Studied by 7 people
Temperature (unit: ℃ or K)
A measure of the average kinetic energy (per particle) of a system.
Heat (unit: J)
Energy transfer due to a temperature difference.
Internal Energy (unit: J)
The total kinetic and potential energy of the system. Note: For ideal gases, this energy is all kinetic
Heat capacity (unit: J K-1)
The amount of energy required to raise the temperature of a system by 1K
Specific Heat capacity (unit: J kg-1 K-1)
The amount of energy per unit mass required to raise the temperature of a given substance by 1K
Assumptions made for an ideal gas
The particles are in constant, random motion, only interacting through elastic collisions with each other and container walls.
A large number of identical particles with volumes negligible compared to the container volume.
Low density, which typically is the case for low pressure and high temperature
Specific latent heat of vaporization (unit: J kg-1)
The energy needed to convert one unit mass of liquid of a given substance to gas.
Specific latent heat of fusion (unit: J kg-1)
The energy needed to convert one unit mass of solid of a given substance to liquid.
Why temperature remains constant during state change
Intermolecular bonds are formed during freezing
Intermolecular PE decreases and difference transferred as heat
Average KE of molecules does not decrease/change
Temperature is related to average KE of molecules hence unchanged
Outline the difference between the molecular structure of a solid and a liquid
in solid state, nearest neighbour molecules cannot exchange places/have fixed positions/are closer to each other/have regular pattern/have stronger forces of attraction
in liquid, bonds between molecules can be broken and re-form
Note
Flashcard