A student is running the Diels-Alder reaction as you did in lab. The student starts the reaction with 5.031 g of maleic anhydride with enough anthracene to run the reaction in full. 7.335 g of product is obtained. What is the percent yield of the reaction?

A student is running the Diels-Alder reaction as you did in lab. The student starts the reaction with 5.031 g of maleic anhydride with enough anthracene to run the reaction in full. 7.335 g of product is obtained. What is the percent yield of the reaction?

Organic Chemistry

8th Edition

ISBN:9781305580350

Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote

Publisher:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote

Chapter6: Reactions Of Alkenes

Section: Chapter Questions

Problem 6.53P

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Question

A student is running the Diels-Alder reaction as you did in lab. The student starts the reaction with
5.031 g of maleic anhydride with enough anthracene to run the reaction in full. 7.335 g of product
is obtained. What is the percent yield of the reaction?

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Step 1: Given data

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Step 2: Calculating the moles of maleic anhydride

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Step 3: Determining the reaction

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Step 4: Calculating the theoretical yield of the product

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Step 5: Calculating the percent yield of the reaction

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