Gases Physical Properties

Solid

Matter that is very clumped, with little space between molecules, and molecules vibrate in place.

Liquid

Matter with a small amount of intermolecular space, where molecules move about and slide past each other.

Gas

Matter with lots of intermolecular space, where molecules move freely and very fast.

Kinetic Molecular Theory (KMT)

A theory stating that particles of matter are always in motion.

Compressibility

The ability of gas to be compressed or expanded due to lots of empty space.

Real Gases

Gases that do not behave ideally and vary in behavior based on particle size and intermolecular forces.

Boyle’s Law

The law stating that volume and pressure are inversely related when temperature and amount are held constant.

Charles’ Law

The law stating that volume and temperature are directly related when pressure and amount are held constant.

Gay-Lussac’s Law

The law stating that pressure and temperature are directly related when amount and volume are held constant.

Avogadro’s Law

The law stating that volume and amount are directly related when pressure and temperature are held constant.

Dalton’s Law

The law that states the total pressure is equal to the sum of all partial pressures in a mixture.

Ideal Gas Law

The mathematical relationship between pressure, volume, temperature, and the number of moles of gas, represented as PV=nRT.

Standard Temperature and Pressure (STP)

Conditions defined as a temperature of 0°C (273 K) and pressure of 1 atm (101.3 kPa, 760 torr).

0°C is how much Kelvin?

273 K

1 atm is how much kPa?

101.3

1 atm is how much mmHg and torr?

760 mmHg and torr