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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

The Limiting Reagent represents the compound that is totally consumed in the reaction. 

Limiting Reagent & Theoretical Yield

Concept #1: Limiting Reagent

Theoretical Yield is the maximum amount of product a certain chemical reaction can form. It is determined by the limiting reagent.

Concept #2: Limiting Reagent Stoichiometric Chart

Example #1: Chromium (III) oxide reacts with hydrogen sulfide (H2S) gas to form chromium (III) sulfide and water:

Cr2O3 (s) + 3 H2S (g) → Cr2S3 (s) + 3 H2O (l)

What is the mass of chromium (III) sulfide formed when 14.20 g Cr2O3 reacts with 12.80 g H2S?

Practice: Acrylonitrile (C­3H3N) is the starting material for many synthetic carpets and fabrics. It is produced by the following reaction: 

2 C3H6 (g) + 2 NH3 (g) + 3 O2 (g)  → 2 C3H3N (g) + 6 H2O (g)

If 12.0 g C3H6, 10.0 g NH­3, and 5.0 g O2 react, what mass of acrylonitrile can be produced, assuming 100% yield?

Practice: The reaction between solid aluminum and iron (III) chloride can generate temperatures reaching 3000 ºC and is used in welding metals. 

2 Al + Fe2O3 → Al2O­3 + 2 Fe

If 150 g of Al are reacted with 432 g of Fe­2O3, what is the mass of the excess reactant remaining?