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Introductory ChemicalEngineering Thermodynamics Chapter 7 - Departure Functions
By J.R. Elliott, Jr.
Chapter 7 - Departure Functions Slide 2
Internal Energy Departure Function
U(T,V)-Uig(T,V) = dV
V
U
V
Uig
TT
V
−
∫
∞ ∂∂
∂∂
FPR tells us (dU)T = T(dS)T - P(dV)TFor the ideal gas (dUig)T = T(dSig)T -P(dVig)Twhere (dSig)T = RdlnV and P(dV
ig)T = RT/V dV = RT dlnV
Substituting we find, (dUig
)T = T*R dlnV - RT dlnV = 0
Therefore,
ig
TV
U
∂∂
=0
Returning to the FPR, TTT V
VP
V
ST
V
U
−
=
∂∂
∂∂
∂∂
Maxwell’s Relation VT T
P
V
S
=
∂∂
∂∂
Finally, ∫∞
−
=−
V
V
ig dVPT
PTUU
∂∂
)(
If we transform to density, the expressions we get are usually easier to integrate.
Chapter 7 - Departure Functions Slide 3
∴ = − ⇒ =−
→ ∞ →dV dV
and12ρ
ρ ∂ ∂ρρ
ρ V
at V , 0,
∫
−=
⇒
ρ
ρ ρρ
∂∂
ρρ0
1- d
T
P
RRT
P
RT
UU ig
−=
−=
−∴ ∫ RT
PTUPTUd
T
ZT
RT
VTUVTU igig ),(),(),(),(
0
ρ
ρ ρρ
∂∂
Because Uig(T,P) - Uig(T,V) = ∫ (∂Uig/∂V)T dV = 0Example. Derive the internal energy departure function for the EOS:Z=1+4bρ/(1-bρ)-aρ/RT(∂Z/∂T)ρ = + aρ/RT2 ⇒ -T(∂Z/∂T)ρ = -aρ/RT
[ ]RT
a
RT
ad
RT
ad
T
ZT
RT
VTUVTU ig ρρρρρ
ρρ
∂∂ ρρ
ρ
ρ
−=−=−=
−=
−∴ ∫∫ 000
),(),(
Chapter 7 - Departure Functions Slide 4
Helmholtz Energy:Departure Function
dVV
A
V
AVTAVTA
V ig
TT
ig ∫∞
−
=−
∂∂
∂∂
),(),(
( )V
RT
V
nVRT
V
AnVRTddV
V
RTdAPdVdAFPR
T
ig
T
igTT
−=
−=
⇒−=−=⇒−=⇒
∂∂
∂∂ l
l)(
Also P
V
A
T
−=
∂∂
⇒ V
RTP
V
A
V
Aig
TT
+−=
−
∂∂
∂∂
Transform to ρ⇒dV = -V dρ/ρ
∫
−=
−⇒ρ
ρρ0
1),(),(d
Z
RT
VTAVTA ig
Chapter 7 - Departure Functions Slide 5
Gibbs energy departure functionAs for the density dependent part, it is easy to see that,G = U + PV -TS = A + PV
∫ −+
−=−+−=−⇒ρ
ρρo
igid
ZdZ
ZRT
VTAVTA
RT
VTGVTG1
11
),(),(),(),(
Since V and P correspond to the properties of the real gas, the pressure of the ideal gas atT and V is P1 =RT/V. The change in Gibbs energy isG T p G T V RT n P P RT n PV RT RT n Zig ig( , ) ( , ) )− = = ( / ( / ) = ( )l l l1
⇒ = − − −G T P G T P
RT
G T P V G T V
RT
G T P G T V
RT
ig ig ig ig( , ) - ( , ) ( , , ) ( , ) ( , ) ( , )=
G T P V G T V
RTZ
ig( , , ) ( , )ln( )
−−
)ln(11),(),(
ZZdZ
RT
PTGPTG
o
ig
−−+
−=−
⇒ ∫ρ
ρρ
Chapter 7 - Departure Functions Slide 6
Summary of density dependent formulas fordeparture functions from equations of state.
( )∫ −+
−=− ρ
ρρ
∂∂
o
ig
Zd
T
ZT
RT
HH1
( ) ( )( ) ( )∫ −−+−=− ρ
ρρo
ig
nZZdZ
RT
PTGPTGl1
1,,
( )ρρ
∂∂ρ
d
T
ZT
RT
UU
o
ig
∫
−− ( ) ( )( ) ( )
∫−=− ρ
ρρo
ig
dZ
RT
VTAVTA 1,,
( ) ( )( ) ( )∫
−−
−=− ρ
ρρ
∂∂
o p
ig dZ
T
ZT
R
VTSVTS1
,, ( ) ( )( ) ( )∫ +
−−
−=− ρ
ρρ
∂∂
o p
ig
nZd
ZT
ZT
R
PTSPTSl1
,,
Chapter 7 - Departure Functions Slide 7
Example 7.1. Use of PREOS to get enthalpy and entropy departures.Propane gas undergoes a change of state from an initial condition of 5 bar and 105°C to25 bar and 190°C. Compute the change in enthalpy and entropy.For propane : A=-4.224; B=0.3063; C= -1.586E-4; D=3.215E-8Tc = 369.8 K; Pc = 42.49 bar.; ω=0.152
Solution:Path, for H(190,25) - H(105,5)[H(190,25) - Hig(190,25)]+[Hig(190,25) - Hig(105,5)]+[Hig(105,5) - H(105,5)]Similarly for S(190,25) - S(105,5)[S(190,25 - Sig(190,25)]+[Sig(190,25) - Sig(105,5)]+[Sig(105,5) - S(105.5)]I. Departure Function + II. Ideal gas + III. Departure function
I. (190,25) → (190,25)ig 190 + 273.15 = 463.15K & 25 bar ⇒ Tr = 1.25135; Pr = 0.58837
PREOS ⇒ Z=0.8891 ⇒ (H-Hig) = (-0.3869) 8.314*463.15 = -1490 J/mol (S-Sig ) = (-0.2757) 8.314 = -2.2918 J/mol-K
Chapter 7 - Departure Functions Slide 8
II. (190,25)ig →(105,5)igHig(190,25) - Hig(105,5) = ∫Cp dT = -4.224(463-378) + 0.3063(4632-3782)/2+ (-1.586E-4) (4633-3783)/3 +(3.215E-8)(4634-3784)/4 = 8405 J/moleSig(190,25) - Sig (105,5) = A ln(T2/T1)+B(∆T) +C∆(T2)/2+D∆(T3)/3 - Rln(P2/P1) ;∆Sig = -4.224 ln(463.15/378.15) + 0.3063(85) + (-1.586E-4)(4632-3782)/2 + + 3.215E-8(4633-3783)/3 - 8.314 ln 5 = 6.613 J/mol-K III. (105,5)→(105,5)ig 105 + 273 = 378.15 & 5 bar → Tr = 1.02258; Pr = 0.11767 Z = 0.9574 ⇒ (H-Hig ) = (-0.1274) 8.314*378.15 = -400 J/mol (S-Sig ) = (-0.0852) 8.314 = -0.7081 J/mol-K∆Htot = -1490 + 8405 + 400 = 7315 J/mol(Note: Chart ⇒ (1265 - 1095)*44 = 7480 J/mol)∆Stot = -2.292 + 6.613 + 0.708 = 5.029 J/mol-K(Note: Chart ⇒ (1.52-1.50)*44*4.184=3.7 J/mol-K)Moral: The difference between the chart and the Peng-Robinson equation is significant,but could be because of error in the Peng-Robinson equation or sensitivity to theaccuracy with which the chart can be read. Entropy is especially difficult because thetemperature and pressure effects tend to cancel and we end up with the small differencebetween large numbers. In reality, the Peng-Robinson equation is only accurate to about10% on enthalpy if compared to a highly accurate equation.
Chapter 7 - Departure Functions Slide 9
Example 7.6. Use of Referenced PREOS to get enthalpy and entropyPropane gas undergoes a change of state from an initial condition of 5 bar and 105°C to25 bar and 190°C. Compute the change in enthalpy and entropy by using a commonreference state of 230K and 0.1MPa.For propane : A = -4.224; B = 0.3063; C = -1.586E-4; D = 3.215E-8Tc = 369.8 K; Pc = 42.49 bar.; ω=0.152
Solution: In this example, we are directed to use a reference state such that, for enthalpy:H2 - H1 = (H2 - Href) - (H1 - Href), and for entropy: S2 - S1 = (S2 - Sref) - (S1 - Sref). Note theequivalence of this procedure to the way steam tables are computed. Furthermore, thecomputation of H2 - Href or S2 - Sref is entirely equivalent to the procedure given inExample 7.1.1. REF: Enter the values of Tc , Pc , ω, A, B, C, D and define the T, P, and root of
interest.2. Press PVTF to enter the pressure and temperature and choose the root of interest.
E.g. at 463.15 K and 2.5 MPa, V = 1369 cm3/mole3. Press UHSG to compute internal energy, enthalpy, entropy, and Gibbs free energy.
E.g. at 463.15 K and 2.5 MPa, H2 - Href = 36901 J/mole; S2 - Sref = 109.15 J/mole-K4. Repeat at 378.15 K and 0.5 MPa, H1 - Href = 29586 J/mole; S1 - Sref = 104.13 J/mole-K5. Subtract ⇒ ∆H = 36901-26756 = 7315 and ∆S = 109.15-104.13 = 5.02 J/mole-K
Chapter 7 - Departure Functions Slide 10
Example 7.3 Enthalpy departure for PREOSObtain a general expression for the enthalpy departure function of the PREOS.Solution: In the previous example we were able to obtain both pressure-explicit anddensity-explicit equations. Therefore, we could solve the problem two different ways.For the PREOS, we can only solve one way.
( ) ( )2221
/
1
1
ρρρ
ρ bb
RTa
bZ
−+−
−=
( )
+−
−+=
−
dT
da
TT
a
bb
RT
T
ZT
1
21
/222 ρρ
ρ∂∂
ρ
( )[ ]Pc
TcRaTcTaa cc
222
45724.0;/11 ≡−+= κ
where κ ω ω= 0.37464 +1.54226 - 0.26993 2
−
−+= − 2/1
2
1112 T
TcTc
Ta
dT
dac
κκ ⇒ ( )[ ]( )TcTTcTadT
daT c //11 κκ −+−=
( )[ ]( )
−+−−−
−+=
− TcTTcT
bRT
a
bRT
a
bb
b
T
ZT c //11
21 22κκ
ρρρ
∂∂
ρ ( ) ( )rTFbb
b2221 ρρ
ρ−+
≡
F(Tr) is shorthand. Also B ≡ bP/RT ⇒ bρ = B/Z and A ≡ aP/R2T2 ⇒ a/bRT = A/B
Chapter 7 - Departure Functions Slide 11
( )( ) ( ) ( )
∫ ∫ =−+
=
−
ρ ρ
ρρ
ρρρ
ρρ
∂∂b
o
b
o
rT b
bdTF
bb
b
b
bd
T
ZT
2221
( ) ( )( )
−+++=
+−++
+−
ρρ
ρρ
ρ
b
bn
TrF
b
bn
TrFb
211
211
8
)(
1)21(
1)21(
21
21
80
ll
Note ( ) ( ) ( )
( )
−+++=
−⇒== ∫ BZ
BZn
TrF
b
bd
T
ZTb
RT
pRT
bp
Z
Bb
T 21
21
80
ρ
ρρ
∂∂ρ
ρ
l
( ) ( )( ) ( )[ ]
−+−−
−++++−=−
rrc
ig
TTbRT
a
bRT
a
BZ
BZnZ
nRT
HH κκ 1121
21
8
11 l
= ( )( )
+
ακ Tr
B
A
B
B1
82-1+Z
2+1+Zn-1-Z l
Chapter 7 - Departure Functions Slide 12
Example 7.4 Gibbs Departure for PREOS.Obtain a general expression for the Gibbs energy departure function of the PR-EOS.
( ) ( )2221
/
1
1
ρρρ
ρ bb
RTa
bZ
−+−
−=
( ) ( ) ( )2222 21
/
121
/
1
1
1
11
ρρρ
ρρ
ρρρ
ρρ
ρ bb
RTa
b
b
bb
RTa
b
b
bZ
−+−
−=
−+−
−−−
−=−
( ) ( )( ) ( )∫ −−+−=− ρ
ρρo
id
nZZdZ
nRT
pTGpTGl1
1,,
=ln(1-bρ) – lnZ + Z – 1 + ( )( )
ρρ
b
b
bRT
a
2-1+1
2+1+1n
8l
=ln(Z-B)-( )( ) 82-1+Z
2+1+Zn
B
A
B
B
l
Chapter 7 - Departure Functions Slide 13
Example 7.7 Liquefaction revisitedReevaluate the liquefaction of methane consideredpreviously using the methane chart by performingthe analogous calculations with the PR EOS.Natural gas, assumed here to be pure methane, isliquefied in a simple Linde process. Compression isto 60 bar and precooling is to 300K. The separator ismaintained at a pressure of 1 bar and unliquefied gasat this pressure leaves the cooler at 295 K. Whatfraction of the gas is liquefied in the process?
Precool
Heat Exch
ThrottleFlashDrum
Compressor
1
23
4
5
6
7
8
Tc =190.6; Pc =4.60MPa; ω=.008; Cp ≈ Cp (200K) ≈ 28.45 J/mol-KSolution: To facilitate comparison to chart, set the reference enthalpies equal.Let: Href=H
satL(1bar) = 4538J/mol (283.6 J/g as given on chart, T
sat(1bar)=111.0K).
( ) ( ) ( ) refsatLidididid HHHHHHHH +−+−+−= 1
1111
1111
30060
30060
30060
30060
= -0.4334(8.314)300+28.45(300-111)+8.9453(8.314)111 + 4538 = 17089 J/mole( ) ( ) ( ) ref
satLidididid HHHHHHHHH +−+−+−== 11111
1111
2951
2951
2951
29518
= 0 + 28.45(295-111) + 8255 + 4538 = 18028J/moleH6 ≡ 4538 E-Bal ⇒ H3 = qH8 + (1-q)H6 ⇒ q=0.9304 ⇒ 6.96% liquefiedThis compares to 7.13% when we read the chart to the best of our ability.