Flashcards on Kinetic theory

Define Mole

The S.I. unit of an ‘amount of substance’ containing as many particles as there are atoms in 12 g of carbon-12.

What is Avogadro’s constant (NA)

The number of particles in 1 mole of a substance, equal to 6.02×10²³ mol^-1.

What are Ideal gases

Gases that follow specific relationships between pressure, volume, and temperature, described by the ideal gas law.

What is the Ideal gas law?

pV = nRT

p is pressure,

V is volume

n is the number of moles

R is the molar gas constant

T is temperature.

Molar gas constant (R)

A constant used in the ideal gas law, equal to 8.31 J mol^-1 K^-1.

What is Boltzmann constant (k)

A constant used in the equation pV = NkT for ideal gases, equal to 1.38×10^-23 J K^-1.

Define Molar mass (M)

The mass of 1 mole of a substance, linked to the relative molecular mass (Mr) of a molecule.

Define Kinetic energy

The energy associated with the motion of molecules, which can be expressed for a gas in terms of its temperature and number of molecules.

Define Kinetic theory

A theory that describes the behavior of gases based on the motion and collisions of molecules, assuming no loss of kinetic energy during collisions.

Define Pressure

The force exerted by gas molecules colliding with the walls of a container

calculable using the density, number of molecules, and mean squared speed.

What is Mean squared speed (c²)

A representation of the average speed squared of gas molecules, important for calculating pressure and energy distribution.

What assumptions are made when using the ideal gas equation?

1. Collisions are perfectly elastic - no KE lost when particles bounce off container walls

2. Gas Particles exert a force on each other only when they collide

3. Volume is negligible due to tiny size.