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Physics > Thermodynamics > Flashcards

Thermodynamics Flashcards

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1
Q

Zeroth Law of Thermodynamics

A

if object 1 is in thermal equilibrium with object 2

and object 2 is in thermal equilibrium with object 3

then object 1 and object 3 are in thermal equilibrium and there will be no net heat flow

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2
Q

Temperature

A

proportional to the avg kinetic energy of the particles that make up the substance

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3
Q

Heat

A

transfer of thermal energy from an object with higher temp(energy) to an object with lower temp (energy)

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4
Q

Thermal Equilibrium

A

if there is no net heat flow between two objects in thermal contact, then their temperatures are the same

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5
Q

F,C, K of Absolute Zero

A

-460
-273
0

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6
Q

F,C, K of Freezing Point Water

A

32
0
273

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7
Q

F,C, K of Boiling Point Water

A

212
100
373

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8
Q

Absolute Zero

A

theoretical temperature at which there is no thermal energy

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9
Q

Third Law of Thermodynamics

A

entropy of a perfectly organized crystal at absolute zero is 0

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10
Q

Fahrenheit, Celsius and Kelvin Equations

A

F = 9/5 C + 32

K = 273 + C

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11
Q

Physical properties of matter that change as a function of temperature

A

Length, volume, solubility and conductivity

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12
Q

Thermal Expansion of Matter: Length

A

delta L = alpha * L * delta T

alpha = coefficient of linear expansion

as temp goes up, length increases
as temp goes down, length decreases

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13
Q

Thermal Expansion of Matter: Volume Expansion

A

delta V = beta * V * delta T

beta = coefficient of volumetric expansion

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14
Q

Relation between Coefficient of Volumetric Expansion (beta) and Linear Expansion (alpha(

A

B = 3 * alpha

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15
Q

Isolated Systems

A

not capable of exchanging energy or matter with their surroundings ; total change in internal energy must be zero

very rare: examples are bomb calorimeter and the entire universe

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16
Q

Closed Systems

A

capable of exchanging energy, but not matter, with the surroundings

gases in vessels with movable pistons

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17
Q

Open Systems

A

exchange both matter and energy with the environment

matter carries energy but can be transferred via heat/work

boiling pot of water, humans, unconstrained combustion’s

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18
Q

State Functions

A

thermodynamic properties that are a function of equilibrium state of a system ; aka independent of the path taken to reach equilibrium

pressure, density, temperature, volume, enthalpy, internal energy, gibbs free energy, entropy

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19
Q

Process Functions

A

work and heat

describe the path taken to get from one state to another

20
Q

First Law of Thermodynamics

A

change in total internal energy of a system is equal to the amount of energy transferred in the form of heat to the system minus the amount of energy transferred from the system in the form of work

deltaU = Q - W

21
Q

deltaU = Q - W

A

U = change in systems internal energy

Q = heat flow into system

W = work done by the system

+ = increasing temp, heat flow into system, work done by the system (expansion)

  • = decreasing temp, heat flow out of system, work is done on the system
22
Q

Second Law of Thermodynamics

A

objects in thermal contact, but not thermal equilibrium will exchange heat energy going from high temp to lower temp until they have the same temperature at thermal equilibrium

23
Q

Conduction

A

direct transfer of energy from molecule to molecule through molecular collisions (physical contact)

metals are good because they have a density of atoms in a sea of electrons while gases are bad because atoms have space between them

24
Q

Convection

A

transfer of heat by physical motion of a fluid over a material

only liquids/gases apply

if fluid has a higher temperature, it will transfer energy to the material

25
Q

Radiation

A

transfer of eneergy via electromagnetic waves

unlike the other two forms, can transfer energy through a vacumn

26
Q

When heat energy is added/removed from a system, the temperature of that system will change in proportion to the amount of heat transfer, unless the system is undergoing ______ during which the temperature is ____

A

phase change

constant

27
Q

Specific Heat (c)

A

amount of heat energy required to raise one gram of a substance by one degree C/K

changes according to its phase

1 cal/gK for water (need to know this)

28
Q

Heat Gained/lost Equation

A

q=mc deltaT

c = specific heat of the substance

29
Q

Phase change occurs at _____ temperature and the temperature will not begin to change until _____ has been converted from one phase into the other.

A

constant

all of the substance

30
Q

Phase changes are related to changes in _____ energy, not ____ energy.

A

potential

kinetic

31
Q

While liquid water may have a greater number of ______ due to increased freedom of movement, its avg kinetic energy is the ____ as solid water at the same temperature.

A

microstates

same

32
Q

Microstates Ex: Water

A

As a solid, the atoms are bound by hydrogen atoms to restrict movement, but there is kinetic energy of the atoms vibrating

When heated up, water molecules move away, breaking the H bonds to increase degrees of freedom and increasing potential energy

however, the normal vibration activity also decreases as there are more methods of moving now

33
Q

When heat energy is added or removed from a system experiencing phase change, _____ cannot be used to calculate heat added as there is no temperature change.

Instead, ______ is used where L is ______

A

q=mcdelta T

q=mL

heat of transformation/latent heat

34
Q

Liquid to Solid Phase Change is called

A

freezing/solidification

35
Q

Solid to Liquid phase change is called

A

melting/fusion

36
Q

Liquid to Gas phase change is called

A

boiling, evaporation, vaporization

37
Q

Gas to Liquid phase change is called

A

condensation

38
Q

Isothermal

A

a process where Q = W

work = heat flow

delta U = 0 so constant temperature

39
Q

Adiabatic

A

delta U = -W

delta U = change in systems internal energy

W = work

Q = 0 = heat flow so no heat flow

40
Q

Isobaric

A

constant pressure

41
Q

Isovolumetric /Isochoric

A

W = 0 so no work

deltaU = Q

42
Q

Energy Dispersion

A

energy goes from being localized to being spread out/disperesed

43
Q

Entropy

A

measure of the spontaneous dispersal of energy at a specific temperature

44
Q

The larger the number of ______ energy can be spread out over, the higher the ___.

A

microstates

entropy

45
Q

Change In Entropy Equation

A

delta S = Qrev / T

Qrev = heat gained/lost in reversible process

T = temp in kelvin

J/mol*k

46
Q

When energy is distributed into a system at a given temperature, its entropy ____ . When energy is distributed out of a system at a given temperature, its entropy _____

A

increaes.

decreases

47
Q

When energy is distributed into a system at a given temperature, its entropy ____ . When energy is distributed out of a system at a given temperature, its entropy _____

A

increase.

decreases

Physics (4 decks)

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