Gas Laws, Mole Concepts, and Organic Chemistry Revision

Boyle's law

States that the volume of a fixed mass of a gas is inversely proportional to the pressure at constant/fixed temperature ($PV = \text{Constant}$).

Charles' law

States that the volume of a fixed mass of a gas is directly proportional to the absolute temperature at constant/fixed pressure ($V/T = \text{Constant}$).

Absolute zero

The temperature of $-273.00311211111103576356356356356356356356356356356356356356356356356356356356356356356356356356356356356356356356356356356356356356357^{\circ}C$ or $0\,K$ where the volume of a gas is zero and is the lowest temperature at which a gas can exist.

The mole

The SI unit of the amount of substance.

Avogadros Constant

The number of particles in one mole, denoted "$L$", which contains $6.023 \times 10^{23}$ particles (sometimes simplified to $6.0 \times 10^{23}$).

Empirical formula

The simplest formula of a compound representing the simplest whole number ratios in which atoms of elements combine to form the compound.

Molecular formula

The actual number of each kind of atoms present in a molecule of a compound, determined as a multiple ($n$) of the empirical formula.

Diffusion

The movement of molecules of a gas from a region of high concentration to a region of low concentration.

Grahams law of diffusion

States that the rate of diffusion of a gas is inversely proportional to the square root of its density at