Chapter Four: Chemical Reactions and Chemical Quantities

These flashcards cover key concepts related to reaction stoichiometry, balanced chemical equations, and the relationships between quantities in chemical reactions.

Stoichiometry

The study of the relationships between the quantities of reactants and products in a chemical reaction.

Balanced Chemical Equation

An equation that has equal amounts of each element on both sides, reflecting the law of conservation of mass.

Law of Conservation of Mass

Mass is neither created nor destroyed in a chemical reaction; the total mass of reactants equals the total mass of products.

Mole-Mole Stoichiometry

The determination of the moles of reactants or products using the mole ratio from a balanced chemical equation.

Mass-Mass Stoichiometry

The determination of the mass of one of the reactants or products from a given mass of another based on their molar relationships.

Chemical Coefficients

Numbers in a balanced chemical equation that represent the relative amounts of each substance involved in the reaction.

Combustion of Octane

The reaction where octane (C8H18) combines with oxygen (O2) to produce carbon dioxide (CO2) and water (H2O).

Quantitative Relationship

The mathematical relationship that relates the amounts of reactants and products in a chemical reaction.

Example of Stoichiometry

Using the reaction 2C8H18 + 25O2 → 16CO2 + 18H2O to understand the ratios of moles involved.

Reactants

Substances that are consumed in a chemical reaction to form products.

Products

Substances that are formed as a result of a chemical reaction.