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Slide 1 of 36 Chemistry 16.3. © Copyright Pearson Prentice Hall Slide 2 of 36 Limiting Reagent and Percent Yield If a carpenter had two tabletops and.

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Presentation on theme: "Slide 1 of 36 Chemistry 16.3. © Copyright Pearson Prentice Hall Slide 2 of 36 Limiting Reagent and Percent Yield If a carpenter had two tabletops and."— Presentation transcript:

1 Slide 1 of 36 Chemistry 16.3

2 © Copyright Pearson Prentice Hall Slide 2 of 36 Limiting Reagent and Percent Yield If a carpenter had two tabletops and seven table legs, he could only build one four-legged table. The number of table legs is the limiting factor in the construction of four-legged tables. Similarly, in chemistry, the amount of product made in a chemical reaction may be limited by the amount of one or more of the reactants. 12.3

3 © Copyright Pearson Prentice Hall Limiting Reagent and Percent Yield > Slide 3 of 36 Limiting and Excess Reagents How is the amount of product in a reaction affected by an insufficient quantity of any of the reactants? 12.3

4 Slide 4 of 36 © Copyright Pearson Prentice Hall Limiting Reagent and Percent Yield > 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 reagent that determines the amount of product that can be formed by a reaction. 12.3

5 Slide 5 of 36 © Copyright Pearson Prentice Hall Limiting Reagent and Percent Yield > Limiting and Excess Reagents In the reaction of nitrogen and hydrogen, hydrogen is the limiting reagent. Nitrogen is the reagent that is not completely used up in the reaction. The reagent that is not used up is called the excess reagent. 12.3

6 Slide 6 of 36 © Copyright Pearson Prentice Hall Limiting Reagent and Percent Yield > Limiting and Excess Reagents 12.3 The Chemical Equation for the Preparation of Ammonia

7 © Copyright Pearson Prentice Hall Slide 7 of 36 Limiting Reagent and Percent Yield > Limiting and Excess Reagents Animation 13 Apply the limiting reagent concept to the production of iron from iron ore.

8 © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 8 of

9 © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 9 of

10 © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 10 of

11 © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 11 of

12 © Copyright Pearson Prentice Hall Slide 12 of 36 Practice Problems for Sample Problem 12.7 Problem Solving Solve Problem 25 with the help of an interactive guided tutorial.

13 © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 13 of

14 © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 14 of

15 © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 15 of

16 © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 16 of

17 © Copyright Pearson Prentice Hall Slide 17 of 36 Practice Problems for Sample Problem 12.8 Problem Solving Solve Problem 28 with the help of an interactive guided tutorial.

18 © Copyright Pearson Prentice Hall Limiting Reagent and Percent Yield > Slide 18 of 36 Percent Yield What does the percent yield of a reaction measure? 12.3

19 Slide 19 of 36 © Copyright Pearson Prentice Hall Limiting Reagent and Percent Yield > 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. 12.3

20 Slide 20 of 36 © Copyright Pearson Prentice Hall Limiting Reagent and Percent Yield > Percent Yield The theoretical yield is the maximum amount of product that could be formed from given amounts of reactants. In contrast, the amount of product that actually forms when the reaction is carried out in the laboratory is called the actual yield. 12.3

21 Slide 21 of 36 © Copyright Pearson Prentice Hall Limiting Reagent and Percent Yield > Percent Yield The percent yield is the ratio of the actual yield to the theoretical yield expressed as a percent. 12.3

22 © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 22 of

23 © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 23 of

24 © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 24 of

25 © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 25 of

26 © Copyright Pearson Prentice Hall Slide 26 of 36 Practice Problems for Sample Problem 12.9 Problem Solving Solve Problem 29 with the help of an interactive guided tutorial.

27 © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 27 of

28 © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 28 of

29 © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 29 of

30 © Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 30 of

31 © Copyright Pearson Prentice Hall Slide 31 of 36 Practice Problems for Sample Problem Problem Solving Solve Problem 31 with the help of an interactive guided tutorial.

32 © Copyright Pearson Prentice Hall Slide 32 of 36 Section Quiz -or- Continue to: Launch: Assess students’ understanding of the concepts in Section 12.3 Section Quiz

33 © Copyright Pearson Prentice Hall Slide 33 of Section Quiz. 1.In the reaction 3NO 2 + H 2 O  2HNO 3 + NO, how many grams of HNO 3 can form when 1.00 g of NO 2 and 2.25 g of H 2 O are allowed to react? a g b g c.15.7 g d.1.37 g

34 © Copyright Pearson Prentice Hall Slide 34 of Section Quiz. 2.How many grams of H 2 O can be formed from 24.0 g O 2 and 6.00 g H 2 ? a.30.0 g b.27.0 g c.54.0 g d.13.5 g

35 © Copyright Pearson Prentice Hall Slide 35 of 36 3.Octane burns according to the following equation. 2C 8 H O 2  16CO H 2 O What is the percent yield if 14.6 g of CO 2 are produced when 5.00 g of C 8 H 18 are burned? a.106% b.94.8% c.34.2% d.62.5% 12.3 Section Quiz.

36 © Copyright Pearson Prentice Hall Slide 36 of 36 Limiting Reagent and Percent Yield > Concept Map 12 Solve the Concept Map with the help of an interactive guided tutorial.

37 END OF SHOW


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