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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
Empirical Formula
Molecular Formula
Combustion Analysis
Combustion Apparatus
Polyatomic Ions
Naming Ionic Compounds
Writing Ionic Compounds
Naming Ionic Hydrates
Naming Acids
Naming Molecular Compounds
Balancing Chemical Equations
Limiting Reagent
Percent Yield
Mass Percent
Functional Groups in Chemistry

The Percent Yield determines how successful the product yield is in a chemical reaction. 

Percent Yield

Concept #1: Percent Yield

Example #1: Consider the following balanced chemical reaction:
2 C6H6 (l) + 15 O2 (g) → 12 CO2 (g) + 6 H2O (l)

If a 2.6 g sample of C6H6 reacted with excess O2 to produce 1.25 g of water, what is the percent yield of water?

Practice: Ammonia, NH3, reacts with hypochlorite ion, OCl, to produce hydrazine, N2H4. How many grams of hydrazine are produced from 115.0 g NH3 if the reaction has a 81.5% yield?  

2 NH3 + OCl → N24 + Cl + H2O

Practice: The reduction of iron (III) oxide creates the following reaction: 

Fe2O3 (s) + 3 H2 (g) → 2 Fe (s) + 3 H2O (g) 

If the above reaction only went to 75% completion, how many moles of Fe2O3 were require to produce 0.850 moles of Fe?