1. Stoichiometry

2.  Describes the mass and mole relationships in a chemical reaction  Use it to predict the amount of product formed or the amount of reactant needed in a particular reaction

3. 1. How many moles of each product are formed: Sodium Chloride  Sodium + Chlorine  + NaClNa Cl 2 22 2.0 moles 1.0 moles 4.0 moles 8.0 moles 2.0 moles 1.0 moles0.5 moles1.0 moles 8.0 moles 4.0 moles

4. 2. Sodium Chlorate  Sodium Chloride + Oxygen  + NaClO 3 NaClO2O2 223 4.0 moles.567 moles 6.0 moles4.0 moles.378 moles

5. 3. How many moles of Oxygen are produced from the decomposition of.849 moles of Potassium Chlorate? Potassium Chlorate  Potassium Chloride + Oxygen KClO 3  O2O2 KCl +322

6. 4. How many grams of Water are produced from the decomposition of 1.42 moles of Sodium Hydroxide? Sodium Hydroxide  Sodium Oxide + Water NaOH  Na 2 O +H2OH2O2

7. 5. How many moles of Hydrogen are produced from the reaction of 2.10 moles of Sodium with Water? Sodium + Water  Sodium Hydroxide + Hydrogen Na + H 2 O  NaOH +H2H2 2

8. 6. Determine the mass of Fluorine that must react with Lithium to produce 12.0 grams of Lithium Fluoride. Lithium + Fluorine  Lithium Fluoride Li + F 2  LiF22

9.  The reactant that is present in least abundance (less amount of moles) determines the amount of product formed.  Example: You need to make as many cakes as possible. Each cake requires 2 eggs, 2 cups of flour, and 1 cup of sugar. You have 6 eggs, 6 cups of sugar, and 4 cups of flour. Which is your limiting reactant (ingredient)?

10. 1. Circle the limiting reactant: NaHCO 3 + HCl  NaCl + H 2 O + CO 2 Given: 1.0 mole 1.5 mole 1.0 mole Actual: Given:.475 mole.214 mole Actual:.214 mole

11. 2. Mg + 2 HCl  MgCl 2 + H 2 Given: 1.0 mole 1.5 mole Actual: Given: 2.0 mole 4.5 mole Actual:

12. 3. 2 Al + 3 S  Al 2 S 3 Given: 4.0 mole 5.0 mole Actual:

13. 4. If 1.00 gram of Hydrogen reacts with 6.00 grams of Oxygen, determine the mass of product formed.