Title: Theory / Unimportant / Experimental / Physics / Thermodynamic - VSI
Tags: examplesSwitchExample1 hasSeenConjDef toBinaryRelation typToBinary récupéré
On every note of this deck, unless a note says otherwise:
Chapter: 1

Name: A system
Definition: part of the universe that is at the centre of attention
Page: 1
Context: thermodynamics

Name: The surroundings
Definition: Everything in the univers, with the exception of the system
Page: 1
Context: thermodynamics

Name: The universe
Definition: A system and its surroundings
Page: 2
Context: thermodynamics
Example: Approximated by: beaker of water immersed in a water bath

Name: An open system
Definition: A system in which matter can be added or removed
Page: 2
Context: thermodynamics

Name: A closed system
Definition: A system in which matter can neither be added nor removed
Page: 2
Context: thermodynamics

Name: An isolated system
Definition: A system which remains unchanged regardless of anything that happens in the surroundings
Page: 2
Context: thermodynamics

Name: Flexible wall
Definition: the boundary of the system is rigid everywhere except for a patch—a piston—that can move in and out
Page: 2
Context: thermodynamics

Name: Extensive property
Definition: Property depending on the quantity of matter in the system
Page: 2
Context: thermodynamics
Example: mass, volume

Name: Intensive property
Definition: Property independant on the quantity of matter in the system
Page: 2
Context: thermodynamics
Example: Temperature
Example2: density

Name: A piston
Definition: a movable patch in the boundary of a system
Page: 3
Section: Introducing equilibrium
Context: thermodynamics

Page: 4
Definition: Condition arising from the equality of pressure
Chapter: 1
Section: Introducing equilibrium
Name: Mechanical equilibrium
Context: thermodynamics
Transitive: Equivalence relation

Page: 4
Definition: The fact that there is no difference if s touch t or not (using diathermic walls)
Chapter: 1
Section: Introducing equilibrium
Variables: s, t two systems
Name: Thermal equilibrium of s and t
Context: thermodynamics
Equivalence: Equivalence relation

Name: zeroth law of thermodynamics
Definition: Being in thermal equilibrium is an equivalence relation
Page: 5
Section: Introducing equilibrium
Context: thermodynamics

Name: Temperature
Definition: A universal property allowing to know whether two things are in thermal equilibrium
Page: 6,11
Section: Introducing equilibrium
Context: thermodynamics
Definition2: the parameter that tells us the most probable distribution of populations of molecules over the available states of a system at equilibrium

Name: diathermic wall
Definition: walls which permit the conduction of heat
Page: 6
Section: Introducing equilibrium
Context: thermodynamics
Example: Saucepans
Etymology: ‘through’ and ‘warm'

Name: adiabatic wall
Definition: walls which are thermally insulated
Page: 6
Section: Introducing equilibrium
Context: thermodynamics
Example: vacuum flask
Example2: if the system is embedded in foamed polystyrene

Name: Thermometer
Definition: device for measuring temperature
Page: 6
Section: Introducing equilibrium
Context: thermodynamics

Name: Fahrenheit
Page: 6
Section: Introducing equilibrium
Context: thermodynamics
Intuition: Lowest temperature the creator can obtain with salt, ice and water is 0. Its body temperature is 100

Name: thermodynamics temperature
Definition: Absolute temperature, with 0 the theoretical minimum
Page: 6
Section: Introducing equilibrium
Context: thermodynamics
Typ: Kelvin
Denoted by: \(T\)

Name: Rankine scale
Definition: Absolute temperature, with 0 the theoretical minimum and scale as in Fahrenheit
Page: 6
Section: Introducing equilibrium
Context: thermodynamics

Name: Classical thermodynamics
Definition: emerged during the nineteenth century
Page: 8
Section: Introducing equilibrium
Context: thermodynamics
Definition2: can be done without considering atoms
Conjdef: part of thermodynamics that

Name: Statistical thermodynamics
Definition: account for the bulk properties of matter in terms of its constituent atoms.
Page: 8
Section: Introducing equilibrium
Context: thermodynamics
Conjdef: part of thermodynamics that
Intuition: in the discussion of bulk properties we don’t need to think about the behaviour of individual atoms but we do need to think about the average behaviour of myriad atoms.

Name: Thermodynamics
Definition: Mecanic which deals with the average behaviour of vast numbers of individual body.
Page: 9
Section: Introducing equilibrium

Question: What is the important condition on atoms that thermodynamic needs to consider.
Answer: Each atom can be in only one of finitely many states
Page: 9
Chapter: 1
Section: Introducing equilibrium
Context: thermodynamics

Name: An atom in ground state
Definition: An atom with lowest energy state
Page: 9
Section: Introducing equilibrium
Context: thermodynamics

Name: Boltzmann distribution
Definition: The ration of population of state of energy E to population of state at ground energy is \(e^{-\beta E}\)
Page: 10
Section: Introducing equilibrium
Context: thermodynamics
Intuition: The precise form of the distribution of the molecules over their allowed states

Name: Boltzmann's constant
Abbreviation: \(k\)
Chapter: 1
Page: 11
Represents: Allow to relate temperature and energy
Exponant: -23
Section: Introducing equilibrium
Typ: joule/kelvin
s: -2
m: 2
Significative digit: 1.38
Basis: 10
Kelvin: -1

Name: Allow to relate temperature and energy
Chapter: 1
Page: 11
Section: Introducing equilibrium
Etymology: 10
Denoted by: joule/kelvin

Definition: \(\frac{1}{kT}\) with \(k\) being Boltzmann's constant and \(T\) being the temperature of C
Page: 11
Section: Introducing equilibrium
Variables: C a collection of molecule
Notation: \(\beta\)

Question: Why do we use temperature and not Boltzmann's parameter in every day life
Answer: C and K allow to have two digits for most temperature we want to consider, and not 20
Page: 12
Chapter: 1
Section: Introducing equilibrium

Name: Gas
Definition: chaotic assembly of molecules
Page: 13
Section: Introducing equilibrium

Name: Maxwell–Boltzmann distribution of speeds
Definition: the average speed of the molecules increases as the square root of the absolute temperature
Page: 13
Section: Introducing equilibrium
Variables: S a system containing a gas of molecule