1. What is Stoichiometry? Objectives: 6.0 Solve stoichiometric problems involving relationships among the number of particles, moles, and masses of reactants and products in a chemical reaction 6.3 Identifying the nomenclature of ionic compounds, binary compounds, and acids 6.4 Classifying chemical reactions as composition, decomposition, single replacement, or double replacement Other AOD C.6.1 Define stoichiometry, reactants, and products. Other AOD C.6.2 Explain the law of conservation of mass. Other AOD C.6.3 Explain the concept of mole in terms of Avogadro's number.

2. Stoichiometry Def.: the quantitative study of relationships between amounts of reactants used and products formed in a chemical reaction Let’s think for a moment. If I hand you a dozen chocolate chips, can you make a dozen chocolate chip cookies? Well, every chemical equation is just a recipe!

3. Let’s Review! Iron + oxygen react to produce iron (III) oxide. 1.Write AND BALANCE the chemical equation. ANSWER: 4 Fe(s) + 3O 2 (g)→ 2Fe 2 O 3 (s) 2.What type of reaction is this? 3.How many moles of each compound are represented? 4.How many grams of each compound are represented?

4. Review, continued….. Aluminum + bromine react to produce aluminum bromide 1.Write AND BALANCE the chemical equation. ANSWER: 2Al(s) + 3Br 2 (l)→ 2AlBr 3 (s) 2.What type of reaction is this? 3.How many moles of each compound are represented? 4.How many grams of each compound are represented?

5. Review – 1 More! Propane (C 3 H 8 ) and oxygen react to produce carbon dioxide and water. 1.Write AND BALANCE the chemical equation. ANSWER: C 3 H 8 (g) + 5O 2 (g)→ 3CO 2 (g) + 4H 2 O 2.What type of reaction is this? 3.How many moles of each compound are represented? 4.How many grams of each compound are represented?

6. Law of Conservation of Mass In every example, mass was conserved, meaning the mass of the reactants EQUALS the mass of the products! While mass was equal on both sides of the equations, what was different? ANSWER: number of molecules or number of moles

7. Assignment Let’s look at Example Problem 12-1 on p.355. (This is the last equation we balanced.) Notice how they write the equation “in terms of” molecules, moles, and mass. Now do the Practice Problems on p.356 --- - ONLY demonstrating conservation of mass, not the rest of the directions.

8. Mole Ratios Def.: the ratio of the number of moles of any two substances in a balanced chemical equation. Let’s look back at the 3 equations we balanced. In the first one, we can identify several mole ratios: –4Fe/3O 2 OR 3O 2 /4Fe –4Fe/2Fe 2 O 3 OR 2Fe 2 O 3 /4Fe –3O 2 /2Fe 2 O 3 OR 2Fe 2 O 3 /3O 2

9. Mole Ratios, continued….. What are the possible mole ratios for the other two example problems we worked? Assignment: 1.Practice Problems (p.357) 2.Study Guide for Content Mastery: pp.67-68