1. BRN  Complete the table using the balanced chemical reaction: ______CH 4 + ______O 2  _____CO 2 + _____H 2 O  Complete the table using the balanced chemical reaction: ______CH 4 + ______O 2  _____CO 2 + _____H 2 O Molecules CH 4 Molecules O 2 → Molecules CO 2 Molecules H 2 O 4.0→ →5.0

2. Stoichiometry Notes New Section in Table of Contents

3. Real Life Application Ingredients  2 1/4 cups all-purpose flour  1 teaspoon baking soda  1 teaspoon salt  1 cup (2 sticks) butter, softened  3/4 cup granulated sugar  3/4 cup packed brown sugar  1 teaspoon vanilla extract  2 large eggs  2 cups (12-oz. pkg.) NESTLÉ® TOLL HOUSE® Semi-Sweet Chocolate Morsels  1 cup chopped nuts Ingredients  2 1/4 cups all-purpose flour  1 teaspoon baking soda  1 teaspoon salt  1 cup (2 sticks) butter, softened  3/4 cup granulated sugar  3/4 cup packed brown sugar  1 teaspoon vanilla extract  2 large eggs  2 cups (12-oz. pkg.) NESTLÉ® TOLL HOUSE® Semi-Sweet Chocolate Morsels  1 cup chopped nuts

4. Real Life Application  We cannot forget about the law of conservation of mass.  The mass of what we put in must be equal to what we get out.  KC 1: The excess reactants are all the leftover unused reactants. (The reactant that’s leftover).  We cannot forget about the law of conservation of mass.  The mass of what we put in must be equal to what we get out.  KC 1: The excess reactants are all the leftover unused reactants. (The reactant that’s leftover).

5. Particle and Mole Relationships  Chemical reactions stop when one of the reactants is used up  KC 2: Stoichiometry is the study of quantitative relationships between the amounts of reactants used and amounts of products formed by a chemical reaction  So based on how much reactant you put in you can calculate how much product you will get out  Chemical reactions stop when one of the reactants is used up  KC 2: Stoichiometry is the study of quantitative relationships between the amounts of reactants used and amounts of products formed by a chemical reaction  So based on how much reactant you put in you can calculate how much product you will get out

6. Particle and Mole Relationships

7.  KC 3: A mole ratio is a ratio between the numbers of moles of any 2 substances in a balanced equation  This can only be determined from a balanced chemical equation  KC 3: A mole ratio is a ratio between the numbers of moles of any 2 substances in a balanced equation  This can only be determined from a balanced chemical equation

8. Particle and Mole Relationships  Let practice: What is the mole-to-mole ratio for…  10C 2 H 4 O + 15O 2  20CO 2 + 2H 2 O  CH 4 + 2O 2  CO 2 + 2H 2 O  H 2 + O 2  H 2 O  Let practice: What is the mole-to-mole ratio for…  10C 2 H 4 O + 15O 2  20CO 2 + 2H 2 O  CH 4 + 2O 2  CO 2 + 2H 2 O  H 2 + O 2  H 2 O

9. Using Stoichiometry CH 4 + 2O 2  CO 2 + 2H 2 O Mol CH 4 Mole H 2 O

10. Using Stoichiometry Key Concept 4: How many moles of SO 3 are formed if you start with 5.25 moles of Sulfur and have excess Oxygen? ____S + ____O 2  ____SO 3 Key Concept 4: How many moles of SO 3 are formed if you start with 5.25 moles of Sulfur and have excess Oxygen? ____S + ____O 2  ____SO 3

11. Using Stoichiometry Key Concept 5: How many moles of SO 3 are formed if you start with 0.25 moles of oxygen and have excess sulfur? ____S + ____O 2  ____SO 3 Key Concept 5: How many moles of SO 3 are formed if you start with 0.25 moles of oxygen and have excess sulfur? ____S + ____O 2  ____SO 3

12. Using Stoichiometry Key Concept 6: How many moles of water are formed if you start with 0.345 moles of CH 4 ? ______CH 4 + ______O 2 → _____CO 2 + _____H 2 O Key Concept 6: How many moles of water are formed if you start with 0.345 moles of CH 4 ? ______CH 4 + ______O 2 → _____CO 2 + _____H 2 O

13. Lab Introduction  Make your own soda!

14. Using Stoichiometry  How many grams of Fe 2 O 3 are formed when 12.37g of iron reacts with excess oxygen using the balanced chemical equation below: 4Fe(s) + 3O 2 (g)  2Fe 2 O 3 (s)

15. Using Stoichiometry 4Fe(s) + 3O 2 (g)  2Fe 2 O 3 (s) 12.37g Fe Mol Fe Mole Fe 2 O 3 ?? g Fe 2 O 3

16. Using Stoichiometry Key Concept 7: How many grams of lithium nitrate will be needed to make 250.0 grams of lithium sulfate, assuming that you have an adequate amount of lead (IV) sulfate to do the reaction? ____Pb(SO 4 ) 2 + ____LiNO 3  ____Pb(NO 3 ) 4 + ____Li 2 SO 4

17. Using Stoichiometry Key Concept 8: How many grams of sodium sulfate will be formed if you start with 20.0 grams of sodium hydroxide and you have an excess of sulfuric acid? ____NaOH + ____H 2 SO 4  ____H 2 O + ____Na 2 SO 4

18. Using Stoichiometry Key Concept 9: How many grams of water will be formed if you start with 200.0 grams of sodium hydroxide and you have an excess of sulfuric acid? ____NaOH + ____H 2 SO 4  ____H 2 O + ____Na 2 SO 4 Key Concept 9: How many grams of water will be formed if you start with 200.0 grams of sodium hydroxide and you have an excess of sulfuric acid? ____NaOH + ____H 2 SO 4  ____H 2 O + ____Na 2 SO 4

19. Practice  How many grams of CaCl 2 are formed when 21.3g of Ca(OH) 2 reacts with excess HCl? _____Ca(OH) 2 + _____HCl  ______CaCl 2 + ______H 2 O

20. Practice  How many grams of BaCl 2 are formed from 6.0 moles of Ba(ClO 3 ) 2 ? _______Ba(ClO 3 ) 2 → _______BaCl 2 + _____O 2

21. Practice  Iron(III) oxide, Fe 2 O 3, can be reduced to iron by passing carbon monoxide, CO, over the heated oxide. How many moles of iron can be produced from 1.234 moles of Fe 2 O 3 oxide and excess carbon monoxide? ______Fe 2 O 3(s) + _____CO (g)  _____Fe (s) ­ + _____CO 2(g)

22. Practice  Butyne, C 4 H 6, burns in the presence of oxygen in air to produce carbon dioxide, CO 2, and water H 2 O. How many moles of oxygen will be required to produce 45.99 moles of carbon dioxide? ______C 4 H 6 + ______O 2  ______CO 2 + ______H 2 O

23. Practice  The following reaction can be used to remove CO 2 breathed out by astronauts in a spacecraft. 2 LiOH + 1 CO 2 → 1 Li 2 CO 3 + 1 H 2 O a.How many grams of carbon dioxide can be removed by 5.5mol LiOH? b.How many grams of water could be produced from 2.23g of LiOH?

24. Practice  Calcium carbide, CaC 2, reacts with water to form acetylene. 1 CaC 2 + 2 H 2 O → 1 C 2 H 2 + 1 Ca(OH) 2 a.How many grams of water (H 2 O) are needed to react with 485g of CaC 2 ? b.How many grams of CaC 2 could make 23.6g C 2 H 2 ?

25. Practice  Oxygen can be prepared by heating potassium chlorate: 2 KClO 3 → 2 KCl + 3 O 2 a.What mass of O 2 can be made from heating 125g of KClO 3 ? b.How many grams of KCl could form from 20.8g KClO 3 ?

27. BRN  Complete the table using: N 2 + 3H 2 → 2NH 3 Moles N 2 Moles H 2 →Moles NH 3 Excess N 2 Excess H 2 1.54.0→ → 20

28. Limiting and Excess Reactants  KC 10: If you have 2 givens in your problem, it is a limiting reactant problem  KC 11: The reactant that produces the smallest amount of a product is the limiting reactant. This is the reactant that will be used up first in the reaction.  KC 10: If you have 2 givens in your problem, it is a limiting reactant problem  KC 11: The reactant that produces the smallest amount of a product is the limiting reactant. This is the reactant that will be used up first in the reaction.

29. Example  How many grams of Cu can be formed when 167.4 g of Fe reacts with 399.2 g of CuCl 2 ? 2 Fe + 3 CuCl 2  3 Cu + 2FeCl 3

30. Steps for solving LR problems  KC 12: 1.Write down the givens 2.Use molar mass to convert to moles 3.Use mole ratio from the balanced equation 4.Convert to desired unit 5.The correct answer is the smallest answer as the reaction will stop once one reactant is gone  KC 12: 1.Write down the givens 2.Use molar mass to convert to moles 3.Use mole ratio from the balanced equation 4.Convert to desired unit 5.The correct answer is the smallest answer as the reaction will stop once one reactant is gone

31. Limiting and Excess Reactant  KC 13: 80.0g Cu reacts with 25.0g S. Determine which is the limiting reactant and calculate how much Cu 2 S is formed in grams? 2Cu(s) + S(s) → Cu 2 S(s)

32.  KC 14: What is the limiting reactant if 65.0g of each reactant is present? ___Zn + ___HCl → ___ZnCl 2 + ___H 2 Limiting and Excess Reactant

33. Excess and Percent Yield  KC 15: To find how much excess you have you must take the limiting reactant and solve for the excess reactant. You need to look at what you are given versus what you need.

34. Excess Reactant - Example  How many grams of Cu can be formed when 167.4 g of Fe reacts with 399.2 g of CuCl 2 ? 2 Fe + 3 CuCl 2  3 Cu + 2FeCl 3 CuCl 2 – limiting reactant 188.5g Cu is formed  How many grams of excess is left over?  How many grams of Cu can be formed when 167.4 g of Fe reacts with 399.2 g of CuCl 2 ? 2 Fe + 3 CuCl 2  3 Cu + 2FeCl 3 CuCl 2 – limiting reactant 188.5g Cu is formed  How many grams of excess is left over?

35. Excess Reactant  KC 16: 24.5g of barium chloride reacts with 45.2g of sodium sulfate. Which is the limiting reactant and how much of the excess reactant is left over at the end of the reaction? ___BaCl 2 + ___Na 2 SO 4  ___BaSO 4 + ___NaCl

37. Percent Yield  KC 17: % yield = actual yieldx 100 theoretical yield  KC 18: Actual yield must be found experimentally. It is recognized by words like “produced” and “formed”  KC 19: Theoretical yield is done using stoichiometry. It is a prediction and will always be done using math.  KC 17: % yield = actual yieldx 100 theoretical yield  KC 18: Actual yield must be found experimentally. It is recognized by words like “produced” and “formed”  KC 19: Theoretical yield is done using stoichiometry. It is a prediction and will always be done using math.

38. Percent Yield  KC 20: A student calculated she should obtain 28g of a substance. In the experiment, 25g was produced. What is the percent yield of the experiment?

39. Percent Yield - Example  167.4 g of Fe reacts with 399.2 g of CuCl 2 to form 170.3g of copper. What is the percent yield of copper? 2 Fe + 3 CuCl 2  3 Cu + 2FeCl 3

40. Practice  KC 21: 11.2g of nickel (II) sulfide reacts with 5.43g of oxygen producing 4.97g of nickel (II) oxide. What is the percent yield of this reaction? _____NiS 2 + _____O 2 → _____NiO + _____SO 2

41. Practice  KC 22: You are given 0.45g of Al(OH) 3 and 0.55g of H 2 SO 4. The reaction produces 0.15g of water. What is the percent yield of this reaction? ____Al(OH) 3 + _____H 2 SO 4 → _____Al 2 (SO 4 ) 3 + _____H 2 O

42. Practice  KC 23: You are given 3 moles of lithium and 3 moles of nitrogen. The reaction produces.5 moles of lithium nitride. What is the percent yield of this reaction? ____Li + _____N 2 → _____Li 3 N