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Entry Task: Feb 27 th -28 th Block #1

Entry Task: Feb 27 th -28 th Block #1. Grab New Entry task sheet Write the question down What are the mole ratios for this reaction? Be sure to label 2H 2 + O 2  2H 2 O You have 5 minutes!. Agenda:. Sign off and Discuss Ch. 12.1 reading notes Stoichiometry notes#1. I can….

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Entry Task: Feb 27 th -28 th Block #1

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  1. Entry Task: Feb 27th -28th Block #1 Grab New Entry task sheet Write the question down What are the mole ratios for this reaction? Be sure to label 2H2 + O2 2H2O You have 5 minutes!

  2. Agenda: • Sign off and Discuss Ch. 12.1 reading notes • Stoichiometry notes#1

  3. I can… • Identify the quantitative relationship in a balanced chemical equation • Determine the mole ratios from a balanced chemical reaction

  4. Stoichiometry • Stoichiometry is based on law of conservation of mass The law of conservation of mass states that the mass of reactants in a chemical reaction will equal the mass of products produced from that reaction.

  5. Stoichiometry • Write the reaction for iron reacting with oxygen 4Fe (s) + 3O2 (g)  2Fe2O3 (s) • What do the coefficients represent? The represent the number of moles of that particular substance

  6. Stoichiometry • So in our Iron reacting with oxygen reaction, there are ____moles of iron reacting with ____moles of oxygen to produce ____ moles of Iron II oxide. 4 3 2

  7. Stoichiometry • We can change the number of moles (along with the molecular mass) to calculate this in to grams. 4Fe (s) + 3O2 (g)  2Fe2O3 (s) How many grams of iron are reacting in this equation? Convert from mole to gram.- Show work below. Fe= 55.85 g x 4 = 223.4 g 55.85 g of Fe 4 moles of Fe = 223.4g of Fe 1 moles of Fe

  8. Stoichiometry 4Fe (s) + 3O2 (g)  2Fe2O3 (s) How many grams of oxygen are reacting in this equation? Convert from mole to gram.- Show work below. O= 15.99 g x 6 = 95.99 g 31.99 g of O2 3 moles of O2 = 95.99 g of O2 1 moles of O2

  9. Stoichiometry 4Fe (s) + 3O2 (g)  2Fe2O3 (s) How many grams of iron II oxide are reacting in this equation? Convert from mole to gram.- Show work below. Fe2O3= (Fe x 4) 223.4 g + (O x 6) 95.99 g = 319.39 g 2 moles of Fe2O3 159.69 g of Fe2O3 = 319.39 g of O2 1 moles of Fe2O3

  10. Stoichiometry • Mole Ratio: Is the ratio between the number of moles of any two substances in a balanced chemical equation Read through the Aluminum + bromine reaction- note the mole ratio relationships between reactants and between reactants and products.

  11. Stoichiometry • Practice Problems- Determine all possible the mole ratios for the following. 1. 4Al(s) + 3O2 (g)  2Al2O3 (s) What is the ratio between aluminum and oxygen? Answer: 4 mol of Al to 3 mol of O2OR 3 mol of O2 to 4 mol of Al

  12. Stoichiometry • Practice Problems- Determine all possible the mole ratios for the following. 1. 4Al(s) + 3O2 (g)  2Al2O3 (s) What is the ratio between aluminum and aluminum oxide? Answer: 4 mol of Al to 2 mol of Al2O3OR 2 mol of Al2O3 to 4 mol of Al

  13. Stoichiometry • Practice Problems- Determine all possible the mole ratios for the following. 1. 4Al(s) + 3O2 (g)  2Al2O3 (s) What is the ratio between oxygen and aluminum oxide? Answer: 3 mol of O2 to 2 mol of Al2O3OR 2 mol of Al2O3 to 3 mol of O2

  14. Chocolate Chip Cookies!! 1 cup butter 1/2 cup white sugar 1 cup packed brown sugar 1 teaspoon vanilla extract 2 eggs 2 1/2 cups all-purpose flour 1 teaspoon baking soda 1 teaspoon salt 2 cups semisweet chocolate chips Makes 3 dozen How many eggs are needed to make 3 dozen cookies? How much butter is needed for the amount of chocolate chips used? How many eggs would we need to make 9 dozen cookies? How much brown sugar would I need if I had 1 cup white sugar? 2 eggs 1 cup 6 eggs 2 cup

  15. Cookies and Chemistry…Huh!?!? • Just like chocolate chip cookies have recipes, chemists have recipes as well. • Instead of calling them recipes, we call them reaction equations • Furthermore, instead of using cups and teaspoons, we use moles. • Lastly, instead of eggs, butter, sugar, etc. we use chemical compounds as ingredients.

  16. Stoichiometry • Stoichiometry is the study of quantitative relationships between amounts of reactants and products formed by a chemical reaction- RATIOS!!. ___H2(g) + ___O2 (g) ___H2O (l) 2 2 For this reaction, 2 moles of hydrogen gas reacts with 1 mole of oxygen gas to create 2 moles of water molecules.

  17. Balance: ___H2(g) + ___O2 (g) ___H2O (l) 2 2 Translate into written equation: 2 moles of hydrogen gas reacts with 1 mole of oxygen gas to produce 2 moles of water What is the ratio of hydrogen gas to oxygen gas? 2 : 1 What is the ratio of oxygen gas to water? 1 : 2 What is the ratio of hydrogen gas to water? 2 : 2 What is the ratio of water to oxygen gas? 2 : 1

  18. Mole ratio Mole ratio Mole ↔ mole 2H2(g) + O2(g) 2H2O(l) a. How many moles of H2 were used if 4 moles of H2O were produced? Units match 2 mol H2 4 mol H2O = moles H2 4 2 mol H2O b. How many moles of H2were used if 0.356 moles of H2O were produced? Units match 0.356 molH2O 2 molH2 = moles H2 0.356 2 mol H2O

  19. Mole ratio Mole ratio Mole ↔ mole 2H2(g) + O2(g) 2H2O(l) c. How many moles of O2 were used if 2.36 moles of H2O were produced? Units match 2.36 molH2O 1 mol O2 = moles O2 1.18 2 mol H2O d. How many moles of H2O were produced if 36.9 moles of H2 were used? Units match 2 mol H2O 36.9 mol H2 36.9 = moles H2O 2 mol H2

  20. You Try!! Silver metal reacts with sulfur solid (S8) to create silver I sulfide. Provide a balanced equation below! 1. Formula of each substance, then set up equation, lastly balance the equation.

  21. You Try!! Silver metal reacts with sulfur solid (S8) to create silver I sulfide. Provide a balanced equation below! 1. Formula of each substance, then set up equation, lastly balance the equation. ___ Ag

  22. You Try!! Silver metal reacts with sulfur solid (S8) to create silver I sulfide. Provide a balanced equation below! 1. Formula of each substance, then set up equation, lastly balance the equation. ___Ag + ___S8

  23. You Try!! Silver metal reacts with sulfur solid (S8) to create silver I sulfide. Provide a balanced equation below! 1. Formula of each substance, then set up equation, lastly balance the equation. ___Ag2S ___Ag + ___S8

  24. You Try!! Silver metal reacts with sulfur solid (S8) to create silver I sulfide. Provide a balanced equation below! 1. Formula of each substance, then set up equation, lastly balance the equation. ___Ag2S ___Ag + ___S8 16 8

  25. You Try!! Silver metal reacts with sulfur solid (S8) to create silver I sulfide 16Ag + S8  8Ag2S a. How many moles of S8 were used if 36 moles of Ag2S were produced? WHY did I balance the equation? To get the mole ratios

  26. You Try!! Silver metal reacts with sulfur solid (S8) to create silver I sulfide 16Ag + S8  8Ag2S a. How many moles of S8 were used if 36 moles of Ag2S were produced? 36 molAg2S Now What? Put starting amounts WITH label in correct spot

  27. 1 mole S8 8 moles Ag2S 8 moles Ag2S 1 mole S8 You Try!! Silver metal reacts with sulfur solid (S8) to create silver I sulfide 16Ag + S8  8Ag2S a. How many moles of S8 were used if 36 moles of Ag2S were produced? What mole ratio would I use in this problem?

  28. 1 mole S8 8 moles Ag2S You Try!! Silver metal reacts with sulfur solid (S8) to create silver I sulfide 16Ag + S8  8Ag2S a. How many moles of S8 were used if 36 moles of Ag2S were produced? WHY this ratio? 1 mole S8needs to be on top because that is what the question is asking for.

  29. 1 mole S8 8 moles Ag2S You Try!! Silver metal reacts with sulfur solid (S8) to create silver I sulfide 16Ag + S8  8Ag2S a. How many moles of S8 were used if 36 moles of Ag2S were produced? 36 mol Ag2S

  30. Mole ratio You Try!! Silver metal reacts with sulfur solid (S8) to create silver I sulfide 16Ag + S8  8Ag2S a. How many moles of S8 were used if 36 moles of Ag2S were produced? Units match 1 mol S8 36 mol Ag2S = moles S8 4.5 8 mol Ag2S

  31. Mole ratio You Try!! Silver metal reacts with sulfur solid (S8) to create silver I sulfide 16Ag + S8  8Ag2S b. How many moles of Ag2S were produced if 7 moles of Ag were used? Units match 8 mol Ag2S 7 mol Ag 3.5 = moles Ag2S 16 mol Ag

  32. Stoichiometry- Grams ___H2(g) + ___O2 (g) ___H2O (l) 2 2 What is the molar mass of hydrogen gas? 4.028 g What is the molar mass of water? 36.026 g What is the molar mass of oxygen gas? 31.998 g

  33. gram ↔ mole a. How many moles of H2 were used if 72.0g of H2O were produced? 2H2(g) + O2(g) 2H2O(l) ? moles 72.0g Units match 72.0 g H2O 1 mol H2O 2 mol H2 = moles H2 4.00 18 g H2O 2 mol H2O Mole/Gram conversion Mole/Mole ratio 72 X 2 = 144 18 X 2 = 36

  34. gram ↔ mole b. How many moles of H2O were produced if 36.5gof H2 were used? 2H2(g) + O2(g) 2H2O(l) 36.5 g ? moles Units match 36.5 g H2 1 mol H2 2 mol H2O = moles H2O 18.1 2.014 g H2 2 mol H2 Mole/Gram conversion Mole/Mole ratio 36.5 X 2 = 73 2.014 X 2 = 4.028

  35. You Try! Aluminum metal reacts with bromine gas to create aluminum bromide. Provide balanced equation below! 2Al + 3Br2  2AlBr3

  36. You Try! a. How many moles of AlBr3 were produced if 65.5g of Br2 were used? 2Al + 3Br2  2AlBr3 65.5 g ? moles Units match 65.5 g Br2 1 mol Br2 2 mol AlBr3 = moles AlBr3 0.273 159.808g Br2 3 mol Br2 Mole/Gram conversion Mole/Mole ratio 65.5 X 2 = 131 159.808 X 3 = 479.424

  37. You Try! b. How many moles of Al were used if 125g of AlBr3 were produced? 2Al + 3Br2  2AlBr3 ? moles 125 g Units match 125 g AlBr3 1 mol AlBr3 2 mol Al = moles Al 0.469 266.69 g AlBr3 2 mol AlBr3 Mole/Gram conversion Mole/Mole ratio 125 X 2 = 250 266.69 X 2 = 533.38

  38. Moles Grams a. How many grams of AlBr3 were produced if 2.35 moles of Al were used? 2Al + 3Br2  2AlBr3 2.35 moles ? grams Units match 2.35 moles Al 2 mol AlBr3 266.69 g AlBr3 = grams AlBr3 627 2 mol Al 1 molAlBr3 Mole/Mole ratio Mole/Gram conversion 2.35 X 2 X 266.69 = 1253.443 2

  39. Moles Grams a. How many grams of Br2 were used if 5.75 moles AlBr3 were produced? 2Al + 3Br2  2AlBr3 ? grams 5.75 moles Units match 5.75 moles AlBr3 3 mol Br2 159.808 g Br2 = grams Br2 1378 2 mol AlBr3 1 molBr2 Mole/Mole ratio Mole/Gram conversion 1380 5.75 X 3 X 159.808 = 2744.13 2

  40. You Try! YOU TRY! Gold III sulfide reacts with hydrogen gas to create gold metal and dihydrogenmonosulfide Provide balanced equation below! __Au2S3+ __H2 __Au + __ H2S

  41. You Try! YOU TRY! Gold III sulfide reacts with hydrogen gas to create gold metal and dihydrogenmonosulfide Provide balanced equation below! Au2S3+ 3H2 2Au + 3H2S

  42. Moles Grams a . How many grams of H2S were produced 3.25 moles of hydrogen gas were used? Au2S3 + 3H2  2Au + 3H2S 3.25 moles ? grams Units match 3.25 moles H2 3 mol H2S 34.06 g H2S = grams H2S 111 3 mol H2 1 molH2S Mole/Mole ratio Mole/Gram conversion 3.25 X 3 X 34.06 = 332.085 3

  43. Moles Grams b . How many grams of H2 were needed to react with 3.25 moles of gold III sulfide? Au2S3 + 3H2  2Au + 3H2S 3.25 moles ? grams Units match 3.25 moles Au2S3 3 mol H2 2.014 g H2 = grams H2 19.6 1 molAu2S3 1 molH2 Mole/Mole ratio Mole/Gram conversion 3.25 X 3 X 2.014 = 19.6 1

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