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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

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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

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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)

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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)

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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

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

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

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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.

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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?

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