Lecture_19_110211 - Lecture 19: Limiting Reactants Goals:...

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Lecture 19: Limiting Reactants Goals: Identify a limiting reactant when given the quantities of two or more reactants; calculate the amount of product formed from the limiting reactant. Describe the energy changes in exothermic and endothermic reactions. Outline (Timberlake 6.8-6.9): ± Percent Yield and Limiting Reactants (6.8) ± Energy Changes in Exothermic and Endothermic Reactions (6.9) Problems for Extra Practice: 6.65, 6.67, 6.69, 6.71, 6.73, 6.75, 6.77, 6.79
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Theoretical, Actual, and Percent Yield Theoretical yield: • the maximum amount of product, which is calculated using the balanced equation. Actual yield: • the amount of product obtained when the reaction takes place Percent yield: • the ratio of actual yield to theoretical yield Percent yield = actual yield (g) x 100 theoretical yield (g)
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Guide to Calculations for Percent Yield
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Learning Check When N 2 and 5.00 g of H 2 are mixed, the reaction produces 16.0 g of NH 3 . What is the percent yield for the reaction? N 2 (g) + 3H 2 (g) 2NH 3 (g) 1) 31.3% of NH 3 2) 56.9% of NH 3 3) 80.0% of NH 3
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Reacting Amounts In a table setting, there is 1plate, 1 fork, 1 knife, and 1 spoon. How many table settings are possible from 5 plates, 6 forks, 4 spoons, and 7 knives? What is the limiting item?
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Reacting Amounts (continued) Only 4 place settings are possible. Initially Used Left over Plates 5 4 1 Forks 6 4 2 Spoons 4 4 0 Knives 7 4 3 The limiting item is the spoon.
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Limiting Reactant A limiting reactant in a chemical reaction is the substance that • is used up
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This note was uploaded on 01/18/2012 for the course CHEM 120A taught by Professor Leahmiller during the Fall '11 term at University of Washington.

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Lecture_19_110211 - Lecture 19: Limiting Reactants Goals:...

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