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L4-1
Slides courtesy of Prof M L Kraft, Chemical & Biomolecular Engr Dept, University of Illinois at Urbana-Champaign.
Ideal CSTR Design Eq
with XA:
Review: Design Eq & ConversionD
ad
C ac
B ab A
fed A moles reacted A moles
XA
BATCHSYSTEM: A0Aj0jj XNNN
jA0A
jj0TjT XNNNN
FLOW SYSTEM: A0Aj0jj XFFF
jA0A
jj0TjT XFFFF
r
XFV
A
A0A
Vr dt
dXN A
A0A Ideal Batch Reactor
Design Eq with XA:
AX
0 A
A0A Vr
dXNt
AA
0A rdV
dXF Ideal SS PFR
Design Eq with XA:
AX
0 A
A0A r
dXFV
'rdW
dXF A
A0A Ideal SS PBR
Design Eq with XA:
AX
0 A
A0A 'r
dXFW
j≡ stoichiometric coefficient; positive for products, negative
for reactants
L4-2
Slides courtesy of Prof M L Kraft, Chemical & Biomolecular Engr Dept, University of Illinois at Urbana-Champaign.
Review: Sizing CSTRsWe can determine the volume of the CSTR required to achieve a specific conversion if we know how the reaction rate rj depends on the conversion Xj
AA
0ACSTR
A
A0ACSTR X
rF
V rXF
V
Ideal SS CSTR
design eq.
Volume is product of FA0/-rA and XA
• Plot FA0/-rA vs XA (Levenspiel plot)
• VCSTR is the rectangle with a base of XA,exit and a height of FA0/-rA at XA,exit
FA 0 rA
X
Area = Volume of CSTR
X1
V FA 0 rA
X1
X1
L4-3
Slides courtesy of Prof M L Kraft, Chemical & Biomolecular Engr Dept, University of Illinois at Urbana-Champaign.
FA 0 rA
Area = Volume of PFR
V 0
X1FA 0 rA
dX
X1
Area = VPFR or Wcatalyst, PBR
dX'r
FW
1X
0 A
0A
Review: Sizing PFRs & PBRsWe can determine the volume (catalyst weight) of a PFR (PBR) required to achieve a specific Xj if we know how the reaction rate rj depends on Xj
A
exit,AX
0 A
0APFR
exit,AX
0 A
A0APFR dX
r
FV
r
dXFV
Ideal PFR design eq.
• Plot FA0/-rA vs XA (Experimentally determined numerical values) • VPFR (WPBR) is the area under the curve FA0/-rA vs XA,exit
A
exit,AX
0 A
0APBR
exit,AX
0 A
A0APBR dX
r
FW
r
dXFW
Ideal PBR
design eq.
dXr
FV
1X
0 A
0A
L4-4
Slides courtesy of Prof M L Kraft, Chemical & Biomolecular Engr Dept, University of Illinois at Urbana-Champaign.
Numerical Evaluation of Integrals (A.4)Simpson’s one-third rule (3-point):
2102X
0XfXf4Xf
3h
dxxf
hXX 2
XXh 01
02
Trapezoidal rule (2-point):
101X
0XfXf
2h
dxxf
01 XXh
Simpson’s three-eights rule (4-point):
32103X
0XfXf3Xf3Xfh
83
dxxf 3
XXh 03
h2XX hXX 0201
Simpson’s five-point quadrature :
432104X
0XfXf4Xf2Xf4Xf
3h
dxxf 4
XXh 04
L4-5
Slides courtesy of Prof M L Kraft, Chemical & Biomolecular Engr Dept, University of Illinois at Urbana-Champaign.
Review: Reactors in Series
2 CSTRs 2 PFRs
CSTR→PFR
VCSTR1 VPFR2
VPFR2VCSTR1
VCSTR2
VPFR1
VPFR1
VCSTR2
VCSTR1 + VPFR2
≠
VPFR1 + CCSTR2
PFR→CSTR
A
A0
r-
F
i j
CSTRPFRPFR VVV
If is monotonically
increasing then:
CSTRi j
CSTRPFR VVV
L4-6
Slides courtesy of Prof M L Kraft, Chemical & Biomolecular Engr Dept, University of Illinois at Urbana-Champaign.
L4: Rate Laws & Stoichiometry
• Reaction Rates (–rA )
1. Concentration2. Temperature 3. Reversible reactions
• How to derive an equation for –rA [–rA = f(XA)]
1. Relate all rj to Cj
2. Relate all Cj to V or u3. Relate V or u to XA
4. Put together
A
A
XA
A00
dX
rt N
V
A
A
A0F XV
r
AXA
A00 Ar
dXV F
A
A
XA
A00
dX
rW
'F
L4-7
Slides courtesy of Prof M L Kraft, Chemical & Biomolecular Engr Dept, University of Illinois at Urbana-Champaign.
Concentration and Temperature• Molecular collision frequency concentration• Rate of reaction concentration
A A A B-r k T f C ,C ,...
Reaction rate is a function of temperature and concentration
CA : Concentration of A CB : Concentration of B
• As temperature increases, collision frequency increases
• Rate of reaction = f [( CA, CB, ……), (T)]
• At constant temperature : r = f(CA, CB, …….)
Specific rate of reaction, or rate constant, for species A is a function of temperature
L4-8
Slides courtesy of Prof M L Kraft, Chemical & Biomolecular Engr Dept, University of Illinois at Urbana-Champaign.
Elementary Reactions & Rate Laws• Dependence of reaction rate –rA on concentration of chemical species in
the reaction is experimentally determined• Elementary reaction: involves 1 step (only)• Stoichiometric coefficients in an elementary reaction are identical to the
powers in the rate law:
CBA BAAA CCkr
Reaction order:• order with respect to A• order with respect to B• Overall reaction order n =
Zero order: -rA = kA k is in units mol/(volume∙time)
1st order: -rA = kACA k is in units time-1
2nd order: -rA = kACA2 k is in units volume/(mol∙time)
3rd order: -rA = kACA3 k is in units volume2/(mol2∙time)
L4-9
Slides courtesy of Prof M L Kraft, Chemical & Biomolecular Engr Dept, University of Illinois at Urbana-Champaign.
Examples:
• This reaction is not elementary, but under some conditions it follows an elementary rate law
• Forward reaction is 2nd order with respect to NO and 1st order with respect to O2 (3nd order overall)
Overall Stoichiometric Equations• Overall equations describe the overall reaction stoichiometry• Reaction order cannot be deduced from overall equations
Compare the above reaction with the nonelementary reaction between CO and Cl2
2 22NO O 2NO 2
NO NO NO O2r k C C
2 2CO Cl COCl 3 2
CO CO Cl2r kC C
Forward reaction is 1st order with respect to CO and 3/2 order with respect to Cl2 (5/2 order overall)
L4-10
Slides courtesy of Prof M L Kraft, Chemical & Biomolecular Engr Dept, University of Illinois at Urbana-Champaign.
Specific Rate Constant, kAkA is strongly dependent on temperature
Where : A = Pre-exponential factor or frequency factor
(1/time)E = Activation energy, J/mol or cal/molR = Gas constant, 8.314 J/mol K (or 1.987 cal/mol K)T = Absolute temperature, K
Arrhenius Equation E RTAk T Ae
To determine activation energy E, run the reaction at several temperatures, and plot ln k vs 1/T. Slope is –E/R
Taking ln of both sides:
E 1lnk lnA
R T
1/T
ln k -E/R
L4-11
Slides courtesy of Prof M L Kraft, Chemical & Biomolecular Engr Dept, University of Illinois at Urbana-Champaign.
Reversible ReactionskA
k AaA b B c C d D
KC: concentration equilibrium constant (capital K)
a b a bfA A A B fA A A Br k C C r k C C
At equilibrium, the reaction rate is zero, rA=0
Rate of disappearance of A (forward rxn):c d
bA A C Dr k C CRate of generation of A (reverse reaction):
A,net A fA bAr r r r
a b c dA A A B A C Dr 0 k C C k C C
c dC DA
Ca bA A B
C CkK
k C C
Thermodynamic equilibrium relationship
RXC C 1
1
H 1 1K (T) K (T )exp
R T T
KC is temperature dependent (no change in moles or CP):
HRX: heat of reactionIf KC is known for temperature T1, KC for temperature T can be calculated
a b c dA A A B A C Dr k C C k C C
a b c dA A B A C Dk C C k C C
L4-12
Slides courtesy of Prof M L Kraft, Chemical & Biomolecular Engr Dept, University of Illinois at Urbana-Champaign.
L4: Rate Laws & Stoichiometry
• Reaction Rates (–rA )
1. Concentration 2. Temperature 3. Reversible reactions
• How to derive an equation for –rA [–rA = f(XA)]
1. Relate all rj to Cj
2. Relate all Cj to V or u3. Relate V or u to XA (Wednesday)
4. Put together (Wednesday)
A
A
XA
A00
dX
rt N
V
A
A
A0F XV
r
AXA
A00 Ar
dXV F
A
A
XA
A00
dX
rW
'F
L4-13
Slides courtesy of Prof M L Kraft, Chemical & Biomolecular Engr Dept, University of Illinois at Urbana-Champaign.
1. Relate all rj to Cj
• rA as a function of Cj is given by the rate law• The rate relative to other species (rj) is determined by stoichiometry
D ad
C ac
B ab A “A” is the limiting reagent
ad
r
ac
r
ab
rr DCBA
rj is negative for reactants,
positive for products
In general:j
Aj
rr
j≡ stoichiometric coefficientpositive for products, negative for reactants
ad
ac
1 ab
dcAB
L4-14
Slides courtesy of Prof M L Kraft, Chemical & Biomolecular Engr Dept, University of Illinois at Urbana-Champaign.
For the reaction the rate of O2
disappearance is 2 mol/dm3•s (-rO2= 2 mol/dm3•s).
What is the rate of formation of NO2?
2 22NO O 2NO
jA
j
rHint: r
2
2
NOO
rr
2 1 2 2O NO2 r r
2 2NO NO3 3
mol mol2 2 r 4 r
dm s dm s
rNO2 = 4 mol/dm3•s
L4-15
Slides courtesy of Prof M L Kraft, Chemical & Biomolecular Engr Dept, University of Illinois at Urbana-Champaign.
2a. Relate all Cj to V (Batch System)
BAAA CCkr Reaction rate is a function of Cj:
How is Cj related to V and XA? Batch: jj
N molC
V L
D ad
C ac
B ab A
B0 A0 AB
B
bN N X
N aCV V
C0 A0 AC
C
cN N X
N aCV V
AA
NC
V A0 A0 A
AN N X
CV
Put NA in terms of XA:
D0 A0 AD
D
dN N X
N aCV V
Do the same for species B, C, and D:
Cj is in terms of XA and V. But what if V varies with XA? That’s step 3a!
A0Aj0jj XNNN
L4-16
Slides courtesy of Prof M L Kraft, Chemical & Biomolecular Engr Dept, University of Illinois at Urbana-Champaign.
2a. Additional Variables Used in Textbook
B0 A0 AB
B
bN X
N aC
N
V V
Book uses term Θi:
A0
0
0
i
Ai
0 iC
C
N
N
So species Ni0 can be removed from the equation for Ci
A0
A0 A
AB0A
0
0
B
NbX
N
N N1 aC
N
VMultiply numerator by NA0/NA0:
A
B
B
B
A
AA0
0
BV
bX
XCba
Ca
NC
D ad
C ac
B ab A
L4-17
Slides courtesy of Prof M L Kraft, Chemical & Biomolecular Engr Dept, University of Illinois at Urbana-Champaign.
T
0 0 0 T0 0
ZN RTPVP V Z N RT
3a. Relate V to XA (Batch System)Volume is constant (V = V0) for:
• Most liquid phase reactions• Gas phase reactions if moles reactants = moles products
2 2 2CO g H O g CO g H g
If the volume varies with time, assume the equation of state for the gas phase:At time t: PV = ZNTRT and at t=0: P0V0 = Z0NT0RT0
P: total pressure, atm Z: compressibility factorNT: total moles T: temperature, K
R: ideal gas constant, 0.08206 dm3∙atm/mol∙K
d c b change in total # moleswhere = 1
a a a Moles A reacted
Want V in terms of XA. First find and expression for V at time t:
NT at time t is:
0 T0
0 0 T0
P NT ZV V
P T Z N
T j T0 A0 Aj
d c bN N N 1 N X
a a a T T0 A0 AN N N X
What is NT at t?
L4-18
Slides courtesy of Prof M L Kraft, Chemical & Biomolecular Engr Dept, University of Illinois at Urbana-Champaign.
TA
T0
N1 X
N
3a. Relate V to XA (continued)
T T0 A0 AN N N X d c b change in total # moleswhere = 1
a a a Moles A reacted
0 T0
0 0 T0
P NT ZV V
P T Z N
Can we use the eq. for NT above to find an expression for NT/NT0?
A0A0
T0 = =mole fraction of A iniS tubstitut ially pre:
Ny
Nesent
A0S eubsti xpanstute ion : ry facto
T T00
0A
T 00 T0
P T ZPlug : into
N NV V
P T1 X
N NZ
00
0A
0
P T ZV V
P T1
ZX
T0TA
T0 T0
A0
T0
N
N
NNX
N N
TA
T0A0
N1 y X
N
L4-19
Slides courtesy of Prof M L Kraft, Chemical & Biomolecular Engr Dept, University of Illinois at Urbana-Champaign.
T T0
AT0
N NX
N
What is the meaning of ε?
When conversion is complete (XA=1):
Tf T0 A
T0
N N Change in total # moles at X 1
N total moles fed
The expansion factor, , is the fraction of change in V per mol A reacted that is caused by a change in the total number of moles in the system
A0A0
T0
Nd c bexpansion factor: y 1
a a a N
TA
T0
N1 X
N If we put the following
equation in terms of ε:
TA
T0
N1 X
N
T T0
T0 A
N N
N X
00 A
0 0
P T ZV V
Z1
P TX where
L4-20
Slides courtesy of Prof M L Kraft, Chemical & Biomolecular Engr Dept, University of Illinois at Urbana-Champaign.
4a. Put it all together (batch reactor)
Batch:
0
j j0 jj
A0 A
0 A0 0
V P T
N N N X
ZV 1
P T
C
XZ
j A0 0 0
A 0
0 Aj
j T ZP1 X P T Z
CC
XC
For a given XA, we can calculate Cj and plug the Cj into –rA=kCjn
jjC
N
V
j0 A Aj
j 0CN
V
N Xj j j A AN N N X 0 0
00 A
0 0
P T ZV V 1 X
P T Z
0
0i0
i
V
NC
What about flow systems?
L4-21
Slides courtesy of Prof M L Kraft, Chemical & Biomolecular Engr Dept, University of Illinois at Urbana-Champaign.
2b. Relate all Cj to u (Flow System)
How is Cj related to uand Xj?
Flow:j
jF mol s mol
CL s Lu
BAAA CCkr
Reaction rate is a function of Cj:
D ad
C ac
B ab A
B0 A0 AB
B
bF F X
F aCu u
C0 A0 AC
C
cF F X
F aCu u
AA
FC
u A0 A0 A
AF F X
Cu
Put FA in terms of XA:
D0 A0 AD
D
dF F X
F aCu u
Do the same for species B, C, and D:
We have Cj in terms of XA and u, but what if u varies with XA? That’s step 3b!
A0Aj0jj XFFF
L4-22
Slides courtesy of Prof M L Kraft, Chemical & Biomolecular Engr Dept, University of Illinois at Urbana-Champaign.
3b. Relate u to XA (Flow System)Start with the equation of
state for the gas phase:
TT
NPC
ZRT V
What is CT0 at the entrance of the reactor?
T0 0T0
0 0 0
F PC
Z RTu
T
T0 0 0 0 0
F ZRT 1 P
F Z RT 1 Puu
TPV ZN RT
Rearrange to put in terms of CT, where CT = NT/V:
TT
FC
u
Can we relate CT to u? T
1F ZRT
Pu
0T0
T0 0 0
PF Z TF Z T P
u u
Rearrange to put in terms of u:
Put in terms of u0: T0 0 0 00
1F Z RT
Pu
Use these 2 equations to put uin terms of known or measurable quantities
TF PZRTu
L4-23
Slides courtesy of Prof M L Kraft, Chemical & Biomolecular Engr Dept, University of Illinois at Urbana-Champaign.
3b. Relate u to XA (continued) T T0 A0 A subst F F F X: and simplifyitute in
0
0T0 0
T0 A0
0
A PZ TF Z T P
F F Xu u
When conversion is complete (XA=1):
Tf T0 A
T0
N N Change in total # moles at X =1
N total moles fed
00
T0
T
0 0
PZ TF Z T P
Fu u
A0 substitute y:
A00
0 A0 0
PZ Ty1 X
Z T Pu u
A 00
0
A
T 0
0
0
X PZ T1
Z T
F
F P
u u
A0 0A0 A0 A0
A0 A0T0 T0 T0 0 T0
Simplify witN VF N F
y yF N N V F
Because : huu
00 A
0 0
PZ T1 X
Z T Pu u
L4-24
Slides courtesy of Prof M L Kraft, Chemical & Biomolecular Engr Dept, University of Illinois at Urbana-Champaign.
4b. Put it all together (flow reactor)
Flow:
0
j j0 j
0 A0 0
0 Aj
A
P T Z1 X
P
CF
T
F F X
Z
uu
j A0 0 0
A 0
0 Aj
j T ZP1 X P T Z
CC
XC
For a given XA, we can calculate Cj and plug the Cj into –rA=kCjn
jjC
F
u
j0 A Aj
j 0CF
V
F Xj j j A AF F F X 0 0
00 A
0 0
P T Z1 X
P T Zu u
0
0i0
iFC
u
This is the same equation as that for the batch reactor!
L4-25
Slides courtesy of Prof M L Kraft, Chemical & Biomolecular Engr Dept, University of Illinois at Urbana-Champaign.
4. Summary: Cj in terms of Xj
Batch:
j j0 j A0 Aj
00 A
0 0
N N N XC
V P T ZV 1 X
P T Z
j0 j A0 A 0 0j
A 0
C C X T ZPC
1 X P T Z
j0j0
0
NC
V
Flow:
j j0 j A0 Aj
00 A
0 0
F F F XC
P T Z1 X
P T Z
u
u j0
j00
FC
u
j0 j A0 A 0 0j
A 0
C C X T ZPC
1 X P T Z
This is the same equation as that for the batch reactor!
For a given XA, we can calculate Cj and plug the Cj into –rA=kCjn