Gases Review Flashcards

Flashcards to review gas laws and related concepts.

Kinetic Molecular Theory (KMT)

Describes the behavior of ideal gas particles.

Ideal Gas Particles

Tiny particles in large space with random constant motion, elastic collisions, no attractive forces, and kinetic energy directly proportional to temperature.

Pressure Conversions

1 atm = 760 mmHg = 760 Torr = 101.3 kPa = 14.7 psi

Boyle's Law

P1V1 = P2V2; inverse relationship between pressure and volume at constant temperature.

Charles' Law

V1/T1 = V2/T2; direct relationship between volume and temperature at constant pressure.

Gay-Lussac's Law

P1/T1 = P2/T2; direct relationship between pressure and temperature at constant volume.

Combined Gas Law

P1V1/T1 = P2V2/T2; relates pressure, volume, and temperature.

Ideal Gas Law

PV = nRT; relates pressure, volume, number of moles, and temperature.

Avogadro's Hypothesis

Explains how STP conditions are the same for every ideal gas; if P, V, and T are constant, then moles are also constant.

STP Conditions

1 mol, 1 atm, 273 K, 22.4 L

Boyle's Law

P1V1=P2V2 applies when temperature and moles are constant.

Charles' Law

V1/T1 = V2/T2 applies when pressure and moles are constant.

Gay-Lussac's Law

P1/T1 = P2/T2 applies when volume and moles are constant.

Combined Gas Law

Used when pressure, volume, and temperature change.

Ideal Gas Law

PV = nRT relates pressure, volume, number of moles, and temperature.

Volume change with temperature

Potato chip bags inflate on hot days due to Charles' Law.

Gas Stoichiometry

Using balanced equations to relate gas volumes and moles.

Ammonium sulfate production

2 NH3 (g) + H2SO4(l) → (NH4)2SO4 (aq)

Combustion of methane

CH4 + 2O2 -> CO2 + 2H2O

Haber Process

N2 + 3H2 -> 2NH3