Limiting Reactants (Section) (a) Define the terms

Chemistry: A Molecular Approach | 3rd Edition | ISBN: 9780321809247 | Authors: Nivaldo J. Tro

Problem 72AE Chapter 3

Chemistry: A Molecular Approach | 3rd Edition

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Chemistry: A Molecular Approach | 3rd Edition | ISBN: 9780321809247 | Authors: Nivaldo J. Tro

Chemistry: A Molecular Approach | 3rd Edition

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Problem 72AE

Limiting Reactants (Section) (a) Define the terms theoretical yield, actual yield, and percent yield, (b) Why is the actual yield in a reaction almost always less than the theoretical yield? (c) Can a reaction ever have 110% actual yield?

Step-by-Step Solution:

Solution 72 Step-by-step solution Step 1 of 3 The theoretical yield is the amount predicted by a stoichiometric calculation based on the number of moles of all reactants present. This calculation assumes that only one reaction occurs and that the limiting reactant reacts completely. However the actual yield is very often smaller (the percent yield is less than 100%) for several reasons Step 2 of 3 Actual yield: The amount of product actually obtained is called the actual yield. Percent yield: The percent yield of a reaction is the actual yield divided by theoretical yield, multiplied by 100%.

Step 3 of 3

Chapter 3, Problem 72AE is Solved
Textbook: Chemistry: A Molecular Approach
Edition: 3rd
Author: Nivaldo J. Tro
ISBN: 9780321809247

This full solution covers the following key subjects: Yield, actual, reaction, theoretical, reactants. This expansive textbook survival guide covers 82 chapters, and 9464 solutions. Since the solution to 72AE from 3 chapter was answered, more than 278 students have viewed the full step-by-step answer. Chemistry: A Molecular Approach was written by Sieva Kozinsky and is associated to the ISBN: 9780321809247. The full step-by-step solution to problem: 72AE from chapter: 3 was answered by Sieva Kozinsky, our top Chemistry solution expert on 02/22/17, 04:35PM. This textbook survival guide was created for the textbook: Chemistry: A Molecular Approach, edition: 3rd. The answer to “Limiting Reactants (Section) (a) Define the terms theoretical yield, actual yield, and percent yield, (b) Why is the actual yield in a reaction almost always less than the theoretical yield? (c) Can a reaction ever have 110% actual yield?” is broken down into a number of easy to follow steps, and 39 words.

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