Ideal Gases Flashcards

Vocabulary flashcards based on IB topic S1.5 regarding Kinetic Theory of Gases, ideal and real gases, Avogadro's Law, STP, and gas equations.

Kinetic Theory of Gases

A model describing gas behavior at a molecular level, proposing that gas particles move in straight lines in random directions, temperature is proportional to average kinetic energy, and pressure depends on the frequency and force of collisions with container walls.

Ideal Gas

A theoretical gas whose particles have negligible volume compared to the container, display no intermolecular forces (no attraction or repulsion), and undergo elastic collisions with no kinetic energy lost.

Elastic Collisions

Collisions between gas particles or with container walls in which no kinetic energy is lost.

Real Gases

Gases that deviate from ideal gas behavior under conditions of low temperature and high pressure, where particle volume, intermolecular forces, and energy lost in collisions become significant.

Avogadro's Law

A law stating that equal volumes of ideal gases, measured at the same temperature and pressure, contain the same number of molecules.

Standard Temperature and Pressure (STP)

Standard reference conditions defined as a temperature of $273.15\,K$ and a pressure of $100\,kPa$.

Molar Volume of an Ideal Gas

The volume occupied by $1\,mol$ of an ideal gas at standard temperature and pressure ($\text{STP}$), which is equal to $22.7\,dm^3$.

Ideal Gas Equation

The equation $PV = nRT$ that describes the overall relationship between volume, temperature, pressure, and number of particles in an ideal gas.

Gas Constant ($R$)

The physical constant in the ideal gas equation with a value of $8.31\,J\,K^{-1}\,mol^{-1}$.

Combined Gas Equation

An equation that brings together different gas laws to calculate changes in pressure, volume, or temperature of a fixed sample of ideal gas between initial and final states.