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Thermodynamics Flashcards

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1
Q

What is the zeroth law of thermodynamics?

A

when Object A is in thermal equilibrium with Object B, and Object B is in thermal equilibrium with Object C, then Object A and C are also in thermal equilibrium and no net heat flow happens

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2
Q

Temperature

A

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

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3
Q

Heat

A

is the transfer of thermal energy from high temp/energy objects to low temp/energy objects (Unit = J)

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4
Q

Thermal Equilibrium

A

when there is no net heat flow between two objects and they are the same temp

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5
Q

Freezing and Boiling Points in Celsius

A

0, 100

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6
Q

Freezing and Boiling Points in Fahrenheit

A

32, 212

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7
Q

Freezing and Boiling Points in Kelvin

A

273, 373

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8
Q

Absolute Zero

A

theoretical temperature in which there is no thermal energy. K = 0, F = -460, C = -273

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9
Q

What is the third law of thermodynamics?

A

the entropy of a perfectly organized crystal at absolute zero is zero

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10
Q

How do you interconvert F and C?

A

F = 9/5C + 32

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11
Q

How do you interconvert C and K?

A

K = C + 273

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12
Q

Thermal Expansion

A

a change in the temperature of most solids results in a change in their length

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13
Q

What is the equation to measure linear thermal expansion?

A 
deltaL = alpha*L*deltaT
DeltaL = change in length
alpha = coefficient of linear expansion
L = original length
deltaT = change in temperature
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14
Q

What is a coefficient of linear expansion?

A

constant that characterizes how a specific material’s length changes the temperature changes. Called alpha, Units = K^-1

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15
Q

What is the equation for volumetric thermal expansion?

A 
deltaV = beta*V*deltaT
DeltaV = change in volume
Beta = coefficient of volumetric expansion
DeltaT = change in temp
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16
Q

What is the coefficient of volumetric expansion?

A

exactly what it sounds like - constant that characterizes how a specific material’s volume changes as the temperature changes. Called beta, Units = K^-1

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17
Q

What is the relationship between the linear expansion and volumetric expansion coefficients?

A

beta = 3alpha

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18
Q

Isolated Systems

A

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

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19
Q

Closed Systems

A

capable of exchanging energy but not matter with their surroundings

20
Q

Open Systems

A

can exchange both matter and energy with the surroundings

21
Q

State Functions

A

thermodynamic properties that are a function of only the current equilibrium state of a system. They are independent of that path they take to get to a particular equilibrium state

Ex: pressure, density, temp, volume, enthalpy, internal energy, Gibbs free energy, and entropy

22
Q

Process Functions

A

describe the path taken to get from one state to another

Ex: work, heat

23
Q

First Law of Thermodynamics

A

states that the change in the 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 form the system in the form of work.

24
Q

Equation for change in internal energy

A 
deltaU = Q - W
deltaU = change in system's internal energy
Q = energy transferred into the system as heat
W = work done by the system
25
Q

Second Law of Thermodynamics

A

objects in thermal contact and not in thermal equilibrium will exchange heat energy such that the object with the higher temperature will give off heat energy to the object with the lower temperature until both objects have the same temperature at thermal equilibrium

26
Q

1 Cal = ? J

A

4184 J

27
Q

Conduction

A

the direct transfer of energy from molecule to molecule through molecular collisions. Must have direct contact, metals are best at this

28
Q

Convection

A

the transfer of heat by a physical motion of a fluid over a material; only liquid and gases can transfer heat. This is a common use in convection ovens

29
Q

Radiation

A

the transfer of energy by electromagnetic waves; only way to transfer energy in a vacuum

30
Q

Specific Heat

A

Specific heat (c) of a substance is defined as the amount of heat energy required to raise one gram of a substance by one degree C or one unit K.

31
Q

What is the specific heat of water in calories?

A

1 cal/ g*K

32
Q

What is the equation that relates heat gained or lost by an object and the change in temp of that object?

A 
q = mcdeltaT
q = amount of heat gained or lost from the material
m = mass
c = specific heat of the substance
deltaT = change in temp (C or K)
33
Q

What is the equation for calculating the amount of heat added or removed for phase changes?

A 
q = mL
q = amount of heat gained or lost from the material
m = mass 
L = heat of transformation(fusion or vaporization)/latent heat - will be provided
34
Q

Solid to Liquid is

A

fusion/melting

35
Q

Liquid to Solid is

A

freezing/solidification

36
Q

Liquid to Gas is

A

boiling/evaporation/vaporization

37
Q

Gas to Liquid is

A

condensation

38
Q

Solid to Gas is

A

sublimation

39
Q

Gas to Solid is

A

deposition

40
Q

What is the heat of transfer called when it occurs at a melting point?

A

heat of fusion

41
Q

What is the heat of transfer called when it occurs at a boiling point?

A

heat of vaporization

42
Q

What is a process with constant temp called and its equation?

A

isothermal (deltaU = 0)

Q = W

43
Q

What is a process with no heat exchange called and its equation?

A

adiabatic (Q = 0)

deltaU = - W

44
Q

What is a process with constant volume called and its equation?

A

isovolumetric/isochoric (W = 0)

deltaU = Q

45
Q

Entropy

A

measure of the spontaneous dispersal of energy at a specific temperature: how much energy is spread out or how widely spread out energy becomes in a process
Energy Into System = Increases Entropy
Energy Out System = Decreases Entropy

46
Q

Equation for entropy

A 
deltaS = Q(subrev)/T
deltaS = change in entropy
Q(subrev) = heat that is gained or lost in a reversible process
T = temp in K
Units = J/mol*K

Physics (10 decks)

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