Chemistry II: Stoichiometry

A set of vocabulary flashcards covering basic stoichiometry concepts, constants, and gas laws based on the Chemistry II lecture notes.

Mol (Mole)

The amount of a substance that contains the same number of elementary entities as there are atoms in twelve grams of carbon-12.

Avogadro constant

The number of particles in one mole, defined as $6.0221367 \times 10^{23}$ or $6.023 \times 10^{23}$ particles.

Particles

Technical term referring to atoms, molecules, ions, or other elementary entities.

Atomic mass units

The two units used for atomic mass are AMUs and $\text{Grams/mole}$.

Molar mass

The sum of the atomic masses of the elements that make up a compound, where $1\text{ mole}$ is equal to the molar mass of a compound.

Standard Temperature for Gases

The temperature condition of $273\text{ k}$ ($0\text{ }^\text{o}\text{C}$) used when considering molar volume.

Standard Pressure for Gases

The pressure condition of $1\text{ Atmosphere}$ used when considering molar volume.

Molar volume

The unit used to measure the amount of space occupied by one mole of a substance; for any gas, this volume is $22.4\text{ L}$.

Law of conservation of matter

A principle stated by Antoine L. Lavoisier in 1785 that «Matter is neither created nor destroyed, only transformed.»

Molar ratio

The ratio established between the number of moles of any two substances in a chemical equation, indicated by the coefficients.

Stoichiometry

The numerical and quantifiable relationship between the reactants and products of a chemical reaction, conceptualized by Jeremías Benjamín Richter.

Stoichiometrical relationships

The specific types of relationships used in calculations, including Mole-to-mole, Mass-to-mass, Volume-to-volume, and Combined relationships.