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Chapter 12 Stoichiometry Part 3. PERCENT YIELD Most reactions never succeed in producing the predicted amount of product. So in order to determine the.

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Presentation on theme: "Chapter 12 Stoichiometry Part 3. PERCENT YIELD Most reactions never succeed in producing the predicted amount of product. So in order to determine the."— Presentation transcript:

1 Chapter 12 Stoichiometry Part 3

2 PERCENT YIELD Most reactions never succeed in producing the predicted amount of product. So in order to determine the success of a reaction, the percent yield is calculated.

3 Comparing the actual quantitative results of a chemical rxn to the theoretical (calculated) maximum. Why? * to determine if a method of manufacturing a product is profitable or another method works better

4 Usually the % yield is less than 100 b/c product is lost somewhere along the way or the reaction wasnt complete. Occasionally the % yield is above 100 if the product is contaminated or if moisture is absorbed b/c of high humidity.

5 % yield = actual yield x 100 theoretical yield theoretical maximum amount of product that can be produced from a given amount of reactant in a chemical equation actual the amount of product actually produced when the chemical reaction is carried out in an experiment

6 Examples When 24.8g of calcium carbonate is decomposed by heating, 13.1g of calcium oxide forms along with some CO 2. What is the % yield of this rxn?

7 Example What is the percent yield if 3.74g of copper are produced when 1.87g of Al are reacted with an excess of copper II sulfate? 2Al + 3CuSO 4 Al 2 (SO 4 ) 3 + 3Cu

8 Example What is the percent yield if 56.15g of Na reacts with an excess of Cl 2 and yields 136.2g of sodium chloride?

9 Example If the decomposition of magnesium chlorate is 92.3% efficient, how many grams of magnesium chlorate are needed to produce g of magnesium chloride?


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