1. Daily Sciencepg. 78  You are heating copper sulfate in the lab. The mass of your test tube is 13.091g. You add 0.498 g of CuSO 4 to the test tube and re-mass the test tube plus the copper sulfate. Your new mass is 13.575 g. After heating the substance for 5 minutes you let it cool and re-mass. The final mass is 13.400 g. What is the formula for the hydrate?

2. STOICHIOMETRY Pg. 79

3. Stoichiometry  Chemical reactions stop when one of the reactants has been completely used  As a scientists, we need to know how much that is  Or we might need to know how much product will be made  Stoichiometry tells us this  Stoichiometry: The study of quantitative relationships between amounts of reactants used and products formed

4. Mole to mass relationships in chemical reactions  Coefficients in an equation tell you how many moles there are of each element  4 Fe(s) + 3 O 2  2Fe 2 O 3 (s)  You can calculate the grams of reactants and products by using stoichiometry (dimensional analysis)  Start with the number of moles of the element and convert to mass using molar mass  Accounts for conservation of mass

5. Practice Moles to mass  N 2 (g) + 3 H 2 (g)  2NH 3 (g)

6. Mole to mole ratios  Use the relationships between coefficients to write conversion factors; called mole ratios  4 Fe(s) + 3 O 2  2Fe 2 O 3 (s)  To determine how many mole ratios you can make, multiply the number of reactants and products by the next lowest number

7. Practice Mole to Mole ratios  2Al (s) + 3 Br 2 (l)  2AlBr 3 (s)

8. Using Stoichiometry – Mole to mole conversions  You must begin with a BALANCED chemical equation  You are given the amount of moles of a substance and you want to know how much of the other reactant you need or how much product will be formed  Start with the given and use mole to mole ratios  Given unit goes on bottom! Desired on top!  Ex. How many moles of hydrogen gas will be produced if you use 0.567 mol of potassium  2K (s) + 2 H 2 O (l)  2KOH (aq) + H 2 (g)

9. Practice using mole to mole conversions  How many moles of carbon dioxide are produced when 11.0 moles of propane (C 3 H 8 ) are burned?  C 3 H 8 (g) + O 2 (g)  CO 2 (g) + H 2 O (l)

10. Pg. 80  Practice problems pg. 356 1 c-e  Practice problems pg. 357 2 c and 3 a  Practice Problems pg. 359 9 and 10