Gases and the Ideal Gas Law

These flashcards cover key terms and definitions related to the properties and behaviors of gases and the Ideal Gas Law, as discussed in the lecture notes.

Ideal Gas Law

Describes the behavior of an ideal gas in relation to pressure, volume, temperature, and number of moles.

Boyle's Law

States that the pressure of a gas is inversely proportional to its volume when temperature and the number of moles are held constant.

Charles's Law

States that the volume of a gas is directly proportional to its temperature in Kelvin when pressure and the number of moles are constant.

Avogadro's Law

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

Dalton's Law of Partial Pressures

States that the total pressure of a mixture of gases is equal to the sum of the partial pressures of the individual gases.

Gas Density

The mass per unit volume of a gas, which is proportional to its molar mass.

Pressure (P)

The force exerted by gas particles colliding with the walls of a container, measured in atmospheres (atm), Pascals (Pa), or Torr.

Temperature (T)

A measure of the average kinetic energy of gas particles, measured in Kelvin (K).

Volume (V)

The amount of space that a gas occupies, typically measured in liters (L).

Molar Mass (M)

The mass of one mole of a substance, usually measured in grams per mole (g/mol).

Root Mean Square Speed (v)

A measure of the average speed of gas particles, calculated from the temperature and molar mass.

Kinetic Energy (Ek)

The energy that a gas particle possesses due to its motion, directly proportional to its temperature.

Gas Effusion

The process by which gas particles pass through a tiny opening into an empty space.

Gas Diffusion

The process by which gas molecules mix due to their random motion.

Barometric Pressure

The pressure exerted by the weight of the air in the atmosphere, variable with altitude.

STP (Standard Temperature and Pressure)

Defined as 0 °C (273.15 K) and 1 atm (101.325 kPa), used for comparisons in gas laws.

Intermolecular Forces

Forces of attraction between particles that are negligible in ideal gas behavior.

Van der Waals Equation

An adjustment of the ideal gas law that accounts for intermolecular forces and the volume occupied by gas particles.

Molar Volume

The volume occupied by one mole of a gas at standard temperature and pressure, approximately 22.4 L.

Liquid Gas Transition

The process where a substance changes from a liquid to a gas due to temperature increase.