Upload
hidayah
View
218
Download
0
Embed Size (px)
Citation preview
8/19/2019 Dehydration of 2 3-Butanediol to Mek.2
1/9
The Dehydration
of
Fermentat ive
2,3=Butanediol into Met h y l Ethyl Ketone
A i
V.
Tran and Robert
P.
Chambers
Department of Chemical Engineering, Aubu rn Universi ty,
Auburn, Alabama 36849
Accepted for publ icat ion February 18, 1986
A solid acid catalyst consisted of sulfonic groups cova-
lently bound to an inorganic matrice was developed to
dehydrate 2,3-butanediol into methyl ethyl ketone. Rate
constant and apparent activation energy of the dehydra-
tion reaction were determined. The decay course
of
the
catalyst was
a
two-stage curve. The catalyst was deac-
tivated more rapidly in the first stage than in the second
stage. The strategy of maintaining constant degree of
dehydration was employed to lengthen the lifetime
of
catalyst. Treatment of the 2,3-butanediol containing fer-
mentation broth wi th activated carbon greatly facilitated
the subsequent dehydration reaction.
INTRODUCTION
Recent interest in the utilization of renewable lig-
nocelluloses has intensified research on the fermen-
tation of xylo se and glucose to 2,3-butanedi01'-~(here-
after butanediol). This is because butanediol is the
precursor of a n umber of com pounds.6 Among those
is methyl ethyl ketone (ME K). Com pared to ethanol ,
M EK has a higher heat of combu stion, 584.2 vs. 326.7
kcal/mol. It also gives an octan e num ber of 96.7 when
mixed (25% volume) with gasoline. ' Thu s, ME K is
more effective as a liquid fuel additive than e thanol.
A two-step process from butenes is usually used t o
make MEK.8 Butenes are f i rs t hydrated to give 2-
butanol which is then dehy drogen ated ov er zinc or
copper based catalysts at high temperatures and low
pressures to produce MEK. The conventional con-
version of ferme ntative butanediol into MEK
is
also
a
two-step process. Butanediol
is
first recovered from
ferme ntation broth and purified. It is then dehydra ted
ov er activ ated bentonite9 or sulfuric ac idlo*' to yield
MEK. Sulfuric acid is not able to convert butanediol
in the fermentation broth directly into MEK. This is
due to the preferential reaction of sulfuric acid with
unfermented xylose in the broth to the reaction of sul-
furic acid with butanediol.
In light of the above facts, the present report de-
scribes the direc t dehydratio n of butanediol in the fer-
mentat ion broth into ME K o ver a sol id acid catalyst .
Biotechnology and Bioengineering,
Vol.
XXIX,
Pp. 343-351
1987)
1987 John Wiley & Sons, Inc.
Th e advantag e of this method is the elimination of the
energy-intensive step of reco very and purification of
butanediol from ferm entation broth prior to the sub-
sequen t dehy drat ion react ion.
MATERIALS AND METHODS
Preparat ion of Sol id Acid Catalysts
Alumina and silica-alumina supports were used in
the preparation of catalysts. Alumina support (35-50
mesh) was obtained from Myco, Inc. and sil-
ica-alumina supports were from Davison Chemical and
Cyanamid. The support of Davison Chemical was in
pellet form (3/16 x 3/16 in.). It was then gro und, and
the 8-20 mesh fraction was retained for further use.
Th e su pport from Cyanamid was in fine form (40-60
mesh). Sulfhydryl groups were first covalently at-
tached t o the inorganic supp orts via silane intermedi-
ates.I2 The y were th en transform ed into sulfonic groups
using the procedure of Backer. l 3 The transformation
react ion was carr ied out at
60
? 1 and 90 +_ 1°C.
In
this w ork , the ca talysts A160, D60, and C60 were those
made at 60 1°C from alumina, Divison Chemical,
and Cyanamid suppo rts, respe ctively. Similarly, A190,
D90, and C90 were the catalysts prepared a t
90
1°C
from the co rresponding supports .
Reactors and th e Dehydrat ion
of
Butanedio l
Tubing Bomb
The dehydrat ion of butanediol into ME K was f irst
made in
a
21-cm-long, I-cm-I.D., stainless-steel tubing
bomb. After charging with A190 and butanediol (50
g/L), the tubing bomb was placed in an oil bath pre-
viously heated to a given temperature. It was then
cooled in a stream of water and filtered. The filtrate
was used for determinat ion of butanediol and M EK .
CCC
0006-3592/87/030343-09 04.00
8/19/2019 Dehydration of 2 3-Butanediol to Mek.2
2/9
Batch Autoc lave
A 600-ml Parr batch autoclave reactor was em-
ployed. About 13.5 g catalyst and 300 mL of
50
g/L
butanediol solution (Sigma Chemical) were used for
each run. T he st i r rer speed was 15 rpm. Tim e zero
(initial time) was the time at wh ich the rea ctor reached
the given tem perature. Sam ples were taken a t intervals
after passing a sampling coil (1 m) imm ersed in an ice-
water bath. After the dehydrat ion react ion, the reactor
was cooled and f il tered. T he catalyst was washed w ith
4 L distilled wate r and allowed to air-dry overnight. It
was used recurrently in three succe ssive runs a t iden-
tical conditions.
Packed Bed Reactor
Figure 1 depicts the packed bed reactor system used
in this work. A minipump (Milton Roy) pumped the
aqueous butanediol solution (50 g/L) through the sys-
tem. A fter passing 40 mL , the packed bed reactor was
immersed in an oil bath which was previously heated
to
a
given temperature. In or der to ensure equilibrium
condit ions, a foreru n of 40 mL w as passed before col-
lecting the liquid products for analysis. The pressure
of the system was 300 psi (gauge pressure).
Regeneration of Catalyst
The catalyst was washed by pumping water (500 ml)
through the packed bed reactor . Water was then re-
placed by hydrochloric acid [5% ( v h ) , 400 mL1. The
water-hydrochloric acid cycle was repeated three times.
Finally, the reactor was washed with water until no
trac e of hydrochloric acid was dete cted (the indicator
was methyl orange).
Preparation of Fermentation Broth
A
solution
(5
L) composed of NaCl (1 g/L),
M gS 047 H2 0 (0.2 g/L), NH4CI (2 g/L), yeast extract
(6
g/L),
and xylose (100 g/L) was sterilized at 120°C
fo r 15 min in
a
16-L fermentor (New Brunswick, type
SF-116). Inoculation (1
L)
of Klebsiella pneumoniae
AU-1-d3 was added to the medium. The butanediol
fermentat ion was then proceeded a t 32°C for 15 h. Th e
pH was maintained at 5.4 with
5N
NaO H. The source ,
grow th conditions, and inoculum composition of Kleb-
siella pneumoniae AU-l-d3 were described else-
where.I4 The fermentation broth was withdrawn from
the fermentor , centr i fuged (15 x lo3 rpm x 15 min,
at 4 C),
and
stored
in
a
cold
room (4°C).
Fermentation
products in
the broth
were butanediol(27.5
a ,
thanol
(4.2
g/L),
acetic
acid (2.1
g/L), and
acetoin
(5.7
g/L).
Figure
1. Scheme
of
the packed bed reactor system:
1 ) reservoir of butanediol solutio n, (2) minipump, (3) pressure gauge,
(4) relief valve,
(5)
filters, (6) quick-fix connector,
(7)
oil bath,
(8)
packed bed reactor,
(9)
coil 1 m), (1 0) ice-water bath, 1
1)
fraction
collector, (12) thermometer, 13) stainless-steel ubing, (14)200 mesh
screen, (15)glass wool, (16)glass bead
(3
mm
O.D.),
and
(17)
catalyst.
Treatment of Fermentation Broth
Since butanediol in the fermentation broth wa s not
efficiently dehydrated to
M E K
over the ca ta lys t s as
will be described later, two treatments were used for
the broth prior to th e subseq uent dehydrat ion react ion.
In the first treatm ent, the broth w as run through
a
glass
column (25 cm long
x
1.2 cm I.D.) packed w ith Am-
berlite IR-120, H+ orm. The treated broth was col-
lected after passing a forerun of 35 mL. In th e second
treatment , the broth w as t reated with act ivated carbon
(50
g/L, Darco grade
MD
3000) at 60°C
for
40 min. It
was then filtered (Whatman filter paper No. 3) and
centrifuged (12 x lo3 rpm x 10 min, a t 4°C).
Analytical
Butanediol and M EK from th e dehydrat ion reaction
were analyzed on a Varian gas c hromatog raph 3700
using a 1-m glass column packed w ith Chrom osorb 101
(60/80 mesh). The gas chromatograph was equipped
with a flame ionization dete ctor , a Varian autosam pler
5000, and a V arian integrater CDS-1 11C. Ferm entatio n
products w ere analyzed on the sam e equipment. Sulfonic
groups of the catalyst were determined by treating
the catalyst
(0.5
g) with 0 .1N NaO H
(50
mL ) overnight
with stirring. Th e residual Na OH was the n titrated with
0.
lNHC1. pH cur ve of the catalyst w as carried out with
a glass-electrode Ho rizon p H Controller 5997-20.
RESULTS AND DISCUSSION
Properties
of
Catalyst
Table I indicates that the catalys ts made at 90 ? 1°C
contained more sulfonic groups than did the
corre-
sponding ones prepared at
60
1°C. As seen in Figure
2, the initial pH of
A190,
D90, and C90 was higher than
344
BIOTECHNOLOGY AN D BIOENGINEERING, VOL.
29
FEBRUARY
1987
8/19/2019 Dehydration of 2 3-Butanediol to Mek.2
3/9
Table I. Sulfonic groups content and the dehydration
of
butanediol over various
catalysts in batch reactor.
Catalyst
A190
Run 1
Run 2
Run 3
A160
Run 1
Run
2
Run
3
D90
Run 1
Run 2
Run
3
6
Run
I
Run
2
Run 3
C90
Run
1
R un 2
Run 3
C60
Run 1
Run 2
Run 3
Rate constant
[min-
g-I ( x
Degree of
First Second butanediol
O,H
(meq/g) Overall stage stage dehydration ( )
1.31 32.97 100
18.48
12.55 26.02 98.6
13.45
9.79 16.13 89.2
1.28 28.47
100
16.55
13.73 21.04 93.4
9.80
8.08 10.84 81.5
1.44 53.37
100
18.67 16.84 23.11 97.3
1.22 9.13 7.03 11.10 91.7
1.41 44.77 100
18.06
14.67
22.46
96.5
7.66
5.42 9.07 87.0
1.81 39.85
100
9.62 7.92 10.65 94.4
I .05 2.61
2.24 2.74 86.7
1.59 32.92
100
11.10
10.53
11.84 90.7
4.33
3.36 5.00 84.3
that of A160, D60, and C60, respectively. Also, the pH
curves (Fig. 2) show that after ca. 0.75 mL of 0.1N
NaOH was consumed, the former catalysts had lower
pH than did the later catalysts. These results suggest
that
AIW, DW,
and C90may have lower external but
higher internal sulfonic groups than do the respective
catalysts
A160, D60,
and
C60.
Dehydrationof Butanediol into
MEK
Tubing
B o m b
In order to establish the reaction conditions of bu-
tanediol dehydration, tubing bomb was used. Results
in Figure 3 indicate that the dehydration reaction was
depended on the temperature and quantity of catalyst.
As temperature increased from 150 to 220 C, ca. 100%
increase in the degree of butanediol dehydration was
obtained. On the other hand, ca. 15 increase in the
degree of butanediol dehydration was observed for a
quadruple in catalyst quantity. Thus, the effect of tem-
perature on the butanediol dehydration was more pro-
nounced than that of catalyst quantity. From these
data, 2 10°C was arbitrarily selected as the dehydration
temperature for subsequent experiments.
2
A l 60
A l 90
D
60
D 90
C
60
c 90
- -
-. -
.
_---
_ . -
1 2
1
2 3
4 5
0 . N NaOH
( m l )
Figure 2. Titration curves with
0.1N
NaOH of various catalysts.
345
RAN AND CHAMBERS: DEHYDRATION
OF
2,3-BUTANEDIOL
8/19/2019 Dehydration of 2 3-Butanediol to Mek.2
4/9
T e m p e r a t u r e
( C)
C
0
0
L
V
>
JZ
W
.-
e
n
-
0
-0
W
t
0
.-
rn
w
0
W
W
L
0
W
n
0
0.5
1
o
1.5
2 . 0
A l 9 0 ( g )
Figure
3. Degree of butanediol dehydration a s a function of tem-
perature and cata lys t quantity.
The emp ty c ircles show 0.5 g A190,
12
m L 50 g/L butanediol, de-
hydrated for 150 min in the tubing bomb ; the solid circles show 12
m L 50 g/L butanediol, at 2WC, dehydrated for 150 min in the tubing
bomb.
Batch Autoclave Reactor
Shown in Figure 4 is the typical relationship of In
C/Co with reaction time for the catalysts D90 and C90.
Parameters
C o
and
C
were butanediol concentrations
at initial and different reaction times, respectively; the
slopes of the lines were the rate constants of the re-
action. Apparently, the dehydration reaction was first
- 1
0
\
c
2
- .
order in butanediol concentration. Both D90 and C90
completely dehydrated butanediol in the first run.
However, their activity was somewhat decreased in
the second and third recurrent runs as indicated by the
decreases in the reaction rate constant and degree of
butanediol dehydration of these runs (Table
I).
This
implies that both catalysts were deactivated. The de-
hydration reaction in the second and third runs fol-
lowed a two-stage path (Fig.
4).
Compared to the re-
action rate constant of the first stage, that of the second
stage was higher (Table I ) . Thus, the dehydration re-
action was faster in the second stage than in the first
stage. The reason of these facts will be elaborated later.
The behavior of other catalysts was similar to that
of D90 and C90. The catalysts made at
60
1°C had
lower reaction rate constants than did the correspond-
ing ones prepared at 90 ? 1°C. This is due to the lower
sulfonic groups of the former catalysts (Table I).
The apparent activation energy of the dehydration
reaction over the catalysts was 2.9
x
lo4 cal/mol, cal-
culated from their Arrhenius plots (not shown here).
This value is lower than that found for the dehydration
of butanediol by sulfuric acid
(3.6 x
lo4 cal/mol).
Packed Bed Reactor
Typical packed bed reactor profiles at 210°C are il-
lustrated in Figure 5 for the catalysts D90 and C90.
The butanediol concentration decreased to a minimal
point then increased gradually. This indicates that the
catalysts were deactivated after the maximal dehydra-
tion of butanediol occurred. Assuming that the dehy-
dration reaction was in the steady state, i.e., the bu-
tanediol concentration after the minimal point was
unchanged, the rate constant of the reaction was eval-
uated from the equation: In
C J C i
= - k ~ here
C i
- 1
- 2
-3
1 ' 1 . l . I . l . ~
40
80 1 2 0
160 2 0 0
0 4
8
120
160
2 0 0
T i m e ( m i n )
Figure 4.
2)
second run, and
(3)
third
run.
Correlation of In C/Co) with time for batch rea ctor at 210°C: A) catalyst D90,
(B)
catalyst C90, (1) first run,
346
BIOTECHNOLOGY AND BIOENGINEERING, VOL.
29,
FEBRUARY
1987
8/19/2019 Dehydration of 2 3-Butanediol to Mek.2
5/9
L
c
50
c
0
V
-
4 0
0
v
0
.-
30
m
20
- 1
T i m e (m in )
Figure
5.
in packed bed reactor at
210°C:
(A) catalyst D90, 15.4 g T
=
7. 7 rnin;
(B) catalyst C90, 27.5 g, T = 19.9 rnin;
( I ) run prior to the regenera tion of catalyst;
(2)
run a fter the first regen eration; and
(3) run after the second regeneration.
Profiles
of
butanediol dehyd ration over different catalysts
and
C
are butanediol concentrations at time zero and
at
the point of maximal dehydration, respectively. The
residence time, T was computed using the feed rate
(mL/min) and void volume of the catalyst bed (mL).
The void volume was assumed to be 70% of the total
volume of catalysts bed.I5
Again, the dehydration reaction rate constants of the
catalysts made at 90 1°C were higher than those of
the counterparts made at 60
?
1°C (Table 11 . Com-
pared to the reaction rate constants measured for batch
reactor, those determined for packed bed reactor were
slightly higher except for A160. Thus, the physical
properties, i.e., the differences in the void and pore
structures of the supports used, of the catalysts have
probably affected their behaviors in packed bed re-
actor. The degree of butanediol dehydration of the cat-
alysts made at 90
*
1°C was also higher than that of
the catalysts prepared at 60 1 C, thus corresponding
to the higher reaction rate constants (Table 11 and
higher sulfonic groups (Table
I
of the former catalysts.
Since the amount of
D90
used was small (Fig. 5 , its
degree of butanediol dehydration was expectedly low
(Table 11 .
The deactivation constant of the catalysts in packed
bed reactor was calculated using the equation
k, =
ke
- k d f , 1 6 where k, is the dehydration reaction rate con-
stant at time t after the maximal dehydration point; k
is the rate constant at the maximal dehydration point;
and kd is the deactivation constant. The deactivation
constant of the catalysts made at
90
1°C was slightly
lower than those of the counterparts made at 60 *
1°C
(Table 11 . As Figure 6 shows, the deactivation of the
catalysts was a two-stage curve. The catalysts were
deactivated faster in the first stage than in the second
stage (Table
11 .
These results will be discussed in de-
tail later.
Improvement
of
Catalyst A ct iv i ty
Batch Au toclave Reactor
One reason of the catalyst deactivation is due to
poisons which block the active sites, i.e. sulfonic groups,
of the ~at a1y st.l ~he dehydration in batch reactor was
then proceeded with the addition of
0.5%
(w/w, cata-
Table
11. Characteristics of the dehydration
of
butanediol over different catalysts in packed b ed reacto r.
Deactivation constant
[min-'
( x
lo- ]
Rate constant First Second Degree of butanediol
Catalyst [min-'
g- l
( x
Overall stage stage dehydration
( )
A190
33.59 33.65 52.17 10.57 87.7
First regeneration 15.21 27.67 40.56 21.96 60.7
Second regeneration
8.01 3 1.47 83.99 29.26 40.9
A160
30.08 34.07 54.07 16.35 79.4
D90
73.06 39.62 63.16 21.21 58.0
First regeneration 27.13 54.45 77.23 29.57 29.9
0 6 0
50.58 39.89 62.92 18.48 71.7
C90
67.06 35.57 52.69 29.37 97.4
First regeneration 16.76 43.79 69.04 27.02 50 0
Second regeneration 12.50 15.98
10.95
12.02 38.8
C60
46.30 39.16 59.46 14.13 83.3
Conditions of the dehydration reaction are given in Figure 5
TRAN AND CHAMBERS: DEHYDRATION
OF
2.3-BUTANEDIOL
347
8/19/2019 Dehydration of 2 3-Butanediol to Mek.2
6/9
A
T i m e (m i n )
Figure
6.
Deactivation curves
of
different catalysts used in packed bed reactor; see Figure
5
for
Codes.
lyst basis) of
0.5%
platinum on alumina
(40-60
mesh).
Prior
to
heating
,
he batch reactor was pressurized to
100 psi with hydrogen. As data in Tables I and I11
indicate, a lthough the p at tern of th e dehyd rat ion re-
action s with and without platinum w as the sam e, i.e.,
one stage in the first run and two-stage path in the
second and third recurrent runs, th e rate constants of
the former reaction (with platinum) were lower than
those of the latter reaction (without platinum). These
results imply that
a
part of sulfonic grou ps was blocked
by platinum containing alumina, thus resulting in lowe r
rate constants of the dehydration reaction with plati-
num. This, in turn, suggests that the deactivation of
catalyst was not caused by poisons but rather by the
decre ase in sulfonic groups. A
case
in point is the low er
sulfonic groups of
D90
and
C90
after the third run
(Table
I).
Due to the decrease in sulfonic groups, and
since the catalyst contained m ore internal than ex ternal
sulfonic groups a s mentioned earlier, i t may th en con-
ceive that afte r the first run the exte rnal sulfonic grou ps
were depleted at
a
much faster rate than were the in-
ternal sulfonic gr oup s. This will explain th e higher re-
Table
111.
Rate constant and degree
of
the butanediol dehydration in batch re-
actor with the addition of 0.5 w/w) platinum.
Rate constant
[rnin-' g-' ( x
Degree of
First Second butanediol
Catalyst Overall stage stage dehydration ( )
090
Run 1
35.39
100
Run
2 15.80 13.91 17.02 98. 2
Run
3 7.04 6.57 7.71 83.5
6
Run
1
34.32
100
Run
2 13.00 12.88 13.17 96.5
Run
3 5.49 3.50 7.82 84.0
C90
Run 1
35.22 100
Run 2 16.45 13.71 17.75 95.9
Run
3 7.82 7.39
8.06
85.7
C60
Run I 23.50 100
Run 2
10.55 9.47
11.10
86.5
Run 3 4.66 3.29 5.12 79.7
348
BIOTECHNOLOGY AND BIOENGINEERING, VOL. 29, FEBRUARY 1987
8/19/2019 Dehydration of 2 3-Butanediol to Mek.2
7/9
- 5 0 -
-
\
0
-
C 4 0 -
0
0
L
0
0
0
.-
2 3 0 -
20-
-
0
-0
0
0
.-
c 1 0 -
a
m
c
I
1
24
10 12 14
16 18
2 0 2 2
;,
2
4 6
T i m e
(hr)
Figure 7.
I ) catalyst D90, 185 C, 45 .9 g, = 74.1 min;
(2) catalyst D60, 192 C, 44.5 g,
=
72.3 min;
(3) ca ta lyst C60 , IW C , 40.6 g, = 83.6 min; and
(4) ca ta lys t C90, I W C , 38.4
g
7
=
87.7 min.
Profiles
of
butandiol dehydration over different catalysts in packed bed reactor at lower reaction temperatures:
action rate constants
of
the second stage compared to
those of the first stage in the second and third recurrent
runs (Tables I and 111).
Packed Bed Reactor
Regeneration of Catalyst.
It
is likely that the de-
hydration of butanediol proceeds with protons derived
from the sulfonic groups of the catalyst. Thus, the
mechanism of the reaction can be written as follows:
H O O H H O O H + *
I I H I I
I
CH3-C-C-CH3 - C H 3 - C - C - ~ ~ 3 ---
H H
H
(butanediol)
HO H + O
H
I II I
I
CH3-C-C-CH3 -- CH3-C-C-CH3
--
H
H
carbonium ion)
(secondary (oxonium ion)
The protons, in ideal state, will be recycled
in
the
dehydration reaction. Since the catalyst was deacti-
vated as proven above, the sulfonic groups might lose
Table
IV.
Rate constant, deactivation constant, and degree
of
butanediol dehydration
of
various catalysts
in packed bed reactor.
Deactivation constant
[rnin-I
(
x
10-91
Rate constant First Second Degree
of
butanediol
Catalyst [min-'
g-I
( X Overall stage stage dehydration ( )
D9
2.35
2.12 6.27 I .67 55.0
D60 3.18
3.85 11.97 2.89 63 .2
C90 8.14
4.60 9.84 3.45 93.6
C60
6.78
4.67 7.13 3.82 89.9
Conditions of the dehydration reaction are given in Figure 7 .
TRAN AND CHAMBERS: DEHYDRATION OF 2,BBUTANEDIOL
349
8/19/2019 Dehydration of 2 3-Butanediol to Mek.2
8/9
Table V.
of the dehydration reaction
of butanediol in simulated fermentation broth over the catalyst D90 in batch
reactor using conditions of Figure 4.
Rate constant [min-l g- ' ( X
Feed composition Run
I
Run
2
Run
3
Butanediol
(50
g/L)
53.37 18.67 9.13
Simulated fermentation broth (SFB)
12.58 3.50 0.03
SFB without yeast extract
53.31 17.31 9.31
a
Composition of SBF (g/L): ethanol,
11.5;
acetic acid, 4.5; acetoin, 2.3;
butanediol,
30;
NaCI, 1; MgSO4.7H2O,
0.2;
NH,CI,
2;
yeast extract,
6;
and
xylose,
100.
their protons. HC1 was then used to regenerate the
catalyst. Figure illustrates the profiles of the dehy-
dration over the regenerated catalysts. The regenera-
tion process did not improve the catalyst activity. The
rate constant and degree of butanediol dehydration of
the reaction over the regenerated catalyst were lower
than those of the reaction over the fresh catalyst (Table
11). These results imply that the deactivation of catalyst
was due to the
loss
of sulfonic groups in the reaction,
thus supporting the above conclusion on the catalyst
deactivation in batch autoclave reactor.
The above suggestion that during the dehydration
reaction the catalyst lost more external than internal
sulfonic groups can also be used to account for the
two-stage deactivation curve of the catalyst (Fig.
6).
It may envisage that the dehydration reaction in packed
bed reactor proceeded first with the external, then with
the internal sulfonic groups. Consequently, the deac-
tivation of the catalyst was a two-stage curve. Since
the remaining external sulfonic groups were lower as
already suggested, it is understandable that the deac-
tivation constant in the second stage was lower than
that of the first stage.
Maintenance of Constant Degree of Butanediol De -
hydration. One of the strategies to lengthen the catalyst
lifetime in packed bed reactor is to maintain a constant
degree of conver~ion.'~his can be done by either
varying the reaction temperature with time while keep-
ing the feed rate constant or changing the feed rate
while holding the reaction temperature constant. The
latter method was selected for the present catalyst. The
reaction temperature, however, was maintained a t ca.
190°C. This is because the temperature of the oil bath
could not be raised to 210°C. This fact, in turn, de-
manded
an
increase in the catalyst quantity. The pro-
files of this experiment is shown in Figure 7. The de-
grees of butanediol dehydration were almost the same
for the reactions at 210 and 190°C (Tables I1 and IV).
However, the lifetime of the catalyst was maintained
longer,
24
h vs.
6
h (Figs.
5
and
7),
although this re-
sulted in lower deactivation constant and reaction rate
constant.
Also,
the deactivation course of the catalyst
was unchanged. That is the catalyst was deactivated
more rapidly in the first stage than in the second stage
(Table IV).
Dehydration of Fermentative Butanediol
The catalyst D90 was first employed to examine the
effect of different components in the simulated fer-
mentation broth on the dehydration of butanediol in
batch reactor. Data in Table V indicate that xylose,
mineral salts, and fermentation products, i.e. butane-
diol, ethanol, acetic acid, and acetoin, did not hinder
the dehydration reaction. Yeast extract, however, in-
hibited the dehydration of butanediol, presumably
through the blockage of sulfonic groups. This is
fur-
thered by the fact that butanediol in the actual fer-
Table VI.
Dehydration of butanediol in actual fermentation broth in packed bed reactor using conditions of Figure
7.
Weight Temperature
Cataly st (g) ( C)
Feed
Rate const ant Degree of butanediol
[m in- ' g - ' ( x lo- )]
dehydration ( )
D90 35.2 185
butanediol
(27.5
g/L)
2.84
D90
35.5 185 actual fermentation broth
I
.27
D90 35.3 185 actual fermentation bro th 2.71
C90 38.4 190 butanediol (50
g/L)
8.14
C90 35.4 190 actual fermentation brotha 3.57
C90 34.7 190 actual fermentation broth 3.96
C90 35.2 190 actual fermentation broth
7.01
treated with activated carbon
treated with IR-120, H'
treated with activated carbon
57.5
21.2
44.4
93.6
60.6
65.7
80.7
a
See the Materials and Methods section.
350
BIOTECHNOLOGY AND BIOENGINEERING, VOL. 29, FEBRUARY 1987
8/19/2019 Dehydration of 2 3-Butanediol to Mek.2
9/9
mentation broth could not be effectively dehydrated
(Table
VI).
Again, the color bodies deposited on the
catalyst were the cause. Removal of the color bodies
by treating the actual fermentation broth with activated
carbon greatly facilitated the subsequent dehydration
reaction. On the other hand, treatment with Amberlite
IR-120, H did not affect much the dehydration over
the catalyst of the treated broth (Table VI). Similar
results were also obtained for the treatments with Am-
berlite
IR-45,
H-,
and trichloroacetic acid.
This research was financed by grants from the Advanced
Manufacturing Technology Center and the Pulp and Paper
Research and Engineering Center, Auburn University.
References
N .
B. Jansen and
G .
T. T sao, in
Adva nces in Biochemical En-
RinreringlBiotechnology A. Fiechter, Ed. (Springer-Verlag, New
York, 19831, pp. 85-99.
N. B. Jansen, M . C . Fl ickinger , and
G .
T. Tsa o , Biotechnol.
Bioeng .
26
362 (1984).
V. M. Laube ,
D.
Groleau, and S. M. Martin, Biotechnol. Le t t .
6
535 (1984).
J. M. Sablayrolles and
G .
G oma , Biotechnol.
Bioeng.
26 148
(1984).
5. A. Willetts,
Biotechnol.
Lett.,
6
263 (1984).
6 .
G.
A. Ledingh am and A. C. N eish in Industrial Fermentations
L. A. U nderkofler and R. J. Hickey, Eds . (Chemical Publishing
Co.,
New York, 1954), Vol. I , pp. 27-93.
7 . F. Baronnet,
M.
iclausa, A . Ahmed, R. Vischnievski, and L.
Charpene t , French Pa tent , French Demande 2367110 (May 5 ,
1978).
8. Kirk-Othmer,
Encyclopedia
of
Chemical Technology
3rd ed.
(Wiley, New York , 1981), Vol. 13, p. 905.
9. A. N . Bourns and R. V. V. Nicholls,
Ca n .
J.
Research
25B,
81
(1947).
10.
A. C. Neish, V. C. Haskell , and
F.
J .
MacDonald, Ca n .
J.
Research 23B, 81 (1945).
11 . R.
R .
Emerson, MS hesis, Purdue University, L.afayette, IN,
1981.
12. R. P. Chambers,
G.
A. Sw an, E. M. W al le , W. Cohen, and
W .
H. Baricos, in
Immobilized Enzyme Technology
H. H Weetall
and
S.
Suzuki, Eds. (Plenum, New York, 197 9, pp. 199-223.
13. H. J. Backer,
Rec . T ra v . Ch i m.
54, 215 (1935).
14. A. V. Tran and R. P. Chambers, App l. Microbiol. Biotechnol.
15. J . M. Sm ith , Chemical Engineering K inetics 3rd ed. (McGraw-
16.
0.
Levenspiel, Chemical Reaction Engineering
2nd
ed. (Wiley,
17.
J.
R. Gonzalez-Velasco, M.
A.
Gutierrez-Ortiz, J. I. Gutierrez-
23 191 (1986).
Hill, New York , 1981), pp. 327-356.
New Yo rk, 1972), p. 544.
Ortis, and A. Romeo, Chem . Eng. J.
28
13 (1984).
35
RAN AND CHAMBERS: DEHYDRATION OF 2.3-BUTANEDIOL