Double Cheeseburgers and Stoichiometry

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Presentation transcript:

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: Buns Patties Cheese Slices Bacon Strips How Many Burgers? 2 4 8 16 30 32 48

Objectives To understand the concept of limiting reactants To learn to recognize the limiting reactant in a reaction To learn to use the limiting reactant to do stoichiometric calculations To learn to calculate percent yield

A. The Concept of Limiting Reactants Stoichiometric mixture N2(g) + 3H2(g)  2NH3(g)

A. The Concept of Limiting Reactants Limiting reactant mixture N2(g) + 3H2(g)  2NH3(g)

A. The Concept of Limiting Reactants For a Limiting reactant mixture the number of moles are not balanced to match the reaction equation N2(g) + 3H2(g)  2NH3(g) Limiting reactant is the reactant that runs out first When the limiting reactant is exhausted, then the reaction stops

B. Calculations Involving a Limiting Reactant

B. Calculations Involving a Limiting Reactant

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.

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?