Gas Laws and Kinetic Molecular Theory

A set of flashcards covering key concepts about gas laws and kinetic molecular theory for exam preparation.

What is the Kinetic Molecular Theory (KMT)?

A model that explains the behavior of gases in terms of pressure, volume, temperature, velocity, frequency, and force of collisions.

What are the assumptions of the Kinetic Molecular Theory?

1. Gases consist of large numbers of particles in constant, random motion. 2. The volume of gas particles is negligible. 3. There are no forces of attraction between gas particles. 4. Collisions are perfectly elastic. 5. Gases have low density.

Under what conditions do gases behave most ideally?

High temperature and low pressure.

What affects the behavior of real gases compared to ideal gases?

Real gases have a small volume and do exert some attractive forces on each other.

What is Boyle's Law?

Describes the inverse relationship between the pressure and volume of a gas at constant temperature: P1V1 = P2V2.

What does Charles' Law state?

Volume is directly related to temperature (in Kelvin) when pressure is held constant.

What is Gay-Lussac's Law?

Describes the direct relationship between the pressure and temperature of a gas at constant volume.

What is the combined gas law?

P1V1/T1 = P2V2/T2, which combines Boyle's, Charles', and Gay-Lussac's laws.

What is Avogadro's Law?

Equal volumes of gases at the same temperature and pressure contain equal numbers of particles.

How do you calculate the density of a gas at STP?

Density = Molar Mass (g/mol) / 22.4 L.

What does Graham's Law describe?

The rates of effusion of two gases are inversely proportional to the square roots of their molar masses.

What are the units for pressure, volume, and temperature in the Ideal Gas Law?

Pressure in atm or kPa, Volume in liters, Temperature in Kelvin.

What is the ideal gas law equation?

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

How does temperature affect gas density?

As temperature increases, gas density typically decreases due to increased particle movement.

What is entropy?

A measure of disorder or randomness of particles in a system.

What happens to gas particles at low temperatures and high pressures?

Gas particles move slower and are closer together, resulting in increased attraction and deviation from ideal behavior.