SL Chem - Unit #3: Boyles, Charles', Gay-Lussac's, Dalton's, Avogadro's, Ideal, Combined Gas laws

Boyle's Law:

• When the pressure of a gas increases its volume decreases and vice versa

• Volume of a fixed mass with a constant temperature of ideal gas is inversely proportional to its pressure (Makes an exponential graph)

Boyle’s Law Formula

P₁V₁ = P₂V₂

Charles Law:

When we have a fixed mass of a gas at a constant pressure, it’s volume is directly proportional to the temperature

• So as temp increases, volume increases (makes a linear graph)

Charl'e’s Law Formula

• V1/T1= V2/T2 

Gay-Lussac’s Law:

When we have a fixed mass of a gas at a constant volume, the pressure is directly proportional to the temperature

• So as temp increases pressure also increases (makes a linear graph)

Gay-Lussac’s Law Formula

P1/T1= P2/T2

Combined Gas Law:

(P₁V₁)/T₁ = (P₂V₂)/T₂

Dalton’s Law

P_t = P₁ + P₂ + P₃….

Dalton’s Law when gas is collected over water

P_{dry gas}  =  P_atm  -  P_H2O

Ideal Gas Law:

PV = nRT

• P = pressure (in kPa)

• V = volume (in L)

• n = moles

• T = temperature (in K)

• R = 8.31

Density Formula

Density = mass/volume

Molar Volume

Molar Volume = volume/mol

Avogadro’s Hypothesis

Equal number of particles of ideal gasses occupy an equal volume when at a constant temp and pressure

Avogadro’s Hypothesis Formula

n₁/V₁= n₂/V₂

Molar Volume

The volume occupied by 1 mol of gas at constant temp/pressure

Molar Volume of an Ideal gas at STP

22.7 L/mol