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Example 1: Solid calcium carbonate, CaCO,, is able to remove sulphur dioxide from waste gases by the reaction: CaCO3 + SO2 ------> CASO3 + CO2 In a particular experiment, an excess of CaCO3 was exposed to 135 g of SO, in the presence of an excess amount of the other chemicals required for the reaction. If only 198 g of Caso, was isolated from the products, what was the percentage yield of CaSo, in this experiment? 1) Solve for the theoretical yield (what you have always been doing). This is a grams-grams problem: (This is the amount of product 2) What is the actual yield as given in the problem? given) 3) Plug in amounts from #1 and #2 into the formula below: A Actual yield here(#2) X 100 = E Theoretical yield here (#1)

Example 1: Solid calcium carbonate, CaCO,, is able to remove sulphur dioxide from waste gases by the reaction: CaCO3 + SO2 ------> CASO3 + CO2 In a particular experiment, an excess of CaCO3 was exposed to 135 g of SO, in the presence of an excess amount of the other chemicals required for the reaction. If only 198 g of Caso, was isolated from the products, what was the percentage yield of CaSo, in this experiment? 1) Solve for the theoretical yield (what you have always been doing). This is a grams-grams problem: (This is the amount of product 2) What is the actual yield as given in the problem? given) 3) Plug in amounts from #1 and #2 into the formula below: A Actual yield here(#2) X 100 = E Theoretical yield here (#1)

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Name: Per: Date: Percent Yield Worksheet: Every percent yield problem will provide an amount of reactant and an ACTUAL YIELD. To solve for the percent yield, do the following: Example 1: Solid calcium carbonate, CaCO3, is able to remove sulphur dioxide from waste gases by the reaction: CaCO3 + SO2 ------> CaSO3 + CO2 In a particular experiment, an excess of CaCO3 was exposed to 135 g of SO, in the presence of an excess amount of the other chemicals required for the reaction. If only 198 g of CaSO3 was isolated from the products, what was the percentage yield of CaSO, in this experiment? 1) Solve for the theoretical yield (what you have always been doing). This is a grams-grams problem: (This is the amount of product 2) What is the actual yield as given in the problem? given) 3) Plug in amounts from #1 and #2 into the formula below: Actual yield here(#2) X 100 = Theoretical yield here (#1) Consider the reaction: Mg + 2HNO3 --> Mg(NO3)2 + H2 Example 2: When 40.0 grams of magnesium is placed in an excess of nitric acid, 1.7 grams of hydrogen is actually produced, what was my percent yield of hydrogen? 1) Solve for the theoretical yield (what you have always been doing). This is a grams-grams problem: 2) What is the actual yield as given in the problem? given) 3) Plug in amounts from #1 and #2 into the formula below: (This is the amount of product Actual yield here(#2) X 100 = Theoretical yield here (#1)
Transcribed Image Text:Name: Per: Date: Percent Yield Worksheet: Every percent yield problem will provide an amount of reactant and an ACTUAL YIELD. To solve for the percent yield, do the following: Example 1: Solid calcium carbonate, CaCO3, is able to remove sulphur dioxide from waste gases by the reaction: CaCO3 + SO2 ------> CaSO3 + CO2 In a particular experiment, an excess of CaCO3 was exposed to 135 g of SO, in the presence of an excess amount of the other chemicals required for the reaction. If only 198 g of CaSO3 was isolated from the products, what was the percentage yield of CaSO, in this experiment? 1) Solve for the theoretical yield (what you have always been doing). This is a grams-grams problem: (This is the amount of product 2) What is the actual yield as given in the problem? given) 3) Plug in amounts from #1 and #2 into the formula below: Actual yield here(#2) X 100 = Theoretical yield here (#1) Consider the reaction: Mg + 2HNO3 --> Mg(NO3)2 + H2 Example 2: When 40.0 grams of magnesium is placed in an excess of nitric acid, 1.7 grams of hydrogen is actually produced, what was my percent yield of hydrogen? 1) Solve for the theoretical yield (what you have always been doing). This is a grams-grams problem: 2) What is the actual yield as given in the problem? given) 3) Plug in amounts from #1 and #2 into the formula below: (This is the amount of product Actual yield here(#2) X 100 = Theoretical yield here (#1)
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