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
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...
icon
Related questions
Question

please show work for the worksheet as soon as possible!

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)
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps with 2 images

Blurred answer
Knowledge Booster
Stoichiometry
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY