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 18 Todays lecture Solution to inclass problem ID: 151991
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Slide1
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
18Slide2
Today’s lecture
Solution to
in-class
problemUser friendly Energy Balance DerivationsAdiabaticHeat Exchange Constant TaHeat Exchange Variable Ta Co-currentHeat Exchange Variable Ta Counter Current
2Slide3
Adiabatic Operation CSTR
The feed consists of both -
Inerts
I and Species A with the ratio of inerts I to the species A being 2 to 1.
Elementary liquid phase reaction carried out in a CSTR
3Slide4
Adiabatic Operation for CSTR
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.
4Slide5
CSTR Adiabatic Example
Mole Balance:
5Slide6
CSTR Adiabatic Example
Rate Law:
Stoichiometry
:
6Slide7
CSTR Adiabatic Example
Energy Balance - Adiabatic, ∆C
p
=0:
7Slide8
CSTR Adiabatic Example
Irreversible for Parts (a)
through
(c)
(a) Given X = 0.8,
find
T and V
(
if
reverible
)
8Slide9
CSTR Adiabatic Example
Given X, Calculate T and V
9Slide10
CSTR Adiabatic Example
(b)
(
if
reverible
)
Given T, Calculate X and V
10Slide11
CSTR Adiabatic Example
(c)
Levenspiel
Plot
11Slide12
CSTR Adiabatic Example
(c)
Levenspiel
Plot12Slide13
CSTR X = 0.95 T = 395
CSTR X = 0.6 T = 360
13
CSTR Adiabatic ExampleSlide14
PFR X = 0.6
PFR X = 0.95
14
CSTR Adiabatic ExampleSlide15
CSTR
X = 0.6
T = 360
V = 2.05 dm
3
PFR
X = 0.6
T
exit
= 360
V = 5.28 dm
3
CSTR
X = 0.95
T = 395
V = 7.59 dm
3
PFR
X = 0.95
T
exit
= 395
V = 6.62 dm
3
Summary
15
CSTR Adiabatic ExampleSlide16
(d) At
Equilibrium
Calculate Adiabatic Equilibrium Conversion and Temperature:
16Slide17
(d) At
Equilibrium
17
Calculate Adiabatic Equilibrium Conversion and Temperature:Slide18
(e) Te = 358
Xe
= 0.59
18
Calculate Adiabatic Equilibrium Conversion and Temperature:Slide19
T
T
a
V+
Δ
V
V
m
c
, H
C
F
A,
F
i
In - Out + Heat Added = 0
PFR
Heat
Effects
V+
Δ
V
V
F
i
T
T
a
F
i
19Slide20
PFR
Heat
Effects
20Slide21
PFR
Heat
Effects
21Slide22
PFR
Heat
Effects
22Slide23
Heat removed
Heat generated
PFR
Heat
Effects
23Slide24
User Friendly Equations Relate T and X or
F
i
3. PBR in terms of molar flow rates
24
4. For multiple reactions
5. Coolant BalanceSlide25
Heat Exchange Example
Elementary
liquid phase reaction carried out in a PFRThe feed consists of both
inerts I and Species A with the
ratio
of inerts to the species A
being
2 to 1.
25
F
A0
F
I
T
a
Heat Exchange Fluid
TSlide26
1)
Mole
Balance
:
2) Rate
Law
:
Heat Exchange Example
26Slide27
3)
Stoichiometry
:
4) Heat Effects:
Heat Exchange
Example
:
Case 1-
Constant
T
a
27Slide28
Parameters:
28
Heat Exchange
Example
:
Case 1-
Constant
T
aSlide29
Heat removed
Heat generated
PFR Heat
Effects
29Slide30
Energy
Balance
:
Adiabtic and ΔCP=0Ua=0
Additional
Parameters (17A) & (17B)
30
Heat Exchange
Example
:
Case 2
Adiabatic
Mole
Balance
:Slide31
Adibatic
PFR
31Slide32
Find conversion,
X
eq
and T as a function of reactor volume
V
rate
V
T
V
X
X
X
eq
Example
:
Adiabatic
32Slide33
Heat Exchange:
33
Need
to
determine
T
aSlide34
A.
Constant
Ta (17B) Ta = 300K
Additional Parameters (18B – (20B):
B. Variable T
a
Co-Current
C. Variable T
a
Counter
Current
Guess
T
a
at V = 0 to match T
a0
= T
a0
at
exit
, i.e., V =
V
f
34
User
Friendly
EquationsSlide35
Coolant balance:
In - Out + Heat Added = 0
Variable
T
a
Co-current
All equations can be used from before except T
a
parameter, use differential T
a
instead, adding
m
C
and C
PC
35
Heat
Exchanger
Energy
BalanceSlide36
In - Out + Heat Added = 0
All equations can be used from before except
dT
a/dV which must be changed to a negative. To arrive at the correct integration we must guess the T
a
value at V=0, integrate and see if T
a0
matches; if not,
re-guess
the value for T
a
at V=0
Variable
T
a
Counter-current
36
Heat
Exchanger
Energy
BalanceSlide37
Derive the User Friendly Energy
Balance
for
a PBRDifferentiating
with
respect
to W:
37Slide38
Mole
Balance
on species i:Enthalpy
for species i:
38
Derive the
User
Friendly
Energy
Balance
for
a PBRSlide39
Differentiating
with
respect
to W:39
Derive the
User
Friendly
Energy
Balance for a PBRSlide40
Final Form of the Differential
Equations
in Terms of
Conversion:
A:
40
Derive the User Friendly Energy Balance for a PBRSlide41
Final Form of terms of Molar Flow Rate:
B:
41
Derive the User Friendly Energy Balance for a PBRSlide42
Reversible Reactions
The rate
law
for this reaction will follow an elementary rate law.
Where
K
e
is the
concentration
equilibrium
constant
.
We
know
from Le
Chaltlier’s
law
that
if
the
reaction
is
exothermic
,
K
e
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, K
e
will
increase
and the
reaction
will
shift
to the right.
42Slide43
Reversible Reactions
Van’t
Hoff
Equation:
43Slide44
Reversible Reactions
For the special
case
of ΔCP=0Integrating the Van’t Hoff Equation gives:
44Slide45
Reversible Reactions
endothermic
reaction
exothermic
reaction
K
P
T
endothermic
reaction
exothermic
reaction
X
e
T
45Slide46
End of Lecture 1846