Gas Laws

Ideal Gas Law

“Pivnert”

PV = nRT

P in atm

V in liters

n in moles

R  = 0.0821(L atm) / (mol K) (latum mulk)

T in Kelvin

Stoichiometry Molar Volume

1 Mole of any gas = 22.4 Liters of that gas

Boyle’s

P1V1 = P2V2

Inversely proportional

Boyle’s explanation

ncreasing volume decreases pressure because particles have to move farther to reach sides

Charles

(V1) / (T1) = (V2) / (T2)

Directly proportional

Charles Explanation

If increase temperature, in order to keep pressure constant (frequency of collisions stays the same), volume must expand bc if particles move faster but also move farther they’ll hit the sides with same frequency as before

Gay-Lussac

(P1) / (T1) = (P2) / (T2)

Directly proportional

Gay-Lussac explanation

Increasing temperature (while keeping volume constant), pressure increased bc particles are moving faster

Avogadro

(n1) / (V1) ‎ =  (n2) / (V2)

Directly proportional

Combined

((P1)(V1)) / (T1) = ((P2)(V2)) / (T2)

Atm to torr

1 atm = 760 torr

Celsius to Kelvin

0 C = 273 K

STP (Temperature)

0 Celsius

273 Kelvin

STP (Pressure)

1 atm

760 torr

760 mmHg

101.3 kPa

29.9”Hg

Dalton

P total = Pa + Pb + Pc

Collecting Gas over Water

Total P = P(water vapor at that temp) + P(other gas)