Gases and Pressure - Lecture Review

These flashcards cover key concepts, laws, and definitions related to gases and pressure as discussed in the lecture.

Boyle's Law

States that the volume of a fixed mass of gas varies inversely with the pressure at constant temperature.

Charles's Law

States that the volume of a fixed mass of gas at constant pressure varies directly with the Kelvin temperature.

Avogadro's Law

States that equal volumes of gases at the same temperature and pressure contain equal numbers of molecules.

Dalton's Law of Partial Pressures

The total pressure of a gas mixture is the sum of the partial pressures of the component gases.

Kinetic Molecular Theory

Describes the behavior of gas particles and how they interact with each other and their environment.

Pressure

Defined as the force per unit area exerted on a surface.

Standard Temperature and Pressure (STP)

Defined as 0°C (273.15 K) and 1 atmosphere (atm) of pressure.

Ideal Gas Law

Expressed as PV=nRT, it relates pressure (P), volume (V), number of moles (n), and temperature (T) of an ideal gas.

Diffusion

The gradual mixing of two or more gases due to spontaneous, random motion.

Graham's Law of Effusion

States that the rates of effusion of gases at the same temperature and pressure are inversely proportional to the square roots of their molar masses.

Barometer

A device used to measure atmospheric pressure.

Pascal (Pa)

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

Atmospheric Pressure

The pressure exerted by the weight of the atmosphere, approximately 101.325 kPa at sea level.

Vapor Pressure

The pressure exerted by a vapor in equilibrium with its liquid or solid form at a given temperature.

Combined Gas Law

Combines Boyle's, Charles's, and Gay-Lussac's laws into one equation: (P1V1)/T1 = (P2V2)/T2.

Ideal Gas Constant (R)

A constant that relates pressure, volume, temperature, and number of moles in the ideal gas equation.