1. Section 9.3 Limiting Reactants and Percent Yield Double Cheeseburgers and Stoichiometry 1 Double Cheeseburger needs 1 bun, 2 patties, 2 slices of cheese, 4 strips of bacon For 5 Double Cheeseburgers how many units of each ingredient do I need? Fill in the final column below with how many complete burgers I can make: BunsPattiesCheese Slices Bacon Strips How Many Burgers? 2448 44816 303248

2. Section 9.3 Limiting Reactants and Percent Yield 1.To understand the concept of limiting reactants 2.To learn to recognize the limiting reactant in a reaction 3.To learn to use the limiting reactant to do stoichiometric calculations 4.To learn to calculate percent yield Objectives

3. Section 9.3 Limiting Reactants and Percent Yield A. The Concept of Limiting Reactants Stoichiometric mixture –N 2 (g) + 3H 2 (g)  2NH 3 (g)

4. Section 9.3 Limiting Reactants and Percent Yield Limiting reactant mixture A. The Concept of Limiting Reactants –N 2 (g) + 3H 2 (g)  2NH 3 (g)

5. Section 9.3 Limiting Reactants and Percent Yield For a Limiting reactant mixture the number of moles are not balanced to match the reaction equation –N 2 (g) + 3H 2 (g)  2NH 3 (g) A. The Concept of Limiting Reactants –Limiting reactant is the reactant that runs out first –When the limiting reactant is exhausted, then the reaction stops

6. Section 9.3 Limiting Reactants and Percent Yield B. Calculations Involving a Limiting Reactant

7. Section 9.3 Limiting Reactants and Percent Yield B. Calculations Involving a Limiting Reactant

8. Section 9.3 Limiting Reactants and Percent Yield C. Percent Yield Theoretical Yield –The maximum amount of a given product that can be formed when the limiting reactant is completely consumed. The actual yield (amount produced) of a reaction is usually less than the maximum expected (theoretical yield). Percent Yield –The actual amount of a given product as the percentage of the theoretical yield.

9. Section 9.3 Limiting Reactants and Percent Yield According to his pre-lab theoretical yield calculations a student’s experiment should have produced 1.44g of magnesium oxide. When he weighed his product after reaction, only 1.23g of magnesium oxide was present. What is the student’s percent yield?