1. Stoichiometry, Percent Yield, Unit 7 Review Week 26 Chemistry

2. Warm Up: 5 Minutes You should be working SILENTLY Stay in your own seat Calculate the number of moles of NH 3 produced by the reaction of 6.2 grams of hydrogen with an excess of nitrogen. N 2 + 3 H 2  2 NH 3 Write the Learning Target

3. Agenda  Warm Up [7 minutes]  Notes/Examples [15 minutes]  Guided Practice [12 minutes]  Independent Practice [17 minutes]  Closing [2 Minutes]

4. Today’s Stoichiometric focus Mass to Mass Mass X  Mole X  Mole Y  Mass Y

6. Example 1 Calculate the number of grams of NH 3 produced by the reaction of 5.40g of hydrogen with an excess of nitrogen. The balanced equation is N 2 + 3 H 2  2 NH 3

7. Acetylene gas (C 2 H 2 ) is produced by adding water to calcium carbide (CaC 2 ). How many grams of acetylene are produced by adding water to 5.00 grams CaC 2 ? CaC 2 + 2 H 2 O  C 2 H 2 + Ca(OH) 2 Example 2

9. Guided Practice  Teacher: 1. Will show the problem on the board  Students: 1. Take 27 seconds to read the problem and write your given and unknown 2. Take 88 seconds to solve the problem with your shoulder partner 3. Be ready to share when Mr. Ghosh says SWAG

11. Guided Practice #1 The combustion of acetylene follows the reaction shown below: 2 C 2 H 2 + 5 O 2  4 CO 2 + 2 H 2 O If 52.00 grams of C 2 H 2 are burned, how many grams of oxygen are required? 159.8 grams O 2

12. Guided Practice #2 Lithium nitride reacts with water to form ammonia and lithium hydroxide: Li 3 N + 3 H 2 O  NH 3 + 3 LiOH What mass of water is required to react with 32.9 grams of Li 3 N? 51.1 grams H 2 O

13. Independent Practice Take some time to practice some mass to mass stoichiometry Practice makes Perfect 85%

14. Closing  What steps would you take to perform a mass to mass stoichiometry problem?

15. Warm Up: 5 Minutes You should be working SILENTLY Stay in your own seat Calculate the number of grams of oxygen required to react with 11.4 grams of magnesium. 2 Mg + O 2  2 MgO Write the Learning Target Hint: Use your flowchart

17. Agenda  Warm Up [7 minutes]  Notes/Examples [15 minutes]  Guided Practice [12 minutes]  Independent Practice [17 minutes]  Closing [2 Minutes]

18. Today’s Stoichiometric focus Mole to Volume Mole X  Mole Y  Volume Y Volume to Mole Volume Y  Mole Y  Mole X

20. When Converting from Mole to Volume… Reaction has to take place at so you can use the following relationship… 22.4 L = 1 Mole STP (Standard Temperature and Pressure)!!!

21. Example 1 Determine the volume of chlorine gas needed react with calcium to produce 5.4 moles of calcium chloride at STP. Ca + Cl 2  CaCl 2

23. Example 2 The combustion of acetylene follows the reaction shown below: 2 C 2 H 2 + 5 O 2  4 CO 2 + 2 H 2 O Determine the number of moles of C 2 H 2 that reacted if 13L of carbon dioxide were produced at STP.

25. Guided Practice  Teacher: 1. Will show the problem on the board  Students: 1. Take 27 seconds to read the problem and write your given and unknown 2. Take 78 seconds to solve the problem with your shoulder partner 3. Be ready to share when Mr. Ghosh says SWAG

27. Guided Practice #1 Assuming STP, how many liters of oxygen are needed to produce 4.2 moles of sulfur trioxide? 2 SO 2 + O 2 → 2 SO 3 47 Liters O 2

29. Guided Practice #2 The following reaction is carried out at STP: 2 C 4 H 10 + 13 O 2  8 CO 2 + 10 H 2 O How many moles of C 4 H 10 reacted if 24.6L of carbon dioxide were produced? 0.275 moles C 4 H 10

30. Independent Practice Take some time to practice some mole to volume stoichiometry Practice makes Perfect 85%

31. Closing  Describe the process used to solve mole to volume stoichiometry problems

32. Wednesday at G/T Training…

33. Warm Up: 4 Minutes You should be working SILENTLY Stay in your own seat What volume of hydrogen gas is produced when 2.96 moles of zinc react? ___Zn + ___HCl  ___ZnCl 2 + ___H 2 Write the Learning Target

34. Agenda  Warm Up [7 minutes]  Flipped Classroom Video [6 minutes]  Notes/Examples [12 minutes]  Guided Practice [12 minutes]  Independent Practice [14 minutes]  Closing [2 Minutes]

35. The Flipped Classroom

36. Thoughts/Questions? I’m planning on trying this starting with our next unit

37. Vocabulary Words for Today Theoretical Yield: Actual Yield: Percent Yield: How much should be formed How much is actually formed

38. Example 1 Use the equation below to answer the following question: 8 Fe + S 8  8 FeS The theoretical yield of FeS is 29.4 grams. If 21.7 grams of FeS are produced from the reaction, what is the percent yield of FeS?

39. Example 2 In an experiment, 17.7 grams of water are formed from the reaction of 1.96 moles of hydrobromic acid. If the theoretical yield is 35.3 grams, what is the percent yield of water, to the nearest tenth of a percent? HBr + NaOH  NaBr + H 2 O

40. Guided Practice  Teacher: 1. Will show the problem on the board  Students: 1. Take 17 seconds to read the problem and write your given and unknown 2. Take 48 seconds to solve the problem with your shoulder partner 3. Be ready to share when Mr. Ghosh says SWAG

41. Guided Practice #1 Use the equation below to answer the following question: 2 FePO 4 + 3 Na 2 SO 4  Fe 2 (SO 4 ) 3 + 2 Na 3 PO 4 The theoretical yield of iron (III) sulfate is 33 grams. If 18.5 grams of iron (III) sulfate are produced from the reaction, what is the percent yield of iron (III) sulfate? 56%

42. Guided Practice #2 In an experiment, 366.7 grams of sodium sulfite are formed from the reaction of 1.322 moles of aluminum sulfite. If the theoretical yield is 499.9 grams, what is the percent yield of sodium sulfite, to the nearest tenth of a percent? Al 2 (SO 3 ) 3 + 6 NaOH  3 Na 2 SO 3 + 2 Al(OH) 3 73.4%

43. Independent Practice Take some time to practice some percent yield problems Practice makes Perfect 85%

44. Closing  Describe the process for finding percent yield

45. Warm Up: 3 Minutes You should be working SILENTLY Stay in your own seat In an experiment, 61.5 grams of iron (III) chloride are formed when 0.712 moles of hydrochloric acid reacts. If the theoretical yield is 120.1 grams, what is the percentage yield of iron (III) chloride, to the nearest tenth of a percent? 5 HIO 3 + 4 FeI 2 + 25 HCl  4 FeCl 3 + 13 ICl + 15 H 2 O Write the Learning Target

46. Agenda  Warm Up: 5 Minutes  Expectations for Stations: 3 minutes  Stations Review: 36 minutes  Closing: 1 Minute

47. How Will Stations Work?? You will be placed with a group of other scholars to complete five stations on the following topics:  Station 1: Mole to Mole Stoichiometry  Station 2: Mole to Volume Stoichiometry  Station 3: Mole to Mass Stoichiometry  Station 4: Mass to Mole Stoichiometry  Station 5: Mass to Mass Stoichiometry You Need: Periodic Table Flowchart

48. How Will Stations Work?? You will spend 7 minutes at each station working each problem as a group on scratch paper. You will write your FINAL answer on the answer document. When time is called, you will leave your current station and move on to the next station You will have 10 seconds to move to the next station

49. Closing  Why did we review these concepts?  Why is it important that everybody master these objectives?