KMT Gas Law Variables

Kinetic Molecular Theory (KMT)

A theory stating that particles are in constant, random motion and that heat usually causes them to gain kinetic energy.

Temperature

A measure that is proportional to the average kinetic energy of particles, with units including Celsius, Fahrenheit, and Kelvin.

Absolute Zero

Theoretical temperature of 0 Kelvin, representing the lowest possible temperature where particles have zero kinetic energy.

Volume

The amount of space that an object occupies, with gases having lots of space between particles and being very compressible.

Pressure

The amount of force exerted on a given area, caused by gas particles striking the walls of their container.

Standard Temperature and Pressure (STP)

A standard set of conditions for gas calculations, defined as 0°C (273K) and 1.0 atm (or equivalent).

Boyle's Law

At constant temperature, the volume of a gas is inversely proportional to its pressure: P1V1=P2V2P1V1=P2V2.

Charles's Law

At constant pressure, the volume of a gas is directly proportional to its absolute temperature: V1/T1=V2/T2V1/T1=V2/T2.

Gay-Lussac's Law

At constant volume, the pressure of a gas is directly proportional to its absolute temperature: P1/T1=P2/T2P1/T1=P2/T2.

Combined Gas Law

Combines Boyle's, Charles's, and Gay-Lussac's laws into one equation: (P1V1)/T1=(P2V2)/T2(P1V1)/T1=(P2V2)/T2.