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?
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%.
Textbook: Chemistry: A Molecular Approach
Author: Nivaldo J. Tro
This full solution covers the following key subjects: Yield, actual, reaction, theoretical, reactants. This expansive textbook survival guide covers 82 chapters, and 9454 solutions. Since the solution to 72AE from 3 chapter was answered, more than 335 students have viewed the full step-by-step answer. Chemistry: A Molecular Approach was written by and is associated to the ISBN: 9780321809247. The full step-by-step solution to problem: 72AE from chapter: 3 was answered by , 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: 3. 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.