Chemical reactions in the real world don't always go exactly as planned on paper. In the course of an experiment, many thingswill contribute to the formation of less product than would be predicted. Besides spills and other experimental errors, there areusually losses due to an incomplete reaction and undesirable side reactions. Chemists need a measurement that indicates howsuccessful 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 onstoichiometry. This is called the theoretical yield, the maximum amount of product that could be formed from the givenamounts of reactants. The actual yield is the amount of product that is actually formed when the reaction is carried out in thelaboratory. 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 forchemical production. When complex chemicals are synthesized by many different reactions, one step with a low percent yieldcan 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 yieldsgreater than 100% are possible if the measured product of the reaction contains impurities that cause its mass to be greaterthan it actually would be if the product was pure. When a chemist synthesizes a desired chemical, he or she is always careful topurify the products of the reaction. StoichiometryTheoretical, Actual, & Percent Yields1. According to the article, what is "theoretical yield"?2. According to the article, what is "actual yield"?3. According to the article, which yield isdetermined from stoichiometry calculations?●4. According to the article, why is it necessary to calculate apercent 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 anactual yield less than the theoretical yield?6. According to the article, why might some reactions produce anactual yield greater than the theoretical yield?

The given questions have to be answered by studying the given article which is about yield of the…

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: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 141QRT

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