Ch.3 - Chemical ReactionsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: If the theoretical yield for a reaction was 180 grams and you actually made 118 grams of the product, what is your percent yield?A. 78.2%B. 122%C. 128%D. 65.6%E. 180%

Problem

If the theoretical yield for a reaction was 180 grams and you actually made 118 grams of the product, what is your percent yield?

A. 78.2%

B. 122%

C. 128%

D. 65.6%

E. 180%

Solution

Use the formula for percent yield to determine the percent yield from the actual and theoretical yield provided

Recall that percent yield  is given by:

% yield = actual yieldtheoretical yield×100


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