oat chem unit 6

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gas molecules

have no definite size or shape, are widely separated, and can be easily compressed. They are in random constant motion.

diatomic gases

gases that consist of atoms in pairs due to unstable nature, like H₂, N₂, F₂, O₂, I₂, Cl₂, Br₂ (have no fear of ice cold beer)

temperature

measurement of kinetic energy or movement of gas particles.

volume

The amount of space a substance occupies. Gases take both the shape and the volume of the container.

pressure

Force of the gas particles colliding with the walls of the container.

• P = F/A

• ^ pressure, force, area

gas compressed

less volume = more collision = more pressure.

gas expanded

more volume = less collision = less pressure.

boyle’s law

P₁V₁ = P₂V₂ (pressure and volume)

charles’s law

V₁/T₁ = V₂/T₂ (volume and temperature in K)

avogadro’s law

V₁/n₁ = V₂/n₂ (volume and number of moles)

gay lussac’s law

P₁/T₁ = P₂/T₂ (pressure and temperature in K)

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combined gas law

P₁V₁/T₁n₁ = P₂V₂/T₂n₂ (pressure, volume, temperature in K, number of moles)

ideal gas

behaves in constant, random, straight line motion according to the kinetic molecular theory of gases.

kinetic molecular theory of gases

• Particles in a gas are in constant random motion

• Combined volume of particles in negligible

• Particles exert no force on each other

• Collisions are completely elastic (no IMFs)

• All gases have the same average kinetic energy at a given temperature.

ideal gas law

The ratio of pressure (atm) and volume (L) to moles, temperature (K) and a constant to depict the behavior of an ideal gas.

• PV = nRT.

• R = ideal gas constant

  • If pressure is atm: R = 0.0821

  • If pressure is kPa: R = 8.314

standard temperature and pressure

• Temperature: 273 Kelvin

• Pressure: 1 atm

dalton’s law of partial pressure

Total pressure of a mixture is equal to the sum of partial pressures of individual gases.

• P_total = P₁ + P₂ + P₃ …

• P₁ = X₁P_total

  • X = mole fraction

gas density

The mass of a gas occupying a certain volume.

• p = m/V = PM/RT

• ^ density, mass, volume, pressure, molar mass, ideal gas constant, temperature.

diffusion

molecules move from high to low concentration.

effusion

Confined gas escaping through a small hole. A gas with lower molecular weight effuses faster.

• Rate: Gas > liquid > solid

graham’s law of effusion

M = molar mass, r = effusion rate.

vaessen’s law

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