KINETIC MOLECULAR THEORY

kinetic molecular theory

explains the states of matter and is based on the idea that matter is composed of tiny particles that are always in motion

Boyle’s law

At constant temp., volume and pressure are inversely proportional

Boyle’s Law Formula

P1V1 = P2V2

Charles’s Law

At constant pressure, volume is directly proportional to temperature.

Charles’s Law Formula

V1T2 = V2T1

Avogadro’s Law

at constant temperature and pressure, the volume of a gas is directly proportional to the number of molecules (n)

Avogadro Formula

V1N2 = V2N1

number of molecules FORMULA

n = m/Mr

Gay-lussac’s Law

At constant volume, the pressure is directly proportional to the temperature

Gay-Lussac formula

P1T2 = P2T1

Ideal Gas Law

explains how gas will behave if you change the amount of molecules, size of the container, temp, and pressure

Ideal Gas Formula

PV = nRT

value of R (constant)

0.08206 L atm/mol K

Relationship of Average KE and absolute temp. of gas 

Directly Proportional 

motion of gases

move in straight lines until collision

Celsius to Kelvin

C + 273.15

Torr or mm Hg to atm

Torr or mm Hg * 0.00131579

molar mass (Mr)

g/mol

ML to L

ml/1000