Chemistry 16.3

Limiting and Excess Reagents 12.3 Limiting and Excess Reagents Bell Work Your cookie recipe calls for 2 eggs and 4 cups of flour. You have 17 cups of flour and 5 eggs. How many full batches of cookies can you make?

Limiting and Excess Reagents 12.3 Limiting and Excess Reagents In a chemical reaction, an insufficient quantity of any of the reactants will limit the amount of product that forms. The limiting reagent is the reactant that determines the amount of product that can be formed by a reaction. (The Eggs from the Example)

Limiting and Excess Reagents 12.3 Limiting and Excess Reagents The reagent that is not used up is called the excess reagent. (The flour from the example)

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for Sample Problem 12.7 Problem Solving 12.25 Solve Problem 25 with the help of an interactive guided tutorial.

12.8

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for Sample Problem 12.8 Problem Solving 12.28 Solve Problem 28 with the help of an interactive guided tutorial.

Numbers 3 and 4 on LR Worksheet (#3) 12.3 Percent Yield Bell Work Numbers 3 and 4 on LR Worksheet (#3) A batting average is actually a percent yield.

A batting average is actually a percent yield. 12.3 Percent Yield The percent yield is a measure of the efficiency of a reaction carried out in the laboratory. A batting average is actually a percent yield. A batting average is actually a percent yield.

12.3 Percent Yield The theoretical yield is the maximum amount of product that could be formed from given amounts of reactants. The actual yield is the amount of product that actually forms when the reaction is carried out in the laboratory.

12.3 Percent Yield The percent yield is the ratio of the actual yield to the theoretical yield expressed as a percent.

12.9 Calculating Theoretical Yield is just Mass:Mass!!!!!!!!

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for Sample Problem 12.9 Problem Solving 12.29 Solve Problem 29 with the help of an interactive guided tutorial.

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for Sample Problem 12.10 Problem Solving 12.31 Solve Problem 31 with the help of an interactive guided tutorial.

12.3 Section Quiz. 12.3.

12.3 Section Quiz. 1. In the reaction 3NO2 + H2O  2HNO3 + NO, how many grams of HNO3 can form when 1.00 g of NO2 and 2.25 g of H2O are allowed to react? 0.913 g 0.667 g 15.7 g 1.37 g

12.3 Section Quiz. 2. How many grams of H2O can be formed from 24.0 g O2 and 6.00 g H2? 30.0 g 27.0 g 54.0 g 13.5 g

12.3 Section Quiz. 3. Octane burns according to the following equation. 2C8H18 + 25O2  16CO2 + 18H2O What is the percent yield if 14.6 g of CO2 are produced when 5.00 g of C8H18 are burned? 106% 94.8% 34.2% 62.5%

Solve the Concept Map with the help of an interactive guided tutorial.

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