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Thermodynamics Flashcards

(58 cards)

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1
Q

thermal equilibrium

A

when no heat flows between objects

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2
Q

What changes as a function of temperature

A

length, volume, solubility and conductivity

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3
Q

Length expansion equation

A

ΔL=αLΔT

α = coefficient of linear expansion

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4
Q

Volumetric expansion equation

A

ΔV=βVΔT

β = 3α

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5
Q

isolated systems

A

not capable of exchanging energy or matter with their surroundings

total change in internal energy must be zero

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6
Q

closed systems

A

capable of exchanging energy but not matter with surroundings

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7
Q

Open systems

A

can exchange both matter and energy with the environment

matter can carry energy and can be transferred in the form of heat or work

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8
Q

state functions

A

path independent to get to particular equilibrium state

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

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9
Q

process functions

A

depend on the path taken to get from one state to another

work and heat

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10
Q

first law of thermodynamics

A

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

ΔU = Q-W

energy cannot be created or destroyed, only exchanged

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11
Q

positive Q

A

heat flows into the system

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12
Q

negative Q

A

heat flows out of the system

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13
Q

positive W

A

work is done by the system (expansion)

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14
Q

negative W

A

work is done on the system (compression)

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15
Q

negative ΔU

A

decreasing temperature

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16
Q

positive ΔU

A

increasing temperature

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17
Q

second law of thermodynamics

A

objects in thermal contact and not in thermal equilibrium will exchange heat energy such that hotter object gives heat to colder object

increase entropy

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18
Q

Heat

A

process by which a quantity of energy is transferred between two objects as a result of a difference in temperature

heat cannot be spontaneously transfer energy from a cooler to a warmer object without work being done on the system

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19
Q

Calorie to Joules

A

1 Cal = 10^3 cal = 4184 J

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20
Q

Conduction

A

transfer of energy between objects through molecular collisions

must have direct physical contact between objects

hotter object transfers some kinetic energy to particles of cooler matter through collisions between the particles of the two materials

ex: touching a hot stove

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21
Q

What are the best heat conductors?

A

metals because metallic bonds contain density of atoms embedded in sea of electrons which facilitates rapid energy transfer

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22
Q

What are the poorest heat conductors?

A

gases because there is so much space between individual molecules which makes energy-transferring collisions occurring infrequently

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23
Q

convection

A

transfer of heat through physical motion of the fluid over the material

only liquids and gases can use this

ex: convection ovens circle hot air inside the oven which causes rapid cooking
ex: using an ice bath to rapidly cool something

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24
Q

Radiation

Study These Flashcards
A

transfer of energy by electromagnetic waves (through a vacuum)

ex: way sun is able to warm the earth

25
specific heat
amount of heat energy required to raise one gram of a substance by one degree C/K changes depending on phase q=mcΔT
26
specific heat of water
1 cal/g*K
27
What happens when you add heat to ice?
the heat energy causes water molecules to move away from one another because breaking hydrogen bonds now the water molecules are held less rigidly in place and have greater degrees of freedom of movement, average PE increases
28
equation for phase change
q = mL ``` q = amount of heat gained or lost m= mass of substance L= heat of transformation ```
29
heat of fusion
heat of transformation between solid and liquid (either direction)
30
heat of vaporization
heat of transformation between liquid and gas
31
melting
solid to liquid
32
freezing
liquid to solid
33
condensation
gas to liquid
34
evaporation/vaporization
liquid to gas
35
sublimation
solid to gas
36
deposition
gas to solid
37
isobaric
pressure held constant
38
isothermic
constant temperature ΔU=0 W=Q
39
isochoric
isovolumetric constant volume W=0 ΔU=Q
40
adiabatic
no heat exchange Q=0 ΔU= -W
41
entropy
measure of spontaneous dispersal of energy at a specific temperature ΔS = Q/T entropy increases when energy is distributed into a system at a given temperature
42
the entropy of a system can decrease when?
the entropy of surroundings increases by at least as much because the entropy of the universe must remain constant or increase during all processes
43
1 mole = how many liters at STP
22.4L
44
gas constants
0. 0821 atm L/mol K | 8. 314 J/mol K
45
Gay Lussac's Law
Pressure is directly proportional to Temperature P1/T1 = P2/T2
46
Charles' Law
Temperature is directly proportional to volume V1/T1 = V2/T2
47
Avogadro's Law
volume is proportional to number of moles V1/n1 = V2/n2
48
Boyles' Law
Pressure is inversely proportional to volume P1V1 = P2V2
49
Van der Waals equation
(P + a(n/v)^2)(V-nb) = nRT
50
Boltzman's Constant
PV = NkbT kb=n/NR kb=1/Na(R) N= nNa (number of moles x avogadro's number) kb=1.38x10^-23 J/K allows us to find ideal gas law focusing on number of molecules
51
internal energy
Uint = 3/2PV = 3/2NKbT = 3/2nRT equal to internal energy
52
changing internal energy
ΔU = Q + W if you are doing work on gas = +W if the gas is doing work = -W W = PΔV
53
What is the work done when pressure is constant
W = PΔV
54
heat capacity
if a certain amount of heat is added, how much will the gas expand C= Q/ΔT
55
molar heat capacity
C = Q/nΔT when at constant volume C = 3/2R when at constant pressure C=5/2R
56
heat capacity (volume)
keeping the volume the same will increase pressure as we add more heat C = Q/ΔT no work can be done because no expansion; will heat up Cv = ΔU/ΔT = 3/2PV/ΔT = 3/2Nkb = 3/2nR Cv=3/2nR
57
heat capacity (pressure)
work can be done on the gas Cp = Q/ΔT = ΔU-W/ΔT = ΔU-PΔV/ΔT = 3/2nRΔT + PΔV/ΔT = 3/2nRΔT + nRΔT/ΔT = 3/2nR + nR = 5/2 nR Cp = 5/2nR
58
force equation
F = ΔP/ΔT = mΔv/ΔT

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