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Theoretical, Actual, & Percent Yields 1. According to the article, what is "theoretical yield"? 2. According to the article, what is "actual yield"? 3. According to the article, which yield is determined from stoichiometry calculations? OR Slide #1, highlight the areas where you found the answers. 4. According to the article, why is it necessary to calculate a percent yield for each reaction? 5. According to the article, why might some reactions produce an actual yield less than the theoretical yield? 6. According to the article, why might some reactions produce an actual yield greater than the theoretical yield.

Theoretical, Actual, & Percent Yields 1. According to the article, what is "theoretical yield"? 2. According to the article, what is "actual yield"? 3. According to the article, which yield is determined from stoichiometry calculations? OR Slide #1, highlight the areas where you found the answers. 4. According to the article, why is it necessary to calculate a percent yield for each reaction? 5. According to the article, why might some reactions produce an actual yield less than the theoretical yield? 6. According to the article, why might some reactions produce an actual yield greater than the theoretical yield.

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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Chemical reactions in the real world don't always go exactly as planned on paper. In the course of an experiment, many things will contribute to the formation of less product than would be predicted. Besides spills and other experimental errors, there are usually losses due to an incomplete reaction and undesirable side reactions. Chemists need a measurement that indicates how successful a reaction has been. This measurement is called the percent yield. To compute the percent yield, it is first necessary to determine how much of the product should be formed based on stoichiometry. This is called the theoretical yield, the maximum amount of product that could be formed from the given amounts of reactants. The actual yield is the amount of product that is actually formed when the reaction is carried out in the laboratory. The percent yield is the ratio of the actual yield to the theoretical yield, expressed as a percentage. Percent yield is very important in the manufacture of products. Much time and money is spent improving the percent yield for chemical production. When complex chemicals are synthesized by many different reactions, one step with a low percent yield can quickly cause a large waste of reactants and unnecessary expense. Typically, percent yields are understandably less than 100 % because of the reasons indicated earlier. However, percent yields greater than 100% are possible if the measured product of the reaction contains impurities that cause its mass to be greater than it actually would be if the product was pure. When a chemist synthesizes a desired chemical, he or she is always careful to purify the products of the reaction.
Transcribed Image Text:Chemical reactions in the real world don't always go exactly as planned on paper. In the course of an experiment, many things will contribute to the formation of less product than would be predicted. Besides spills and other experimental errors, there are usually losses due to an incomplete reaction and undesirable side reactions. Chemists need a measurement that indicates how successful a reaction has been. This measurement is called the percent yield. To compute the percent yield, it is first necessary to determine how much of the product should be formed based on stoichiometry. This is called the theoretical yield, the maximum amount of product that could be formed from the given amounts of reactants. The actual yield is the amount of product that is actually formed when the reaction is carried out in the laboratory. The percent yield is the ratio of the actual yield to the theoretical yield, expressed as a percentage. Percent yield is very important in the manufacture of products. Much time and money is spent improving the percent yield for chemical production. When complex chemicals are synthesized by many different reactions, one step with a low percent yield can quickly cause a large waste of reactants and unnecessary expense. Typically, percent yields are understandably less than 100 % because of the reasons indicated earlier. However, percent yields greater than 100% are possible if the measured product of the reaction contains impurities that cause its mass to be greater than it actually would be if the product was pure. When a chemist synthesizes a desired chemical, he or she is always careful to purify the products of the reaction.
Stoichiometry Theoretical, Actual, & Percent Yields 1. According to the article, what is "theoretical yield"? 2. According to the article, what is "actual yield"? 3. According to the article, which yield is determined from stoichiometry calculations? ● 4. According to the article, why is it necessary to calculate a percent yield for each reaction? Answer these questions, using this text on Slide #1 for reference. On Slide #1, highlight the areas where you found the answers. 5. According to the article, why might some reactions produce an actual yield less than the theoretical yield? 6. According to the article, why might some reactions produce an actual yield greater than the theoretical yield?
Transcribed Image Text:Stoichiometry Theoretical, Actual, & Percent Yields 1. According to the article, what is "theoretical yield"? 2. According to the article, what is "actual yield"? 3. According to the article, which yield is determined from stoichiometry calculations? ● 4. According to the article, why is it necessary to calculate a percent yield for each reaction? Answer these questions, using this text on Slide #1 for reference. On Slide #1, highlight the areas where you found the answers. 5. According to the article, why might some reactions produce an actual yield less than the theoretical yield? 6. According to the article, why might some reactions produce an actual yield greater than the theoretical yield?
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