Gaseous State

Boyle's Law
P1V1 = P2V2 = constant

Charle's Law
V = Vo(1 + T/273.15)

Gay Lussac's Law
V1/ T1= V2/undefinedT2 = constant

Avogadro's Law
V α n

Ideal Gas Equation
PV = nRT

P = dRT / M

P1V1/ T1= P2V2/ T2

Dalton's Law of Partial Pressures
(only for non-reacting gases)

PT = P1+ P2+ P3 + ........ +Pn

Where, P1= x1P1 ; x1= n1/ nT ( x = mole fraction )

Graham's Law of Diffusion
Rate of diffusion (r) = Volume of Gases Diffused                                                                                                                                 --TIme

r = V/t
r1 / r2 = V1T2/ V2T1 r α 1/√d

... r1/ r2= √ (d2/d1)

... r1/ r2= √ (M2/ M1)

Amagat's Law of Equal Volumes

The total volume of a gas mixture is equal to the sum of partial volumes of individual gases.

Van der Wahl's Equation or Real Gas Equation
(for real gases)

(P+(a/V2))(V-b) = RT  {for 1mole }

(P+(an/V2))(V-nb) = nRT

Unit of a = atm lit2/ mol2

Unit of b = lit / mol

Note : For Low Pressure, ignore b and for low volme ignore a.

Standard Temperature Pressure
Temperature : 0o C = 273 K

Pressure = 1 atm = 1.0132 x 105N/m2(Pa)

Kinetic Theory of Gases
(& relation with temperature)

Mean Square Velocity
Average Velocity

Most Probable Velocity