Gas Law Contributors

Front 1

Avogadro's

Back 1

(no duh principle)

V/n = K

(V1/N1) = (V2/N2)

fixed pressure and temperature, more particles means more volume

Front 2

Boyle's

Back 2

syringe

PV = K

P1V1=P2V2

fixed n, T

if you decrease the volume of a container, the pressure will increase

Front 3

Charles'

Back 3

V/T = K

V1/T1 = V2/T2

fixed P, N

if you heat up a sample of fixed moles and pressure, the volume will increase

Front 4

Diver's

Back 4

if you add moles to a container of fixed volume and temperature, the pressure will increase

P/n = k

P1/n1 = P2/n2

fixed T, V

Front 5

Dalton's

Back 5

P(total) = P1 + P2 + P3 + ... + Pn

Front 6

Graham's

Back 6

1/2 m1 (v1)^2 = 1/2 m2 (v2) ^2

fixed T, P

at a fixed temperature and pressure, all gases have the same amount of kinetic energy

Front 7

Henry's

Back 7

Partial pressure = K (concentration)

Front 8

in fixed volume and temperature (same container), the mole fraction "chi" is equal to the pressure fraction of a gas present.

n1/(ntotal) = P1/(Ptotal)

Back 8

therefore!

P1 = (n1/ntotal) * (Ptotal)

Front 9

Kinetic Molecular Theory

Back 9

1. molecules aren't attracted to each other
2. molecules have no volume
3. collisions between molecules are completely elastic
4. molecules move faster when temperature is increased
5. pressure is the result of molecules striking their container

Front 10

KE(avg) of a gas

Back 10

(3/2)(RT)

Front 11

vavg, or u("root mean square")

Back 11

root[(3RT)/(M)]