Honors Chem vocabulary final

Kinetic molecular theory

The kinetic molecular theory explains the behavior of gases in terms of particles in motion. It states that gas particles are in constant random motion, have negligible volume, and experience elastic collisions.

Kmt theory

states that gas particles move rapidly and randomly, with their kinetic energy determining the temperature of the gas.

Dalton’s law

states that in a mixture of gases, the total pressure is equal to the sum of the partial pressures of each individual gas.

Charles law

states that the volume of a gas is directly proportional to its absolute temperature at constant pressure.

Boyles law

states that the pressure of a gas is inversely proportional to its volume at constant temperature.

Gay-lussacs law

states that the pressure of a gas is directly proportional to its absolute temperature at constant volume.

Grahams law

describes the rates of diffusion of gases inversely proportional to the square root of their molar masses.

Ideal gas law

relates pressure, volume, temperature, and number of moles of a gas, expressed as $PV=nRT$.

Heterogeneous mixture

a mixture composed of components that are not uniform throughout, such as salad or sand and salt.

Homogeneous mixture

a mixture that has a consistent composition throughout, such as air or saltwater.

Solution

a homogeneous mixture where one substance (the solute) is dissolved in another (the solvent), resulting in a single phase.

Solute

The substance that is dissolved