Ideal+Gases 2

Gases

State of matter characterized by low interaction energy among individual particles relative to available thermal energy.

Pressure

Pressure is defined as Force per unit area (P = F/A).

Boyle's Law

At constant temperature, pressure and volume of a gas are inversely related (P1V1 = P2V2).

Charles's Law

At constant pressure, the volume of a gas is directly proportional to its temperature in Kelvin (V ∝ T).

Avogadro's Law

Under the same temperature and pressure, equal volumes of gases contain equal numbers of molecules.

Ideal Gas Law

The relationship of pressure, volume, temperature, and number of moles of a gas is given by PV = nRT.

Kinetic Molecular Theory

Theory describing the behavior of gas particles, emphasizing their random motion and negligible volume.

Diffusion

The process of intermolecular mixing of gas particles due to their kinetic motion.

Effusion

The escape of gas molecules through a tiny hole into a vacuum.

Real Gases

Gases that deviate from ideal behavior due to interactions between molecules and finite molecular volume.

Pascal (Pa)

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

Newton (N)

The SI unit of force, equivalent to the force required to accelerate one kilogram of mass at one meter per second squared.

Standard Temperature and Pressure (STP)

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

Molar Volume

Volume occupied by one mole of an ideal gas at STP is approximately 22.4 L.

Kinetic Energy (KE)

The energy of an object due to its motion, calculated as KE = 1/2 mv².

Potential Energy (PE)

The energy stored in an object due to its position or configuration.

Dalton's Law of Partial Pressures

In a mixture of non-reacting gases, the total pressure is the sum of the partial pressures of each gas.