Ideal Gas Laws Diagram

Units for gas pressure

atm, mm Hg, Torr, kPa

STP

Standard Temperature and Pressure

temperature unit for gases

Kelvin

Compressibility

the measure of how much a given volume of matter decreases when placed under pressure

Dalton's Law

The total pressure of a mixture of gases is the sum of the individual pressures

Boyle's Law

for a fixed amount of gas at constant temperature, the volume of the gas varies inversely with pressure

Charles' Law

for a fixed amount of gas at a constant pressure, the volume of the gas is directly proportional to the temperature

Gay-Lussac's Law

for a fixed amount of gas at constant volume, the pressure is directly proportional to the Kelvin temperature

Combined Gas Law

for a fixed amount of gas, the relationship between the pressure, volume, and temperature

Ideal Gas Law

the relationship between pressure, volume, moles and temperature of an ideal gas at a fixed set of conditions

ideal gas

a hypothetical gas that does not exist but its' characteristics fits all the assumptions of the kinetic-molecular theory

Diffusion

Movement of molecules from an area of higher concentration to an area of lower concentration.

effusion

A process by which gas particles pass through a tiny opening

Kelvin

SI unit for temperature

atmosphere (atm)

a unit equal to the pressure exerted by a column of mercury 760 mm high

pressure

the force exerted by a gas on the inside surface area of it's container

Volume

measure of the volume of the container filled wth a gas

moles

the number of moles of gas particles

absolute zero

The coldest temperature, 0 Kelvin, that can be reached. It is the hypothetical temperature at which all molecular motion stops.

IMFs of Ideal Gases

we consider Ideal Gases to have NO Intermolecular Forces since the gas particles do not interact

elastic collision

objects bounce off one another, a collision in which no kinetic energy is lost or transferred

barometer

An instrument that measures atmospheric pressure

manometer

A device used to measure the pressure of a sample of gas in a container.

vacuum

A space where no particles of matter exist, has no particles and no pressure

Avogadro's Law

equal volumes of gases at the same temperature and pressure contain equal numbers of molecules

1 mole of any gas at STP

occupies 22.4 Liters of space

Density

Mass per unit volume

Graham's Law

the rate of diffusion of a gas is inversely proportional to the square root of its molar mass

Gas Stoichiometry

The method of predicting or analyzing the quantity of a gas involved in a chemical reaction

Ideal Gas Constant

relationship between pressure, volume, moles and temperature of an ideal gas

temperature

a measure of the average kinetic energy of all the particles of a substance

standard temperature

0 degrees Celsius or 273 Kelvin

standard pressure

101.3 kPa or 1 atm or 760 Torr or 760 mm Hg or 14.7 psi

Molar Mass equation of an Ideal Gas

MM = (dRT)/P

Real vs. Ideal Gases

*Real*

- gas particles have volume

- some attraction

*Ideal*

- volume of gas particles compared to distances is insignificant

- no attractions

ideal gas conditions

- high temperature

- low pressure

- particles size small compared to space in between particles

- interactions between particles are insignificant

Kinetic Molecular Theory

the theory that all matter is composed of particles (atoms and molecules) moving constantly in random directions