Lecture 20 - University of Michigan · 2019-08-07 · Web Lecture 20 Class Lecture 16-Thursday...
Transcript of Lecture 20 - University of Michigan · 2019-08-07 · Web Lecture 20 Class Lecture 16-Thursday...
Chemical Reaction Engineering (CRE) is the field that studies the rates and mechanisms of
chemical reactions and the design of the reactors in which they take place.
Lecture 20
Fi0∑ Ui0 + P0 !Vi0!" #$
Hi0" #$ %$− Fi∑ Ui + P !Vi#$ %&
Hi" #$ %$+ &Q − &WS =
dEsysdt
Fi0∑ Hi0 − Fi∑ Hi +!Q − !WS =
dEsysdt
Last Lecture Energy Balance Fundamentals
2
Substituting for !W
∑∑ =−+− 000 iiiiS HFHFWQ !!
dtdE
WQEFEF sysiiii =−+−∑∑ 00
!!
Web Lecture 20 Class Lecture 16-Thursday 3/14/2013
3
� Reactors with Heat Exchange � User friendly Energy Balance Derivations
� Adiabatic � Heat Exchange Constant Ta � Heat Exchange Variable Ta Co-current � Heat Exchange Variable Ta Counter Current
The feed consists of both - Inerts I and Species A with the ratio of inerts I to the species A being 2 to 1.
A B€
FA0
FI
Elementary liquid phase reaction carried out in a CSTR
4
Adiabatic Operation CSTR
Adiabatic Operation CSTR
5
� Assuming the reaction is irreversible for CSTR, A → B, (KC = 0) what reactor volume is necessary to achieve 80% conversion?
� If the exiting temperature to the reactor is 360K, what is the corresponding reactor volume?
� Make a Levenspiel Plot and then determine the PFR reactor volume for 60% conversion and 95% conversion. Compare with the CSTR volumes at these conversions.
� Now assume the reaction is reversible, make a plot of the equilibrium conversion as a function of temperature between 290K and 400K.
1) Mole Balances: exitA
0A
rXFV
−=
6
CSTR: Adiabatic Example
A B€
FA0
FI
Δ𝐻↓𝑅𝑥𝑛 =−20000𝑐𝑎𝑙/𝑚𝑜𝑙 𝐴 (exothermic)
𝑇= ?�𝑋= ?
𝐹↓𝐴0 =5𝑚𝑜𝑙/𝑚𝑖𝑛 𝑇↓0 =300 𝐾 𝐹↓𝐼 =10𝑚𝑜𝑙/𝑚𝑖𝑛
⎥⎦
⎤⎢⎣
⎡⎟⎟⎠
⎞⎜⎜⎝
⎛−
Δ=
=
⎥⎦
⎤⎢⎣
⎡−=−
⎟⎟⎠
⎞⎜⎜⎝
⎛−
T1
T1
RHexpKK
ekk
KCCkr
2
Rx1CC
T1
T1
RE
1
C
BAA
1
2) Rate Laws:
( )
XCC
X1CC
0AB
0AA
=
−=3) Stoichiometry:
7
CSTR: Adiabatic Example
4) Energy Balance Adiabatic, ∆Cp=0
( ) ( )
( )( )( )
X36164000,20300X
182164000,20300T
CCXHT
CXHTT
IAi PIP
Rx0
Pi
Rx0
++=⎥
⎦
⎤⎢⎣
⎡
+
−−+=
Θ+
Δ−+=
Θ∑
Δ−+=
X 100300T +=
8
CSTR: Adiabatic Example
Irreversible for Parts (a) through (c)
( ) )K (i.e., X1kCr C0AA ∞=−=−
(a) Given X = 0.8, find T and V
€
Given X Calc⎯ → ⎯ T Calc⎯ → ⎯ k Calc⎯ → ⎯ −rACalc⎯ → ⎯ V
€
Calc KC(if reversible)
9
CSTR: Adiabatic Example
( )
( )
( )( )( )( )( )
3
A
0A
0A
0A
exitA
0A
dm 82.28.01281.3
8.05rXFV
81.3380
12981
989.1000,10exp1.0k
K3808.0100300T
X1kCXF
rXFV
=−
=−
=
=⎥⎦
⎤⎢⎣
⎡ −=
=+=
−=
−=
Given X, Calculate T and V
10
CSTR: Adiabatic Example
(b) VrkTXGiven CalcA
CalcCalcCalc ⎯⎯→⎯−⎯⎯→⎯⎯⎯→⎯⎯⎯→⎯
CK Calc(if reversible)
( )
( )( )( )( )( )
3
1
0
05.24.0283.1
6.05min83.1
6.0100
300360
ble)(Irreversi 1
dmV
k
TX
KTXkCr AA
==
=
=−
=
=
−=−
−
Given T, Calculate X and V
11
CSTR: Adiabatic Example
(c) Levenspiel Plot
( )X1kCF
rF
0A
0A
A
0A
−=
−
€
Choose X Calc⎯ → ⎯ T Calc⎯ → ⎯ k Calc⎯ → ⎯ −rACalc⎯ → ⎯
FA0
−rA
X100300T +=
12
CSTR: Adiabatic Example
(c) Levenspiel Plot
13
CSTR: Adiabatic Example
0
5
10
15
20
25
30
0 0.1 0.2 0.3 0.4 0.5 0.6 0.7 0.8 0.9 1
X
-Fa0/Ra
CSTR 95%
CSTR X = 0.95 T = 395 K
0
5
10
15
20
25
30
0 0.1 0.2 0.3 0.4 0.5 0.6 0.7 0.8 0.9 1
X
-Fa0/Ra
CSTR 60%
CSTR X = 0.6 T = 360 K
14
CSTR: Adiabatic Example
PFR X = 0.6
PFR X = 0.95
0
5
10
15
20
25
30
0 0.1 0.2 0.3 0.4 0.5 0.6 0.7 0.8 0.9 1
X
-Fa0/Ra
PFR 60%
0
5
10
15
20
25
30
0 0.1 0.2 0.3 0.4 0.5 0.6 0.7 0.8 0.9 1
X
-Fa0/Ra
PFR 95%
15
CSTR: Adiabatic Example
CSTR X = 0.6 T = 360 V = 2.05 dm3
PFR X = 0.6 Texit = 360 V = 5.28 dm3
CSTR X = 0.95 T = 395 V = 7.59 dm3
PFR X = 0.95 Texit = 395 V = 6.62 dm3
16
CSTR: Adiabatic Example - Summary
( )
( )
⎥⎦
⎤⎢⎣
⎡+−=
−
=−+−
=Δ−+−
∑∑∑
∑
∑∑ Δ+
dVdF
HdVdH
FdV
HFd
TTUadV
HFd
VTTUaHFHF
ii
ii
ii
aii
aVViiVii
0
0
Energy Balance in terms of Enthalpy
17
( )RPiii TTCHH −+= 0
dVdTC
dVdH
Pii =
( )
xRii
AiiPiiii
HH
rHdVdTCF
dVHFd
Δ=
⎥⎦
⎤⎢⎣
⎡ −+−=−
∑
∑ ∑∑
υ
υ
PFR Heat Effects
18
( )Aiii rr
dVdF
−== υ
− CPiFi∑ dTdV
+ΔHRx −rA( )$
%&'
()+Ua Ta −T( ) = 0
Fi∑ CPidTdV
= ΔHRxrA −Ua T −Ta( )
dTdV
=ΔHRx( ) −rA( )−Ua T −Ta( )
Fi∑ CPi
19 Need to determine Ta
PFR Heat Effects
Heat Exchange:
( )( ) ( )iPi
aRxA
CFTTUaHr
dVdT
∑
−−Δ−−=
dTdV
=−rA( ) −ΔHRx( )−Ua T −Ta( )
FA0 ∑ΘiCPi
20 Need to determine Ta
Energy Balance:
Adiabatic (Ua=0) and ΔCP=0
( ) )A16( C
XHTTiPi
Rx0 Θ∑
Δ−+=
Heat Exchange Example: Case 1 - Adiabatic
21
A. Constant Ta e.g., Ta = 300K
( ))17( 0 , CTTV
CmTTUa
dVdT
aoaP
aa
cool
==−
=!
B. Variable Ta Co-Current
C. Variable Ta Counter Current ( ) Guess ? 0 ==
−= a
P
aa TVCm
TTUadVdT
cool!
Guess Ta at V = 0 to match Ta0 = Ta0 at exit, i.e., V = Vf
User Friendly Equations
22
Coolant Balance:
In - Out + Heat Added = 0
( )
( ) 0
0
=−+−
=−Δ+−Δ+
aC
C
aVVCCVCC
TTUadVdH
m
TTVUaHmHm
!
!!
Heat Exchanger Energy Balance Variable Ta Co-current
( )
dVdTC
dVdH
TTCHH
aPC
C
raPC0CC
=
−+=
23
( )0 0 , aa
PCC
aa TTVCmTTUa
dVdT
==−
=!
In - Out + Heat Added = 0
24
( )
( )
( )
0
0
PCC
aa
aC
C
aVCCVVCC
CmTTUa
dVdT
TTUadVdH
m
TTVUaHmHm
!
!
!!
−=
=−+
=−Δ+−Δ+
Heat Exchanger Energy Balance Variable Ta Counter-current
Elementary liquid phase reaction carried out in a PFR
The feed consists of both inerts I and species A with the ratio of inerts to the species A being 2 to 1.
25
FA0 FI
Ta cm!
Heat Exchange Fluid
€
A⇔ BT
Heat Exchanger – Example Case 1 – Constant Ta
⎥⎦
⎤⎢⎣
⎡⎟⎟⎠
⎞⎜⎜⎝
⎛−=
T1
T1
REexpkk )3(
11
⎥⎦
⎤⎢⎣
⎡⎟⎟⎠
⎞⎜⎜⎝
⎛−
Δ=
T1
T1
RHexpKK )4(
2
Rx2CC
FrdVdX )1( 0AA−=1) Mole Balance:
⎥⎦
⎤⎢⎣
⎡−−=
C
BAA K
CCkr )2(2) Rate Laws:
26
Heat Exchanger – Example Case 1 – Constant Ta
( )0CP =Δ
( ) ( )
( )6 XCC
5 X1CC
0AB
0AA
=
−=3) Stoichiometry:
( )9 CCC PIIPAPii θ+=θ∑
( )8 k1
kXC
Ceq +=
4) Heat Effects: ( )( ) ( ) ( )7 0∑
−−−Δ=
PiiA
aAR
CFTTUarH
dVdT
θ
Heat Exchanger – Example Case 1 – Constant Ta
27
Parameters:
A
IPIPAA
AaC
R
rrateCCC
FTUakkTTREH
−=
Δ
, , , ,, , , , ,
, , , , ,
0
021
21
θ
Heat Exchanger – Example Case 1 – Constant Ta
28
Pii
rg
CFQQ
dVdT
∑−
=
Heat removed
Heat generated
FiCPi =∑ FA0 θi +υiX( )CPi = FA0∑ θiCPi +ΔCPX∑#$ %&
dTdV
=ΔHR( ) rA( )−Ua T −Ta( )FA0 θiCPi +ΔCPX∑$% &
'
PFR Heat Effects
29
Energy Balance:
Adiabatic and ΔCP=0 Ua=0
( ) )A16( C
XHTTiPi
Rx0 Θ∑
Δ−+=
Additional Parameters (17A) & (17B)
IAi PIPPi0 CCC ,T Θ+=Θ∑30
Mole Balance:
€
dXdV
=−rAFA 0
Heat Exchanger – Example Case 2 – Adiabatic
31
Adiabatic PFR
Find conversion, Xeq and T as a function of reactor volume
V
rate
V
T
V
X X
Xeq
Example: Adiabatic
32
( )( ) ( )iPi
aRxA
CFTTUaHr
dVdT
∑
−−Δ−−=
( )( ) ( ) )B16( CF
TTUaHrdVdT
iPi0A
aRxA
Θ∑
−−Δ−−=
Heat Exchange
33 Need to determine Ta
A. Constant Ta (17B) Ta = 300K
Ua ,C ,TiPia Θ∑
Additional Parameters (18B – (20B):
( ) )17( 0 CTTVCmTTUa
dVdT
aoaP
aa
cool
==−
=!
B. Variable Ta Co-Current
C. Variable Ta Countercurrent
( ) ? 0 ==−
= aP
aa TVCm
TTUadVdT
cool!
Guess Ta at V = 0 to match Ta0 = Ta0 at exit, i.e., V = Vf
User Friendly Equations
34
Coolant balance:
In - Out + Heat Added = 0
( )
( ) 0
0
=−+−
=−Δ+−Δ+
aC
C
aVVCCVCC
TTUadVdHm
TTVUaHmHm
!
!!
( )
dVdTC
dVdH
TTCHH
aPC
C
raPC0CC
=
−+=All equations can be used from before except Ta parameter, use differential Ta instead, adding mC and CPC
Heat Exchange Energy Balance Variable Ta Counter-current
35
( )0 0 , aa
PCC
aa TTVCmTTUa
dVdT
==−
=!
In - Out + Heat Added = 0
All equations can be used from before except dTa/dV which must be changed to a negative. To arrive at the correct integration we must guess the Ta value at V=0, integrate and see if Ta0 matches; if not, re-guess the value for Ta at V=0
36
( )
( ) ( )PCC
aaa
CC
aVCCVVCC
CmTTUa
dVdTTTUa
dVdHm
TTVUaHmHm
!!
!!
−==−+
=−Δ+−Δ+
0
0
Heat Exchange Energy Balance Variable Ta Co-current
( ) 0HFHFdWTTUaii0i0ia
W
0 B
=−+−ρ ∑∑∫
( ) 0dWdHFH
dWdF0TTUa i
iii
aB
=−−+−ρ ∑∑
Differentiating with respect to W:
37
Derive the user-friendly Energy Balance for a PBR
⎟⎠⎞⎜
⎝⎛ ʹ′−υ=ʹ′= Aii
i rrdWdF
Mole Balance on species i:
( ) ∫+= οT
TPiRii
R
dTCTHH
Enthalpy for species i:
38
Derive the user-friendly Energy Balance for a PBR
Differentiating with respect to W:
dWdTC0
dWdH
Pii +=
( ) 0dWdTCFHrTTUa
PiiiiAaB
=−υʹ′+−ρ ∑∑
39
Derive the user-friendly Energy Balance for a PBR
( ) 0dWdTCFHrTTUa
PiiiiAaB
=−υʹ′+−ρ ∑∑
( )THH Rii Δ=υ∑( )XFF ii0Ai υ+Θ=
Final Form of the Differential Equations in Terms of Conversion:
A:
40
Derive the user-friendly Energy Balance for a PBR
Final form of terms of Molar Flow Rate:
( )
Pii
AaB
CF
HrTTUa
dWdT
Δʹ′+−ρ
=
B: ( )T,Xg
Fr
dWdX
0A
A =ʹ′−
=
41
Derive the user-friendly Energy Balance for a PBR
The rate law for this reaction will follow an elementary rate law.
DCBA +⇔+
⎟⎟⎠
⎞⎜⎜⎝
⎛−=−
C
DCBAA K
CCCCkr
Where Ke is the concentration equilibrium constant. We know from Le Chaltlier’s law that if the reaction is exothermic, Ke will decrease as the temperature is increased and the reaction will be shifted back to the left. If the reaction is endothermic and the temperature is increased, Ke will increase and the reaction will shift to the right.
42
Reversible Reactions
( )δ=RTKK P
C
Van’t Hoff Equation:
( ) ( ) ( )2
RPRR2
RP
RTTTCTH
RTTH
dTKlnd −Δ+Δ
=Δ
=ο
43
Reversible Reactions
For the special case of ΔCP=0
Integrating the Van’t Hoff Equation gives:
( ) ( ) ( )⎥⎦
⎤⎢⎣
⎡⎟⎟⎠
⎞⎜⎜⎝
⎛−
Δ=
ο
21
RR1P2P T
1T1
RTHexpTKTK
44
Reversible Reactions
endothermic reaction
exothermic reaction
KP
T
endothermic reaction
exothermic reaction
Xe
T
45
Reversible Reactions
46
End of Lecture 20