Lecture_13-Reaction_Stoichiometry

Stoichiometry

The branch of chemistry that involves the calculation of reactants and products in chemical reactions.

Chemical reaction

A process that involves the rearrangement of the molecular or ionic structure of a substance.

Balanced equation

An equation that has the same number of atoms of each element on both sides of the reaction.

Limiting reactant

The reactant that is completely consumed in a reaction and limits the amount of product that can form.

Diatomic elements

Elements that naturally exist as molecules made up of two atoms; examples include H2, N2, O2, etc.

Synthesis reaction

A type of reaction in which two or more reactants combine to form a single product.

Decomposition reaction

A type of reaction in which a single reactant breaks down into two or more products.

Single displacement reaction

A reaction where an element substitutes for another in a compound, resulting in a new element and compound.

Double displacement reaction

A reaction in which two compounds exchange ions or bonds to form two new compounds.

Combustion reaction

A reaction in which a substance reacts with oxygen to produce energy in the form of heat and light.

Percent yield

The ratio of the actual yield to the theoretical yield, expressed as a percentage, indicating the efficiency of a reaction.

Molar mass (MM)

The mass of one mole of a substance, usually expressed in grams per mole (g/mol).