Gas Laws and Kinetic Molecular Theory

Flashcards covering gas laws, kinetic molecular theory, and related concepts.

Dalton's Law of Partial Pressures

In a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of the individual gases: Pt = PA + PB + PC + …

Diffusion

The process of a substance spreading out to evenly fill its container or environment. Molecules move towards areas of lower concentration until the concentration is uniform throughout the system.

Boyle's Law

P1V1 = P2V2 (Temperature and moles held constant; Inversely proportional relationship between pressure and volume)

Charles's Law

V1/T1 = V2/T2 (Pressure and moles held constant; Directly proportional relationship between volume and temperature)

Gay-Lussac's Law

P1/T1 = P2/T2 (Volume and moles held constant; Directly proportional relationship between pressure and temperature)

Combined Gas Law

Moles held constant. Combines Boyle's, Charles's, and Gay-Lussac's Laws.

Ideal Gas Law Constant (R) in atmospheres

R = 0.0821 atm L/(K mol)

Ideal Gas Law Constant (R) in kilopascals

R = 8.31 kPa L/(K mol)

Partial Pressure

The pressure exerted by an individual gas in a mixture of gases.

Kinetic Molecular Theory: Temperature and Kinetic Energy

The relationship is directly proportional. As the Kelvin temperature increases, the average kinetic energy increases. If the Kelvin temperature doubles, the average kinetic energy will double.

Ideal Gases (Kinetic Molecular Theory)

Gases are assumed to have no volume and no attractive forces between gas particles.

Real Gases (Kinetic Molecular Theory)

Real gas particles do have volume and there are attractive forces between gas particles.

Graham's Law of Effusion

R1/R2 = [ M2/M1]1/2

Molar Mass Calculation (Density)

Molar Mass = DRT)/ P