Stoichiometry and Gas Laws Review

Vocabulary and core concepts covering stoichiometry, kinetic molecular theory, and gas laws based on the lecture notes.

Pressure

The amount of force applied per unit area.

Absolute Pressure

The actual pressure of the gas inside a container, without reference to the pressure on the outside.

Force

A push or pull on an object.

Gauge Pressure

The difference between the pressure inside a container and the atmospheric pressure.

Mole

An amount equal to the number of atoms in $12\,g$ of carbon-12, abbreviated as $mol$.

Atomic weight

The average mass of the atoms of an element, based on the abundance of its isotopes.

Molar mass

The mass in grams of one mole of a substance, calculated as the sum of the molar masses of the elements forming a compound.

Stoichiometry

The calculation of the quantities of reactants and products in a chemical reaction.

Chemical Equation

A representation of a chemical reaction using formulas and symbols to show reactants and products.

Empirical formula

A chemical formula in which the subscripts represent the relative quantity of each element as the smallest whole-number ratio of atoms.

Oxidation state

The charge an atom would have if all bonds were completely ionic.

Percent Composition

The percent by mass of each element in a compound.

Avogadro’s number

The number of particles in one mole, equal to $6.022 \times 10^{23}$.

Law of conservation of matter

A principle stating that matter cannot be created or destroyed.

Stoichiometric Ratios

Ratios derived from a balanced equation used to find the amount of a reactant or product produced from another reactant or product.

Kinetic Molecular Theory

A theory describing the states of matter and gas particle behavior, assuming particles are in constant motion and collisions are elastic.

Elastic collisions

Collisions where no energy is lost, though energy can be transferred between particles or container walls.

Ideal Gas

A theoretical gas that perfectly follows the assumptions of kinetic molecular theory, assuming no particle volume and no attractive forces.

Pascal (Pa)

The SI unit for pressure, defined as a unit of force per unit area.

Atmospheric Pressure (Sea Level)

The standard pressure exerted by the atmosphere, equal to $14.7\,psi$, $101.3\,kPa$, or $1\,atm$.

Absolute zero

The lowest possible temperature, defined as $0\,K$ or $-273.15^{\circ}C$.

Standard Temperature and Pressure (STP)

Standard conditions for scientific comparison, defined as $0^{\circ}C$ ($273.15\,K$) and $1\,atm$ ($101.3\,kPa$).

Boyle’s Law

A gas law stating $P_1V_1 = P_2V_2$ when temperature and moles remain constant.

Charles’s Law

A gas law stating $\frac{V_1}{T_1} = \frac{V_2}{T_2}$ when pressure and moles remain constant.

Avogadro’s Law

A gas law stating $\frac{V_1}{n_1} = \frac{V_2}{n_2}$ when temperature and pressure remain constant.

Ideal Gas Law

The comprehensive gas equation $PV = nRT$, where $R$ is the ideal gas constant ($0.0821$ or $8.314$).

Partial pressure

The pressure exerted by an individual gas within a mixture of gases; the sum of these pressures equals the total pressure.