Chapter 9 Gases Study Guide Flashcards

A set of flashcards covering key terms and concepts related to gases from Chapter 9.

Pressure

The force exerted per unit area by gas molecules against the walls of their container.

Pascal (Pa)

The SI unit of pressure, defined as one newton per square meter.

Bar

A unit of pressure that is defined as 100,000 pascals.

Atmosphere (atm)

A unit of pressure defined as 101,325 pascals, approximately equal to atmospheric pressure at sea level.

Torr

A unit of pressure equal to 1/760 of an atmosphere.

Boyle’s Law

A gas law stating that the pressure of a gas is inversely proportional to its volume at constant temperature.

Charles’s Law

A gas law stating that the volume of a gas is directly proportional to its temperature at constant pressure.

Avogadro’s Law

A gas law stating that the volume of a gas is directly proportional to the number of moles of gas at constant temperature and pressure.

Ideal Gas Law

The equation of state for an ideal gas, represented as PV = nRT.

Standard Temperature and Pressure (STP)

A standard set of conditions for experimental measurements, defined as 0°C and 1 atm.

Kinetic Molecular Theory

A theory that describes gases as particles in constant motion and explains the behavior and properties of gases.

Mean Free Path

The average distance traveled by a gas molecule between collisions.

Diffusion

The process by which gas molecules spread from an area of higher concentration to an area of lower concentration.

Effusion

The process by which gas escapes through a tiny opening into a vacuum.

Dalton’s Law of Partial Pressures

A law stating that the total pressure of a gas mixture is equal to the sum of the partial pressures of each individual gas.

Compressibility Factor (Z)

A factor that accounts for deviations from ideal gas behavior, defined as Z = PV/nRT.