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thermodynamics Flashcards

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1
Q

thermodynamics

A

the study of the flow of energy in the universe

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2
Q

zeroth law of thermodynamics

A

based on a simple observation: when one object is in thermal equilibrium with another object, and the second object is in thermal equilibrium with a third object, then the first and third object are also in thermal equilibrium. no net flow of heat occurs

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3
Q

temperature

A

is a physical property of matter related to the average kinetic energy of the particles. Differences in temperature determine the direction of heat transfer

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4
Q

heat

A

the transfer of thermal energy from a hotter object with higher temperature (energy) to a colder object with lower temperature (energy). cannot spontaneously transfer energy from a cooler object to a warmer one without work being done on the system.

Unit is Joule (J)

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5
Q

Fahrenheit

A

absolute zero= -460 freezing point of water= 32 boiling point of water= 212

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6
Q

Celsius

A

absolute zero= -273 freezing point of water= 0 boiling point of water= 100

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7
Q

Kelvin

A

absolute zero= 0 freezing point of water= 273 boiling point of water= 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

Celsius to Fahrenheit

A

F= 9/5C+32

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10
Q

Celsius to Kelvin

A

K=C+273

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11
Q

thermal expansion

A

an increase in the length or volume of a substance as a result of an increase in temperature

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12
Q

thermal expansion equation

A

deltaL = alpha x L x deltaT

deltaL=change in length

alpha= coefficient of linear expansion

L= orignial length

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13
Q

volumetric thermal expansion

A

deltaV = beta x V x delta T

beta= coefficient of volumetric expansion

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14
Q

coefficient of linear and volumetric expansion

A

beta = 3alpha

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15
Q

system

A

the portion of the universe that we are interested in observing or manipulating

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16
Q

isolated systems

A

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

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17
Q

closed system

A

are capable of exchanging energy, but not matter, with its surroundings

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18
Q

open systems

A

can exchange both matter and energy with the surroundings

ex: boiling water, humans

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19
Q

state functions

A

thermodynamic properties that are a function of only the current equilibrium state, think vectors and scalars

include pressure, density, temp, volume, enthalpy, internal energy, gibbs free energy, and entropy

20
Q

process functions

A

describe the path taken to get to from one state to another, think vectors and scalars

include work and heat

21
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 from the system in the form of work

deltaU=Q-W

U=internal energy

Q=energy transferred into the system as heat

W= work done by the system

22
Q

delta U

A

negative sign= decrease in temp

postive sign= increase in temp

23
Q

Heat (Q) in the first law

A

positive value= heat flows into the system

negative value= heat flows out of the system

24
Q

Work (W) in the first law

A

positive value= work is done by the system (expansion)

negative value= work is done on the system (compression)

25
Q

what are the only two processes that energy can be transferred?

A

heat and work

26
Q

little calorie (c not C)

A

1 c = the amount of heat required to raise 1 g of water 1 degress Celsius.

27
Q

big calorie (C no c)

A

1 C = the amount of heat required to raise 1 kg of water 1 degree Celsius

equal to 1000 c

28
Q

conduction

A

the direct transfer of energy from molecule to molecule through molecular collisions; must be direct physical contact

29
Q

convection

A

the transfer of heat by the physical motion of a fluid over a material. only include gases and liquids

30
Q

radiation

A

the transfer of energy by electromagnetic waves, only form of heat transfer that can transfer energy through a vacuum

31
Q

specific heat (c)

A

defined as the amount of heat energy required to raise one gram of a substance by one degree Celsius or one unit Kelvin

changes according to its phase

32
Q

specific heat of water

A

1 cal/(g K)

33
Q

heat gained or lost (with temp change)

A

q=mcAT

AT=delta T

c=specific heat

m= mass

34
Q

Heat of transformation

A

during a phase change, heat energy causes energy changes in particles potential energy and energy distribution (entropy), but not kinetic energy. Therefore, phase changes have no change in temperature (kinetic energy), just in the thermal energy

35
Q

heat gained or lost (phase change)

A

q= mL

q= amount of heat gained or lost from the material

m= mass

L= heat of transformation or latent heat

36
Q

heat of fusion

A

melting point

phase change from liquid to solid (solidification) or solid to liquid (fusion)

37
Q

heat of vaporization

A

boiling point

phase change from liquid to gas (evaporation, vaporization) or gas to liquid (condensation)

38
Q

thermodynamic processes

A

isothermal, adiabatic, isovolumetric, and isobaric

in each case, some physical property is held constant during the process

39
Q

isothermal

A

constant temperature, so no chane in the internal energy

(delta U=0) Q=W

40
Q

adiabatic

A

no heat exchange

(Q=0) deltaU= -W

41
Q

isovolumetric (isochoric)

A

no change in volume, and therefore no work accomplished

(W=0) deltaU=Q

42
Q

Isobaric

A

processes at constant pressure

no special from ofthe first law

43
Q

Second Law of Thermodynamics

A

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

Energy spontaneously disperses form being localized to becoming spread out if it is not hindered from doing so.

44
Q

entropy (S; J/[molxK])

A

the 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

deltaS= Qrev/T

Qrev =the heat that is gained or lost in a reversable process

T= temp in kelvin

45
Q

changes in entropy with changes in energy

A

energy distributed into a system, entropy increases

energy distributed out of a system, entropy decreases

Physics and Math (12 decks)

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