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Jahrdenas_GEAS > Thermodynamics > Flashcards

Thermodynamics Flashcards

1
Q

Who coined the term “Thermodynamics”?

A

James Prescott Joule

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2
Q

Who is considered the Father of Thermodynamics?

A

Nicolas Sadi Carnot

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3
Q

Formula for Farenheit to Celcius

A

C = (5/9) (F - 32)

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4
Q

Formula for Celcius to Farenheit

A

F = (9/5)C + 32

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5
Q

A change in Celcius is ______ths of a change in Farenheit

A

5 / 9

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6
Q

Boiling point of Water IN FARENHEIT

A

212 F

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7
Q

The unit for temperature named after William Thomson

he is also known as ______________

A

Kelvin, Lord Kelvin :v

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8
Q

A change in Celcius is ________ a change in Kelvin

A

Equal to

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9
Q

Another absolute temperature scale other than Kelvin

A

Rankine

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10
Q

Formula for Rankine

A

R = F + 460

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11
Q

A change in Kelvin is ______ths of a change in Rankine

A

5 / 9

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12
Q

A change in Rankine is ________ a change in Farenheit

A

Equal to

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13
Q

Formula for Thermal Expansion

A

ΔL = α L ΔT

ΔL - change in length
α - Linear coefficient of thermal expansion
L - original Length
ΔT - Change in temperature

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14
Q

Linear coefficient of thermal expansion of Copper

A

18 x 10^-6 (in /C)

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15
Q

Formula for Areal Expansion

A

ΔA = γ A ΔT

ΔA - change in Area
γ - Areal coefficient of thermal expansion
A - original Area
ΔT - Change in temperature

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16
Q

Formula for Volumetric Expansion

A

ΔV) = β V ΔT

ΔV - change in Volume
β - Volumetric coefficient of thermal expansion
V - original Volume
ΔT - Change in temperature

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17
Q

Relation of Linear coefficient of thermal expansion(α) to Areal coefficient of thermal expansion(γ) and Volumetric coefficient of thermal expansion(β)

A 
β= 3α
γ = 2α
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18
Q

Defined as the Internal energy in transit from one body to another By virtue of a temperature difference between them

A

Heat

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19
Q

1 calorie is equivalent to how many joules?

A

4.186 J

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20
Q

1 BTU is equivalent to how many joules?

A

1054 J

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21
Q

1 BTU is equivalent to how many foot-pounds?

A

778 ft.lb

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22
Q

How much heat in calories is required to heat one gram of water by 1 Celcius?

A

1 Calorie

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23
Q

How much heat in BTU is required to heat one pound-mass of water by 1 Farenheit

A

1 BTU

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24
Q

A property of a material that defines how many calories or heat is required to raise a material’s Temperature by a specific amount, without considering the material’s mass

A

Heat Capacity

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25
Q

Formula of Heat that uses Heat Capacity as a variable

A

Q = C ΔT (unit in calories)

C-Heat capacity (in cal/Celcius)
Q-Heat in Calories

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26
Q

Defined as the Heat Capacity per unit mass

A

Specific Heat

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27
Q

The two variations of Specific Heat Capacity

A

Cp (Specific Heat @ Constant pressure)

Cv ( Specific Heat @ Constant Volume)

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28
Q

Formula for Molar Specific Heat

A

Cm = (MW)(c)

MW - Molar Weight
c - Specific Heat

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29
Q

Formula of heat, given mass and specific heat

A

Q = m (c) ΔT

Q - Sensible heat
m - mass of material
c - specific heat of material

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30
Q

Specific heat of water

A

1 cal/(g . C)

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31
Q

Specific Heat of Ice

A

0.5 cal/(g . C)

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32
Q

Specific Heat of Steam

A

0.45 cal/(g . C)

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33
Q

The Constant that relates Cp and Cv

A

Adiabatic Constant (γ)

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34
Q

Formula for Adiabatic Constant(γ)

A

γ = Cp / Cv

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35
Q

Adiabatic Constant for a monoatomic compound

A

γ = 1.67

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36
Q

Adiabatic Constant for a diatomic compound

A

γ= 1.4

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37
Q

Latent heat that involves change from solid to liquid and vice versa

A

Latent Heat of Fusion

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38
Q

Latent Heat of Fusion(L) in J/g

A

L = 333.5 J/g

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39
Q

Latent Heat of Fusion(L) in Cal/g

A

L = 80 Cal/g

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40
Q

Latent heat that involves change from Liquid to gas and vice versa

A

Latent Heat of Vaporization

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41
Q

Latent Heat of Vaporization(L) in J/g

A

L = 2256.7 J/g

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42
Q

Latent Heat of Vaporization(L) in cal/g

A

L = 540 cal/g

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43
Q

Latent heat that involves change from Gas to solid and vice versa

A

Latent Heat of Sublimation

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44
Q

Latent Heat of Sublimation(L) in J/g

A

L = 2838 J/g

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45
Q

Latent Heat of Sublimation(L) in cal/g

A

L = 670 cal/g

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46
Q

The heat required to perform phase(solid liquid gas) transformation

A

Heat of Transformation

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47
Q

Formula for Heat of Transformation(Q)

A

Q = m(L)

m - mass in grams
L - Latent Heat (Fusion, Sublimation, or Vaporization)

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48
Q

Formula for the rate of Heat transfer(Q/t)

AKA FOURIER’s LAW

A

(Q/t) = (k . A . ΔT) / L

k - Thermal Conductivity
A - Cross sectional area (m^2)
ΔT - difference in temperature between the two ends of the material wehre heat is transferred (in Kelvin)
L - Length of material (meters)

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49
Q

Formula for Thermal Resistance(R)

A

R = L / K

k - Thermal Conductivity
L - Length of material (meters)

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50
Q

Formula for the Temperature Gradient

A

Temp. Gradient = ΔT / L

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51
Q

The Property that measures the thermal insulating ability of a material

A

Thermal Resistance

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52
Q

Heat transfer that involves the flow of fluids or matter

A

Convection

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53
Q

Formula of Rate of Heat Transfer(Q/t) Due to Convection

A

Q/t = h . A . ΔT

h - convection Coefficient
A - Area in contact of convection
ΔT - Difference in temperature between two regions

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54
Q

Heat transfer that does not require a medium

A

Radiation

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55
Q

Stefan-Boltzmann Constant(sigma)

A

(sigma) = 5.68 x 10^-8 W / (m^2 . K^4)

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56
Q

Formula for Stefan-Boltzmann Law

AKA HEAT TRANSFER(Q/t) DUE TO RADIATION

A

Q/t = (sigma)(e)(A) . (T)^4

e = emissivity
A - Area of Coverage
(sigma) - Stefan-Boltzmann Constant

T - Temperature; if Temp. difference exists, replace T^4 with: (T2)^4 - (T1)^4

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57
Q

The ability to emit radiation

A

emissivity

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58
Q

emissivity(e) of the sun

A

1

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59
Q

emissivity(e) of a perfect reflector

A

0

60
Q

emissivity(e) of a black body

A

1 Manacup….. jk lang,

Answer: 1

61
Q

The formula that depicts the first law of thermodynamics

A

U = +-(Q) +-(W)

U - CHANGE in internal energy of system
Q - Heat absorbed/released by system
W - Work done on/by the system

62
Q

Who coined the term “Energy”

A

Thomas Young

63
Q

In Engineering convention, If heat is ABSORBED by the system, Q is (Positive/Negative)?

A

Positive

64
Q

In Engineering convention, If heat is RELEASED by the system, Q is (Positive/Negative)?

A

Negative

65
Q

In Engineering convention, If work is done ON the system, W is (Positive/Negative)?

A

Positive

66
Q

In Engineering convention, If work is done BY the system, W is (Positive/Negative)?

A

Negative

67
Q

The Interface that separates a system to its surroundings

A

Boundary

68
Q

A system where matter enters and leaves at the same rate

A

Steady Flow System

69
Q

A system where NOTHING crosses the boundary

A

Isolated System

70
Q

A system where heat does not cross the boundary

Therefore ΔQ = 0

A

Adiabatic System

71
Q

A system where heat MAY cross the boundary

A

Diathermic System

72
Q

A system where Matter may not cross the boundary, but heat may cross

A

Closed System

73
Q

Another term for Closed System

A

Control Mass System

74
Q

A system where EVERYTHING can cross the Boundary

A

Open System

75
Q

Another Term for Open System

A

Control Volume System

76
Q

The fastest reaction in a Thermodynamic system

A

Adiabatic

77
Q

In an adiabatic system, only ___________ contributes to a change in the internal energy of the system

A

work

78
Q

Value of Cv of a monoatomic substance

A

Cv = 3R / 2

R - 8.314 J/k.mol

79
Q

Value of Cp of a monoatomic substance

A

Cp = 5R/2

R - 8.314 J/k.mol

80
Q

Value of Cv of a diatomic substance

A

Cv = 5R/2

R - 8.314 J/k.mol

81
Q

Value of Cp of a diatomic substance

A

Cp = 7R/2

R - 8.314 J/k.mol

82
Q

Formula that depicts relationship of Cv to Cp

A

Cp = Cv + R

R - 8.314 J/k.mol

83
Q

Formula for Heat in an adiabatic process

A

Q = n(Cp OR Cv) . ΔT

n - number of moles
ΔT - Change in Temperature

84
Q

Formula for Work in an adiabatic process

A

W = (1 / (γ - 1))[P2V2 - P1V1]

γ - adiabatic constant

85
Q

Thermodynamic process where pressure is held constant

A

Isobaric

86
Q

Thermodynamic process where Volume is held constant

A

Isochoric

87
Q

Thermodynamic process where Temperature is held constant

A

Isothermal

88
Q

Formula for Work in an Isobaric Process

A

W = -P . ΔV

P - Pressure
V - Volume

89
Q

Formula for Heat in an Isobaric Process

A

Q = m Cp ΔT

m - mass
Cp - Specific heat when constant pressure
ΔT - Change in Temperature

90
Q

In an Isothermal process, the energy in a system __________?

A

Remains the same (Change in energy is zero)

91
Q

In an Isothermal process, What two properties of a system are the same in magnitude?

A

Heat and Work:

U = Q + W ; but in isothermal, U = 0
therefore, Q = -W

92
Q

Formula for Work in an Isothermal process (Using Initial and Final Volume)

A

W = -nRT ln (V2 / V1)

n - # moles
R -8.314 J/k.mol
T - Temp. in Kelvin

93
Q

Formula for Work in an Isothermal process (Using Initial and Final Pressure)

A

W = +nRT ln (P2 / P1)

n - # moles
R -8.314 J/k.mol
T - Temp. in Kelvin

94
Q

The work in an Isochoric Process is equal to

A

since ΔV = 0,
W = -P . ΔV
W = 0

95
Q

Change in internal energy is attributed only to ________ in an isochoric process

A

Answer: Heat

ΔU = Q + W
but W = 0
therefore, ΔU = Q

96
Q

Formula for Heat in an Isochoric Process

A

Q = m Cv ΔT

m - mass
Cv - Specific heat when constant volume
ΔT - Change in Temperature

97
Q

An adiabatic process in which there is no change in entropy (ΔS = 0)

A

Isentropic Process

98
Q

An adiabatic Process that Throttles

A

Isenthalpic Process

99
Q

The Change in Enthalphy in an Isenthalpic Process is ____________________

A

ΔH = 0

100
Q

With Throttling, there is a significant drop in _________

A

Pressure

P2 < P1

101
Q

When Gas is Throttled, the change in temperature over the change in pressure is called

A

Joule -Thomson Coefficient

102
Q

All Thermodynamic processes are (Reversible/Irreversible)

A

Irreversible

103
Q

Formula for Polytropic Process

A

P1 . (V1)^n = P2 . (V2)^n

n - Polytropic Exponent

104
Q

If the Polytropic Exponent(n) is ZERO, the effect is that the process becomes a/an ___________ process

A

Isobaric

105
Q

If the Polytropic Exponent(n) is ONE, the effect is that the process becomes a/an ___________ process

A

Isothermal

106
Q

If the Polytropic Exponent(n) is INFINITY, the effect is that the process becomes a/an ___________ process

A

Isochoric

107
Q

If the Polytropic Exponent(n) is the ADIABATIC CONSTANT, the effect is that the process becomes a/an ___________ process

A

Adiabatic

108
Q

If the Polytropic Exponent(n) is K, the effect is that the process becomes a/an ___________ process

A

Isentropic

Note: idk what K is :v, maybe boltzmann

109
Q

Formula for Polytropic Specific Heat

A

Cn = Cv . ( n - K ) / ( n - 1 )

n - polytropic exponent

Note: idk what K is :v, maybe boltzmann

110
Q

2nd Law of Entropy

A

Entropy Increases as time approaches Infinity.

Entropy never increases

111
Q

3rd Law of Entropy

A

Entropy is 0 at T = 0 Kelvin

112
Q

0th Law of Entropy

A

if Ta = Tb, and Ta = Tc,

therefore, Tb = Tc

113
Q

What is the Input and Output of a Heat Engine?

A

Input: Qhot
Output: Work(out)

114
Q

Formula for Output Work in a Heat Engine

A

Wout = Qh - Qc

115
Q

Formula for Heat Engine Efficiency(e)

A

Derivation:
e = Output / Input
e = Wout / Qh
e = (Qh - Qc) / Qh

Final Ans: e = 1 - (Qc / Qh)

116
Q

Formula for Heat Engine CARNOT EFFICIENCY

A

e = 1 - (Tc / Th)

IN KELVIN

117
Q

Formula for Refrigerator CARNOT Coefficient of Performance

A

COP = (Th - Tc) / Tc

IN KELVIN

118
Q

What is the Input and Output of a Refrigerator?

A

Input: Work(in)
Output: Qcold

119
Q

Formula for Output Qc in a Refrigerator

A

Qc = Qh - Win

120
Q

Formula for the Coefficient of Performance of a Refrigerator

A

Derivation:
COP = Output / Input
COP = Qc / Win

Final Ans: COP = Qc / (Qh - Qc)

121
Q

What is the Input and Output of a Heat Pump?

A

Input: Work(in)
Output: Qhot

122
Q

Formula for Input Work in a Heat Pump

A

Win = Qh - Qc

123
Q

Formula for Coefficient of Performance of a Heat Pump

A

Derivation:
COP = Output / Input
COP = Qh / Win

Final Ans: COP = Qh / (Qh - Qc)

124
Q

Another parameter that measures refrigerator performance

A

Energy Efficiency Ratio (EER)

125
Q

Formulas for Energy Efficiency Ratio(EER)

A 
EER = (Q per Hour)/Power
EER = 3.42 . COP

Q - MUST BE IN BTU/hour

126
Q

Kevin-Planck Statement

A

Assume a Heat Engine:
Because Qc can never become 0,
from the formula Wout = Qh - Qc,

Conclusion: Wout can never be equal to Qh

127
Q

Clausius Statement

A

Assume a Refrigerator/Air conditioner:
Because the input work(Win) required to cool a system cannot be just 0,
from the formula Qc = Qh - Win,

Conclusion: Qc cannot equal Qh

Restatement: “Heat does not flow from cold to hot normally”

128
Q

Caratheodory Statement

A

At equilibrium, There are equilibrium states inaccessible by an adiabatic process

129
Q

Nernst Postulate

A

from the 3rd Law if Thermodynamics (Tk = 0 Kelvin, The entropy is zero), “It is impossible to achieve this state with finite number of operations”

130
Q

The amount of Disorder in a system

A

entropy

131
Q

The formula for the Change in Entropy

A

ΔS = Q / T

Q - Heat
T -Temperature

132
Q

When Solid transfoms Into Liquid and/or Liquid into Gas(S»»L»»G), Change in Entropy (Increases/Decreases)

A

Increases

133
Q

When Gas transfoms Into Liquid and/or Liquid into Solid(G»»L»»S), Change in Entropy (Increases/Decreases)

A

Decreases

134
Q

What are the processes involved in a Carnot Cycle

A

Involves 2 Adiabatic and 2 Isothermal Processes to complete one cycle (4 processes in total)

135
Q

The Phase transformation from Gas to Solid

A

Deposition

136
Q

The Triple Point of Water is Found at what temperature?

A

0.01 Celcius

137
Q

Water is most dense at what temperature?

A

4 Celcius

138
Q

How much of a Proton’s Energy is attributed to Heat?

A

1/3 of Proton’s energy is equal to heat

139
Q

Unit of electron volts (eV)

A

Joules per Coloumb (J/C)

140
Q

If in problems a gas is not specified if whether monoatomic or diatomic, what do we assume by default?

A

the gas is monoatomic

141
Q

Kinetic Energy of MONOATOMIC gas

A

KE = 3.K.T / 2

k - boltzmann constant
T - Temp. in Kelvin

142
Q

Kinetic Energy of DIATOMIC gas

A

KE = 5.K.T / 2

k - boltzmann constant
T - Temp. in Kelvin

143
Q

Vrms of MONOATOMIC gas (given Temperature and mass)

A

Vrms = sqrt( (3KT / m)

k - boltzmann constant
T - Temp. in Kelvin
m - mass in kg

144
Q

Vrms of DIATOMIC gas (given Temperature and mass)

A

Vrms = sqrt( (5KT / m)

k - boltzmann constant
T - Temp. in Kelvin
m - mass in kg

145
Q

Vrms of MONOATOMIC gas (given Temperature and Molar mass)

A

Vrms = sqrt( (3RT / MM)

R - 8.314 J/K.mol
T - Temp. in Kelvin
MM - Molar Mass

146
Q

Vrms of DIATOMIC gas (given Temperature and Molar mass)

A

Vrms = sqrt( (5RT / MM)

R - 8.314 J/K.mol
T - Temp. in Kelvin
MM - Molar Mass

Jahrdenas_GEAS (9 decks)

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