Formulas Flashcards

1
Q

differential form of the first law

A

dU = δQ + δW

all infinitesimal changes

U - internal energy (J)
Q - heat or thermal energy (J)
W - work (J)

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2
Q

second law

A

ΔS ≥ 0

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3
Q

reciprocal theorem

A

(∂x/∂y)(z) = [(∂y/∂x)(z)]^-1

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4
Q

reciprocity theorem

A

(∂x/∂y)(z) (∂y/∂z)(x) (∂z/∂x)(y) = -1

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5
Q

work during reversible processes

A

δW = -PdV

W = -(2 ∫ 1) PdV

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6
Q

heat capacity at constant volume

A

C(V) =lim(ΔT->0) (∂Q/∂T)(V) = (∂U/∂T)(V)

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7
Q

enthalpy

A

H = U + PV

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8
Q

enthalpy in differential form

A

dH = d(U+PV) = dU +PdV + VdP = ∂Q + VdP

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9
Q

heat capacity at constant pressure

A

C(P) =lim(ΔT->0) (∂Q/∂T)(P) = (∂H/∂T)(P)

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10
Q

efficiency of an engine

A

η = 1 - Q(2)/Q(1)

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11
Q

efficiency of a carnot engine

A

η(C) = 1 - T(2)/T(1)

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12
Q

triple point of water

A

T(K) = 273.16K Q/[Q(TP) H(2)O]

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13
Q

efficiency of a carnot refrigirator

A

η(C)^(R) = T(2)/T(1)-T(2)

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14
Q

efficiency of a carnot heat pump

A

η(C)^(HP) = Q(1)/Q(1)-Q(2) = T(1)/T(1)-T(2)

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15
Q

Clausius inequality

A

∮ δQ/T(0) ≤ 0

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16
Q

central equation of thermodynamics

A

dU = TdS - pdV

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17
Q

δQ

A

= TdS

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18
Q

δW

A

= -PdV

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19
Q

entropy change for heating a body

A

ΔS = cmln(Tf/Ti)

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20
Q

entropy change for adding heat to a reservoir at constant T

A

ΔS = Q/T

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21
Q

entropy change for phase changes

A

phase changes are isothermal processes

ΔS = mL/T

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22
Q

absolute entropy of an ideal gas

A

ΔS = n[c(V) ln(T2/T1) + Rln(V2/V1)]

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23
Q

molar specific entropy of an ideal gas

A

Δs = c(V) ln(T2/T1) + R ln(V2/V1)

24
Q

c(P) - C(V) =

25
isobaric coefficient of thermal cubic expansion
β(P) on the formula sheet
26
adiabatic coefficient of thermal cubic expansion
β(S) on the formula sheet
27
isothermal bulk compressibility
κ(T) on the formula sheet
28
adiabatic bulk compressibility
κ(S) on the formula sheet
29
isothermal bulk modulus
K(T) on the formula sheet
30
latent heat of expansion change
L(V) on the formula sheet
31
latent heat of pressure change
L(P) on the formula sheet
32
absolute entropy
s = s(0) + c(v) ln[T/T(0)] + R ln[V/v(0)]
33
enthalpy in a chemical reaction under constant pressure
Q = ΔH for ΔP = 0
34
entropy in a chemical reaction under constant pressure and enclosed in an adiabatic wall
ΔS + ΔS(0) ≥ 0 ΔG ≤ 0 for ΔP = ΔT = 0
35
entropy in a chemical reaction under constant volume and enclosed in an adiabatic wall
ΔS + ΔS(0) ≥ 0 ΔF ≤ 0
36
molar specific enthalpy of an ideal gas
h = u + pV(m) = u + RT
37
monoatomic
3/2 RT
38
diatomic
5/2 RT
39
enthalpy for a phase change at constant pressure
ΔH = ΔQ + VΔP = mL(p)
40
enthalpy for a incompressible fluid
ΔH = CΔT + VΔP or Δh = cΔT + ΔP/p where p is density
41
van der waals gas
see formula sheet a, accounts for attractive forces between molecules b, accounts for the finite particle volume
42
dieterici equation
Pexp(an/RTV)(V-nb) = nRT
43
joule-kelvin coefficient
µ on formula sheet
44
inversion temperature
= joule-kelvin coefficient where µ is the gradient of the curve
45
overall enthalpy is conserved in the liquification and hence
h(i) = αh(f,l) + (1-α)h(f,v) α = [h(i)-h(f,v)]/[h(f,l)-h(f,v)]
46
phase change equilibria
g(1) = g(2)
47
Clausius-Clapeyron equation for first-order phase changes
dP/dT = mL/[T(V(2) - V(1))] where P is the saturation vapour pressure L is the specific latent heat of vaporisation in J/kg V(1) and V(2) are the specific volumes of the vapour and liquid phases
48
partition function
Z = ( Σ i) exp[-ε(i)/k(b)T ] ε(i) is the microstates of energy
49
boltzmann's hypothesis
S = k(b) ln Ω Ω is the number of ways a system can be configured
50
three dimensional density of states
g(k)dk on formula sheet
51
maxwell-boltzmann distribution
f(k)dk on formula sheet
52
rayleigh-jeans law
u(BB) (λ) on formula sheet
53
the entropy for a single particle
S = k(b) [lnV + 3/2ln[mk(B)T/2πℏ^2 + 3/2]
54
probability or fraction of particles in a state
P(i) = 1/Z exp[-ε(i)/k(B)T]
55
Z = 1/N! [V (mk(B)T/2πℏ^2) ]^N
the partition function given derives from Z(gas) = 1/N! Z^N(particle) for Z^N(particle) the one-particle partition function N! derives from the indistinguishability of particles
56
entropy
dS = δQ/T where entropy is measured in JK^(-1)kg^(-1)