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Week 25 Chemistry

Week 25 Chemistry. Stoichiometry. Write the Learning Target. Warm Up: 7 Minutes. Stay in your own seat. You should be working SILENTLY. Classify each of the following reactions. Explain how you know using specific parts of the reaction. 2 C 2 H 6 + 7 O 2  4 CO 2 + 6 H 2 O

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Week 25 Chemistry

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  1. Week 25 Chemistry Stoichiometry

  2. Write the Learning Target Warm Up: 7 Minutes Stay in your own seat You should be working SILENTLY Classify each of the following reactions. Explain how you know using specific parts of the reaction. 2 C2H6 + 7 O2 4 CO2 + 6 H2O H2+ Cl2 2 HCl 2 AgNO3 + Ni  Ni(NO3)2 + 2 Ag Fe(OH)2FeO + H2O 2 NH4Cl + Hg(C2H3O2)2  2 NH4C2H3O2 + HgCl2

  3. Agenda • Warm Up [12 minutes] • Chemical Reactions Essay [38 minutes] • Closing[3 Minutes]

  4. About the Prompt • Every year, you are required to create a writing sample in your classes • This is the day for our prompt in Chemistry

  5. Expectations • It should be SILENT during the writing time • This means no talking, noises, or being out of your seat.

  6. Close all laptops Your Prompt On your provided handout, answer the prompt below: Two chemical reactions are shown below. Zn + 2 HCl ZnCl2 + H2 FeS + 2HCl  FeCl2 + H2S Write an essay that addresses the following to receive full credit: • Why are all chemical reactions considered to be chemical changes? • Classify each reaction and provide support for its classification. • How are the given reactions similar to each other and how are these reactions different from each other?

  7. Closing • How do you feel about types of reactions?

  8. Write the Learning Target Warm Up: 4 Minutes Stay in your assigned seat You should be working SILENTLY Calculate the molar mass of the following compounds: Hint: add the masses of the elements… N2O3 Ba(OH)2

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

  10. What have we learned so far? Mole to Mole Mole X  Mole Y

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

  12. You will need… • Periodic Table • Calculator

  13. Guaranteed method for success How to Perform Stoichiometry Mole to Mass problems? WRITE and BALANCE the equation Write down GIVEN number AND unit Write down MOLE RATIO with UNKNOWN on top and GIVEN on bottom Use MOLAR MASS of the unknown to solve for grams MULTIPLY the numbers on TOP DIVIDE by the numbers on the BOTTOM

  14. Example 1 Step 1: Write and Balance the Equation Step 2: Write down GIVEN number AND unit Step 4: Use MOLAR MASS of the unknown to solve for grams Step 6:DIVIDE by the numbers on the BOTTOM Step 5:MULTIPLY the numbers on TOP Step 3:Write down MOLE RATIO with UNKNOWN on top and GIVEN on bottom Iron reacts with Oxygen to form Iron (III) Oxide. How much (mass) of Oxygen gas was produced from 4 moles of Iron (III) Oxide? ___Fe + ___O2 ___Fe2O3

  15. Example 2 When an electrical current is passed through a sample of water, hydrogen and oxygen gases formed. Determine the mass of water required to decompose to form 3.4 moles of hydrogen. ___H2O  ___H2 + ___O2

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

  17. Guided Practice #1 Hydrogen and nitrogen gases react to form ammonia by the reaction below: ___H2 + ___N2 ___NH3 If 0.99 moles of ammonia are formed, determine the mass in grams of hydrogen gas that reacted. 3.0 grams H2

  18. Guided Practice #2 Potassium metal reacts with chlorine gas to produce potassium chloride by the reaction below: ___K + ___Cl2 ___KCl If 4.50 moles of chlorine reacts, how many grams of potassium chloride are produced? 671 grams KCl

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

  20. Closing • Describe the process used to solve mole to mass stoichiometry problems

  21. Write the Learning Target Warm Up: 4 Minutes Stay in your own seat You should be working SILENTLY When an electrical current is passed through a sample of water, hydrogen and oxygen gases formed. Determine the mass in grams of oxygen required to decompose to form 12 moles of water. ___H2O  ___H2 + ___O2

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

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

  24. Example 1 How many moles of O2 are required to react with 400g of C4H10? 2 C4H10 + 13 O2 8 CO2 + 10 H2O

  25. Example 2 How many moles of copper are required to form 163.0 grams of nitrogen monoxide, assuming an excess of nitric acid? 3 Cu + 8 HNO3 3 Cu(NO3)2 + 4 H2O + 2 NO

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

  27. Guided Practice #1 Water and nitrogen monoxide are produced from the reaction of ammonia and oxygen according to the reaction below: 4 NH3 + 5 O2 6 H2O + 4 NO If 37.2 grams of NH3 are reacted, how many moles of water are produced? 3.28 moles H2O

  28. Guided Practice #2 Sodium hydroxide and sulfuric acid react to form water and sodium sulfate according to the reaction below: 2 NaOH + H2SO4 2 H2O + Na2SO4 If you start with 2.41 moles of sodium hydroxide and an excess of sulfuric acid, how many grams of sodium sulfate will be formed? 171 grams Na2SO4

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

  30. Closing • Describe the process of converting from mass to mole. • How do you distinguish between mass to mole and mole to mass?

  31. Write the Learning Target Warm Up: 5 Minutes Stay in your own seat You should be working SILENTLY Calculate the number of moles of NH3 produced by the reaction of 6.2 grams of hydrogen with an excess of nitrogen. N2 + 3 H2 2 NH3

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

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

  34. Example 1 Calculate the number of grams of NH3 produced by the reaction of 5.40g of hydrogen with an excess of nitrogen. The balanced equation is N2 + 3 H2 2 NH3

  35. Example 2 Acetylene gas (C2H2) is produced by adding water to calcium carbide (CaC2). How many grams of acetylene are produced by adding water to 5.00 grams CaC2? CaC2 + 2 H2O  C2H2 + Ca(OH)2

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

  37. Guided Practice #1 The combustion of acetylene follows the reaction shown below: 2 C2H2 + 5 O2 4 CO2 + 2 H2O If 52.00 grams of C2H2 are burned, how many grams of oxygen are required? 159.8 grams O2

  38. Guided Practice #2 Lithium nitride reacts with water to form ammonia and lithium hydroxide: Li3N + 3 H2O  NH3 + 3LiOH What mass of water is required to react with 32.9 grams of Li3N? 51.1 grams H2O

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

  40. Closing • What steps would you take to perform a mass to mass stoichiometry problem?

  41. Write the Learning Target Warm Up: 7 Minutes Stay in your own seat You should be working SILENTLY Barium Chloride reacts with Silver (I) Nitrate to form Barium Nitrate and Silver (I) Chloride. ___BaCl2 + ___AgNO3 ___Ba(NO3)2 + ___AgCl If 115.4 grams of barium chloride are consumed, how many grams of silver (I) chloride are produced?

  42. Agenda • Warm Up [11 minutes] • Quiz [30 minutes] • Closing[4 Minutes]

  43. Material Covered on Quiz • All types of Stoichiometry! • Mole to Mole • Mole to Mass • Mass to Mole • Mass to Mass

  44. Goal • To demonstrate mastery, we are shooting for 85%

  45. Check Point What is your goal for this quiz? 85%

  46. Expectations for Quiz Clear your desk of everything except a.... • Writing Utensil • Calculator Periodic Table will be provided to you

  47. Expectations • Students will keep eyes on own paper • Cheating will result in an automatic ZERO • Students will remain SILENT for the duration of the quiz

  48. Good Luck!!

  49. Closing • How was your Quiz Today? • What topics do you feel you still need review on?

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