example 2 Name:Per:Date:Percent Yield Worksheet:Every percent yield problem will provide an amount of reactant and an ACTUAL YIELD. To solve for the percentyield, do the following:Example 1: Solid calcium carbonate, CaCO3,is able to remove sulphur dioxide from waste gases by the reaction:CaCO3 + SO2 ------> CaSO3 + CO2In a particular experiment, an excess of CaCO3 was exposed to 135 g of SO, in the presence of an excess amountof the other chemicals required for the reaction. If only 198 g of CaSO3was isolated from the products, what wasthe 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 product2) 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 + H2Example 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 productActual yield here(#2)X 100 =Theoretical yield here (#1)

Given: Mass of Mg = 40 g Mass of H2 = 1.7 g Standard data: The molar mass of Mg = 24.305 g/mol…

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? Consider the reaction: Mg + 2HNO3 --> Mg(NO3)2 + H2 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)

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? Consider the reaction: Mg + 2HNO3 --> Mg(NO3)2 + H2 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)

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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Concept explainers

Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".

Question

example 2

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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