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Ch.6 Chemical Reactions & QuantitiesWorksheetSee all chapters
All Chapters
Ch.1 Matter and Measurements
Ch.2 Atoms and the Periodic Table
Ch.3 Ionic Compounds
Ch.4 Molecular Compounds
Ch.5 Classification & Balancing of Chemical Reactions
Ch.6 Chemical Reactions & Quantities
Ch.7 Energy, Rate and Equilibrium
Ch.8 Gases, Liquids and Solids
Ch.9 Solutions
Ch.10 Acids and Bases
Ch.11 Nuclear Chemistry
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Empirical Formula
Molecular Formula
Calculating Molar Mass
Mole Concept
Mass Percent
Limiting Reagent
Percent Yield

Stoichiometry deals with the numerical relationship between compounds in a balanced chemical equation.


Concept #1: Stoichiometry

Concept #2: Stoichiometric Chart

Utilize the stoichiometric chart to do all your stoichiometric calculations.

Example #1: How many grams of H2O are produced when 12.3 g H2 reacts?

2 H2 (g) + 1 O2 (g) → 2 H2O (g)

Practice: The oxidation of chromium solid is represented by the following equation:  


How many moles of chromium (III) oxide are produced when 34.69 g Cr reacts with excess oxygen gas? 

Practice: The reaction of potassium chlorate and sucrose is given below: 

If 2.33 x 10-7 formula units of potassium chlorate are reacted, how many grams of carbon dioxide will be produced? 

Practice: If the density of ethanol, CH3CH2OH, is 0.789 g/mL, how many milliliters of ethanol are needed to produce 4.8 g of H2O in the following reaction?