Balancing Chemical Equations and Reaction Types

These flashcards cover key vocabulary and concepts related to balancing chemical equations, types of reactions, and stoichiometry.

Balancing Chemical Equation

The process of ensuring that the number of atoms for each element is the same on both sides of the equation.

Reactants

Starting materials in a chemical reaction.

Products

Substances formed as a result of a chemical reaction.

Limiting Reactant

The reactant that limits the amount of product in a chemical reaction.

Excess Reactant

The reactant that is not completely used by the other reactants.

Theoretical Yield

The amount of product that can be produced in a chemical reaction based on the amount of limiting reactant.

Actual Yield

The amount of product actually produced by a chemical reaction.

Percent Yield

The percentage of the theoretical yield that was actually attained, calculated as the ratio of actual yield to theoretical yield.

Synthesis Reaction

A reaction in which two or more compounds react to form one product.

Decomposition Reaction

A reaction in which a single reactant is converted to two or more simpler substances.

Combustion Reaction

A type of chemical reaction where a substance combines with oxygen and produces energy in the form of heat and light.

Conversion Factor

A ratio used to convert from one unit to another, often used in stoichiometric calculations.

Balanced Equation

An equation in which the number of atoms for each element is equal on both sides of the equation.

Moles

A unit of measurement in chemistry representing a specific number of particles (6.022 x 10^23).

Aqueous Solution

A solution in which the solvent is water.

Combustion of Hydrocarbons

The process of burning hydrocarbons (such as alkanes) in the presence of oxygen to produce carbon dioxide and water.