mol D. 3.0 mol

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 4. Hydrogen and oxygen react to form water: 2H 2 (g) + O 2 (g)  2H 2 O (l). If you have 5.0 mol H 2 and 3.0 mol O 2, determine the number of moles of O 2 needed to react with all the H 2. A. 1.5 mol B. 2.0 mol C. 2.5 mol D. 3.0 mol

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 5.How many grams of water are produced from 1.25 moles of methane? 1 CH O 2  2 H 2 O + 1 CO 2 A grams B.22.5 grams C.45 grams D.90 grams

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 5.How many grams of water are produced from 1.25 moles of methane? 1 CH O 2  2 H 2 O + 1 CO 2 A grams B.22.5 grams C.45 grams D.90 grams

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 6. How many moles of carbon dioxide are produced from 50 grams of methane? 1 CH O 2  2 H 2 O + 1 CO 2 A.0.78 moles B.1.57 moles C.3.13 moles D.6.26 moles

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 6. How many moles of carbon dioxide are produced from 50 grams of methane? 1 CH O 2  2 H 2 O + 1 CO 2 A.0.78 moles B.1.57 moles C.3.13 moles D.6.26 moles

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 7. Which of the following statements is true? A. Actual yield is the amount of product collected when the reaction ends. B.Theoretical yield is the amount of product when the reaction does not go to completion. C. Actual yield is always more than the theoretical yield. D. Theoretical yield is always less than the actual yield.

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 7. Which of the following statements is true? A. Actual yield is the amount of product collected when the reaction ends. B. Theoretical yield is the amount of product when the reaction does not go to completion. C. Actual yield is always more than the theoretical yield. D. Theoretical yield is always less than the actual yield.

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 8. What is the percent yield if 100 g of C 3 H 8 combusts to produce 200 g CO 2 ? A.50% B.67% C.75% D.100%

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 8. What is the percent yield if 100 g of C 3 H 8 combusts to produce 200 g CO 2 ? A.50% B.67% C.75% D.100%

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 9. The enthalpy of solution for ammonium nitrate is 25.7 kJ/mole, making the reaction A.endothermic. B.exothermic.

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 9. The enthalpy of solution for ammonium nitrate is 25.7 kJ/mole, making the reaction A.endothermic. B.exothermic.

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 10.A sample of bleach and sodium sulfite is placed in a calorimeter and measures a temperature change of +7°C. This reaction is A.endothermic. B.exothermic.

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 10.A sample of bleach and sodium sulfite is placed in a calorimeter and measures a temperature change of +7°C. This reaction is A.endothermic. B.exothermic.

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 11.The energy yield in ATP molecules associated with the complete combustion of glucose is A.6 ATP. B.12 ATP. C.24 ATP. D.36 ATP.

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 11.The energy yield in ATP molecules associated with the complete combustion of glucose is A.6 ATP. B.12 ATP. C.24 ATP. D.36 ATP.

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 12.How many grams of CO 2 are produced from the complete combustion of 100 g of propane? A.100 g B.200 g C.300 g D.400 g

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 12.How many grams of CO 2 are produced from the complete combustion of 100 g of propane? A.100 g B.200 g C.300 g D.400 g

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 13.How many grams of water are produced from the complete combustion of 100 g of propane? A.327 g B.222 g C.164 g D. 123 g

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 13.How many grams of water are produced from the complete combustion of 100 g of propane? A.327 g B.222 g C.164 g D.123 g

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 14.Suppose that 2.8 moles of CH4 (methane) is allowed to react with 5 moles of oxygen. What is the limiting reagent? A.Methane B.Oxygen C.Carbon dioxide D.Water

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 14.Suppose that 2.8 moles of CH4 (methane) is allowed to react with 5 moles of oxygen. What is the limiting reagent? A. Methane B.Oxygen C.Carbon dioxide D.Water

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 15.A sample of water and ammonium nitrate is placed in a calorimeter and measures a temperature change of –10°C. This reaction is A.endothermic. B.exothermic.

© 2014 Pearson Education, Inc. Chapter 9 – Chemical Quantities in Reactions 15.A sample of water and ammonium nitrate is placed in a calorimeter and measures a temperature change of –10°C. This reaction is A.endothermic. B.exothermic.