Presentation is loading. Please wait.

Presentation is loading. Please wait.

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

Published bySusan Austin Modified over 9 years ago

Similar presentations

Presentation on theme: "© 2014 Pearson Education, Inc. Basic Chemistry, 4/e Chapter 9: Chemical Quantities in Reactions Karen Timberlake."— Presentation transcript:

1 © 2014 Pearson Education, Inc. Basic Chemistry, 4/e Chapter 9: Chemical Quantities in Reactions Karen Timberlake

2 © 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.30.03 g B.31.04 g C.32.15 g D.34.06 g

3 © 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.30.03 g B.31.04 g C.32.15 g D.34.06 g

4 © 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

5 © 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

6 © 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.60.00 g

7 © 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.60.00 g

8 © 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

9 © 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

10 © 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 4 + 2 O 2  2 H 2 O + 1 CO 2 A.11.25 grams B.22.5 grams C.45 grams D.90 grams

11 © 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 4 + 2 O 2  2 H 2 O + 1 CO 2 A.11.25 grams B.22.5 grams C.45 grams D.90 grams

12 © 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 4 + 2 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

13 © 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 4 + 2 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

14 © 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.

15 © 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.

16 © 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%

17 © 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%

18 © 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.

19 © 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.

20 © 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.

21 © 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.

22 © 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.

23 © 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.

24 © 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

25 © 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

26 © 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

27 © 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

28 © 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

29 © 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

30 © 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.

31 © 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.

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

Similar presentations

Chapter 5 Chemical Reactions

Chapter 5 Chemical Reactions
Chapter 9: Chemical quantities Chemistry 1020: Interpretive chemistry Andy Aspaas, Instructor.

Chapter 9: Chemical quantities Chemistry 1020: Interpretive chemistry Andy Aspaas, Instructor.
VI. Organic Compounds = carbon containing compounds

VI. Organic Compounds = carbon containing compounds
Chemical Quantities Chapter 9

Chemical Quantities Chapter 9
HONORS CHEMISTRY Feb 27, 2012. Brain Teaser Cu + 2 AgNO 3  2 Ag + Cu(NO 3 ) 2 – How many moles of silver are produced when 25 grams of silver nitrate.

HONORS CHEMISTRY Feb 27, Brain Teaser Cu + 2 AgNO 3  2 Ag + Cu(NO 3 ) 2 – How many moles of silver are produced when 25 grams of silver nitrate.
Copyright © Houghton Mifflin Company. All rights reserved. 9 | 1 Information Given by the Chemical Equation Balanced equations show the relationship between.

Copyright © Houghton Mifflin Company. All rights reserved. 9 | 1 Information Given by the Chemical Equation Balanced equations show the relationship between.
Zumdahl • Zumdahl • DeCoste

Zumdahl • Zumdahl • DeCoste
Limiting Reagent What happens in a chemical reaction, if there is an insufficient amount of one reactant?

Limiting Reagent What happens in a chemical reaction, if there is an insufficient amount of one reactant?
Limiting Reactants & Percent Yield. Limiting Reactants  The reactant that limits the amount of product formed in a chemical reaction. The quantity of.

Limiting Reactants & Percent Yield. Limiting Reactants  The reactant that limits the amount of product formed in a chemical reaction. The quantity of.
Chapter 9 Stoichiometry.

Chapter 9 Stoichiometry.
CHEMISTRY February 13, 2012.

CHEMISTRY February 13, 2012.
Stoichiometry Chemistry Ms. Piela.

Stoichiometry Chemistry Ms. Piela.
Chapter 9 Chemical Quantities. 9 | 2 Information Given by the Chemical Equation Balanced equations show the relationship between the relative numbers.

Chapter 9 Chemical Quantities. 9 | 2 Information Given by the Chemical Equation Balanced equations show the relationship between the relative numbers.
AP Chemistry Chap. 3 Stoichiometry, Part 2. 3.6 Chemical Equations (p. 100)- shows a chemical change. Reactants on the LHS, products on the RHS. Bonds.

AP Chemistry Chap. 3 Stoichiometry, Part Chemical Equations (p. 100)- shows a chemical change. Reactants on the LHS, products on the RHS. Bonds.
Stoichiometry.

Stoichiometry.
Mole-to-Mole Conversions

Mole-to-Mole Conversions
Starter S-125 1.2 moles NaC 2 H 3 O 2 are used in a reaction. How many grams is that?

Starter S moles NaC 2 H 3 O 2 are used in a reaction. How many grams is that?
Chapter 9 – Review Stoichiometry

Chapter 9 – Review Stoichiometry
Lecture 109/21/05. Mass reactant Stoichiometric factor Moles reactant Moles product Mass product Stoichiometric Calculations.

Lecture 109/21/05. Mass reactant Stoichiometric factor Moles reactant Moles product Mass product Stoichiometric Calculations.
The general steps for finding PERCENT YIELD : * Write the balanced chemical equation * Find the limiting reactant * Find the theoretical yield (what you.

The general steps for finding PERCENT YIELD : * Write the balanced chemical equation * Find the limiting reactant * Find the theoretical yield (what you.

Similar presentations

Ads by Google