Properties of Gases

Flashcards covering the properties of gases, gas laws, and the kinetic model of gases.

Intensive Properties

Properties that are independent of the amount of substance present, such as boiling point, color, and temperature.

Extensive Properties

Properties that depend on the amount of substance present, such as volume, mass, and length.

The Perfect Gas Equation of State

A fundamental relationship between the gas constant, Avogadro's number, and Boltzmann's constant.

Perfect Gas

Absence of molecular interactions.

Ideal Gas

Mixtures in which all molecular interactions are the same, but not necessarily zero.

Real Gas

Gases where intermolecular forces cause deviations from ideal behavior.

Standard Ambient Temperature and Pressure (SATP)

25 ℃ (298.15 K) and 1 bar (100 kPa).

Standard Temperature and Pressure (STP)

0 ℃ (273.15 K) and 1 atm (1.01325 bar).

Dalton's Law

The total pressure of a gas mixture is the sum of the partial pressures of each individual gas.

PA = xA * P

Partial pressure of a gas in a mixture.

Kinetic Model of Gases Assumptions

1. Ceaseless random motion, 2. Size is negligible (point-like), 3. Do not interact; all collisions are elastic.

Root-Mean-Square Speed (Vrms)

A measure of the average speed of gas particles.

Maxwell Distribution of Speeds

Describes the distribution of molecular speeds in a gas at a given temperature.

Diffusion

The spreading of molecules of one substance into a region initially occupied by another species.

Effusion

The escape of molecules through a small hole in a confining wall.

Graham’s Law of Effusion

The rate of effusion of a gas is inversely proportional to the square root of its molar mass.

Mean Free Path (λ)

Average distance a molecule travels between collisions.

Collision Frequency (z)

The average number of collisions a molecule undergoes per unit time.