1. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu S.15.C.6 Identify the physical state for each substance in a reaction equation Reinforced

2. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Main Standards

3. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Table of Contents Stoichiometry Section 2 Ideal Stoichiometric Calculations

4. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Objective Calculate the amount in moles of a reactant or a product from the amount in moles of a different reactant or product. Calculate the mass of a reactant or a product from the amount in moles of a different reactant or product. Section 2 Ideal Stoichiometric Calculations

5. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Objectives, continued Calculate the amount in moles of a reactant or a product from the mass of a different reactant or product. Calculate the mass of a reactant or a product from the mass of a different reactant or product. Section 2 Ideal Stoichiometric Calculations

6. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Conversions of Quantities in Moles Section 2 Ideal Stoichiometric Calculations

7. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Visual Concepts Click below to watch the Visual Concept. Visual Concept Conversion of Quantities in Moles http://my.hrw.com/sh/hc6_003036809x/ student/ch09/sec02/vc00/hc609_02_v00 fs.htm

8. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Solving Mass-Mass Stoichiometry Problems Section 2 Ideal Stoichiometric Calculations

9. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Conversions of Quantities in Moles, continued Sample Problem A In a spacecraft, the carbon dioxide exhaled by astronauts can be removed by its reaction with lithium hydroxide, LiOH, according to the following balanced chemical equation. CO 2 (g) + 2LiOH(s) → Li 2 CO 3 (s) + H 2 O(l) How many moles of lithium hydroxide are required to react with 20 mol CO 2, the average amount exhaled by a person each day? Section 2 Ideal Stoichiometric Calculations

10. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Conversions of Quantities in Moles, continued Sample Problem A Solution CO 2 (g) + 2LiOH(s) → Li 2 CO 3 (s) + H 2 O(l) Given: amount of CO 2 = 20 mol Unknown: amount of LiOH (mol) Solution: mol ratio Section 2 Ideal Stoichiometric Calculations

11. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Practice problems pg. 306 Write the balanced equation for practice problems pg. 306 and answer the question in your notes.

12. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 ANSWERS Practice problems pg. 306 Write the balanced equation for practice problems pg. 306 and answer the question in your notes. Make sure you understand why.

13. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Conversions of Amounts in Moles to Mass Section 2 Ideal Stoichiometric Calculations

14. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Solving Stoichiometry Problems with Moles or Grams Section 2 Ideal Stoichiometric Calculations

15. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Conversions of Amounts in Moles to Mass, continued Sample Problem B In photosynthesis, plants use energy from the sun to produce glucose, C 6 H 12 O 6, and oxygen from the reaction of carbon dioxide and water. What mass, in grams, of glucose is produced when 3.00 mol of water react with carbon dioxide? Section 2 Ideal Stoichiometric Calculations

16. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Conversions of Amounts in Moles to Mass, continued Sample Problem B Solution Given: amount of H 2 O = 3.00 mol Unknown: mass of C 6 H 12 O 6 produced (g) Solution: Balanced Equation: 6CO 2 (g) + 6H 2 O(l) → C 6 H 12 O 6 (s) + 6O 2 (g) mol ratio molar mass factor 90.1 g C 6 H 12 O 6 Section 2 Ideal Stoichiometric Calculations

17. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Practice problems pg. 308 Write the balanced equation for practice problems pg. 308 #1-2 and answer the question in your notes.

18. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 ANSWERS Practice problems pg. 308 Write the balanced equation for practice problems pg. 308 #1-2 and answer the question in your notes. Make sure you understand why.

19. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Conversions of Mass to Amounts in Moles Section 2 Ideal Stoichiometric Calculations

20. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Visual Concepts Click below to watch the Visual Concept. Visual Concept Mass and Number of Moles of an Unknown http://my.hrw.com/sh/hc6_00303680 9x/student/ch09/sec02/vc01/hc609_0 2_v01fs.htm

21. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Conversions of Mass to Amounts in Moles, continued Sample Problem D The first step in the industrial manufacture of nitric acid is the catalytic oxidation of ammonia. NH 3 (g) + O 2 (g) → NO(g) + H 2 O(g) (unbalanced) The reaction is run using 824 g NH 3 and excess oxygen. a. How many moles of NO are formed? b. How many moles of H 2 O are formed? Section 2 Ideal Stoichiometric Calculations

22. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Conversions of Mass to Amounts in Moles, continued Sample Problem D Solution Given: mass of NH 3 = 824 g Unknown:a. amount of NO produced (mol) b. amount of H 2 O produced (mol) Solution: Balanced Equation: 4NH 3 (g) + 5O 2 (g) → 4NO(g) + 6H 2 O(g) a. b. molar mass factor mol ratio Section 2 Ideal Stoichiometric Calculations

23. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Conversions of Mass to Amounts in Moles, continued Sample Problem D Solution, continued a. b. molar mass factor mol ratio Section 2 Ideal Stoichiometric Calculations

24. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Practice problems pg. 309 Write the balanced equation for practice problems pg. 309 #1-2 and answer the question in your notes.

25. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 ANSWERS Practice problems pg. 309 Write the balanced equation for practice problems pg. 309 #1-2 and answer the question in your notes. Make sure you understand why.

26. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Mass-Mass to Calculations Section 2 Ideal Stoichiometric Calculations

27. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Visual Concepts Click below to watch the Visual Concept. Visual Concept Mass-Mass Calculations http://my.hrw.com/sh/hc6_003036809x/stu dent/ch09/sec02/vc02/hc609_02_v02fs.htm

28. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Solving Mass-Mass Problems Section 2 Ideal Stoichiometric Calculations

29. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Mass-Mass to Calculations, continued Sample Problem E Tin(II) fluoride, SnF 2, is used in some toothpastes. It is made by the reaction of tin with hydrogen fluoride according to the following equation. Sn(s) + 2HF(g) → SnF 2 (s) + H 2 (g) How many grams of SnF 2 are produced from the reaction of 30.00 g HF with Sn? Section 2 Ideal Stoichiometric Calculations

30. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Mass-Mass to Calculations, continued Sample Problem E Solution Given: amount of HF = 30.00 g Unknown: mass of SnF 2 produced (g) Solution: molar mass factor mol ratio molar mass factor = 117.5 g SnF 2 Section 2 Ideal Stoichiometric Calculations

31. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Practice Problems p.311 #1-3 Write a balanced equation before answering questions.

32. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Practice Problems p.311 #1-3 ANSWERS

33. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Section 2 Ideal Stoichiometric Calculations Solving Various Types of Stoichiometry Problems

34. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Solving Various Types of Stoichiometry Problems Section 2 Ideal Stoichiometric Calculations

35. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Solving Volume-Volume Problems Section 2 Ideal Stoichiometric Calculations

36. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Solving Particle Problems Section 2 Ideal Stoichiometric Calculations

37. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 9 Visual Concepts Click below to watch the PROBLEM ACTIVITIES MASS TO MOLES PROBLEM Ideal Stoichiometric Calculations MOLES TO MASS PROBLEM MOLES TO MASS #2 MASS TO MASS PROBLEM CALCULATING MOLES REACTED

38. © Copyright Pearson Prentice Hall Slide of 25 End Show Online Self-Check Quiz Complete the online Quiz and record answers. Ask if you have any questions about your answers. click here for online Quiz 9.2 (7 questions) You must be in the “Play mode” for the slideshow for hyperlink to work.

39. © Copyright Pearson Prentice Hall Slide of 28 End Show VIDEOS FOR ADDITIONAL INSTRUCTION Additional Videos for Section 9.2: Ideal Stoichiometric Calculations None at this time

40. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu End of Chapter 9.2 Show