91
CHAPTER III
HYDROGENATION OF BENZYLIDENEANILINE AND ITS PARA
SUBSTITUTED DERIVATIES USING POLYMER-SUPPORTED
PALLADIUM IMIDAZOLE AND PALLADIUM
2-METHYLIMIDAZOLE COMPLEX CATALYSTS
In order to elucidate the potential of the synthesized polymer-
supported palladium-complexes as catalysts, hydrogenation of a few Schiff
bases (C=N), olefins and nitro compounds under ambient conditions has
been undertaken. This chapter is focused on catalytic activity of the
supported complexes towards hydrogenation of Schiff bases like
N-benzylideneaniline and few of its para derivatives under ambient
conditions (Scheme 3.1).
Scheme 3.1 Hydrogenation of benzylideneaniline and its derivatives.
3.1 Introduction
Hydrogenation of imines (C=N) to corresponding amines is an
important reaction which is one among the most fundamental chemical
transformations and a convenient way for synthesizing amines which are
useful pharmaceutical and agrochemicals1-5. Purest form of thallium-201
which is used routinely in nuclear medicine for imaging the myocardium
92
was obtained by liquid extraction of its precursor Pb201using N-benzylaniline
the hydrogenation product of benzylideneaniline by Sodd et.al.6.
Khosla et.al., has also reported the extraction of thallium in the presence of
other metal ions using N-benzylaniline7. Heterogeneous catalytic
hydrogenation of C=N using molecular hydrogen is environmentally clean
and commercially viable8. Earlier researchers have reported the
hydrogenation of Schiff bases like benzylideneaniline using transition metal
complexes as catalysts under high pressure and temperature1,9,10. Herein
the author has used the synthesized polymer-supported catalysts for the
hydrogenation of benzylideneaniline and few of its para substituted
derivatives at ambient conditions. The effect of the presence of substituents
on the rate of hydrogenation of benzylideneaniline has also been
investigated11.
Experimental
3.2 Preparation of Schiff bases
Schiff bases chosen as substrates for hydrogenation reactions;
benzylideneaniline and its para substituted derivatives (Table 3.1) were
prepared according to the procedure described in literature12. The general
condensation reaction is as follows. Eqimolar mixture of corresponding
freshly distilled aldehydes and aniline in ethanol (25 mL) was refluxed in a
round-bottom flask for about 3 hours. The products separated as solids on
pouring the reaction mixture into ice cold water. They were filtered and
recrystallized in ethanol. The prepared Schiff bases were characterized by
their melting point and GC-MS.
93
3.3 Polymer-supported palladium-imidazole complex catalyst for
hydrogenation of substituted benzylideneanilines*
3.3.1 Procedure for hydrogenation of Schiff bases
The reactor consisted of a horizontal water-jacketed, three-necked
glass tube of 75 mL volume connected to a water-jacketed hydrogen burette
and monometer. Water was circulated at a desired temperature from a
thermostat through the outer jacket of the reactor and that of the hydrogen
gas burette. In a typical experiment the catalyst was added to 30 mL of
ethanol in the reaction vessel and allowed to saturate in an atmosphere of
hydrogen for an hour. The system was evacuated and again filled with
hydrogen. A known quantity of the substrate was injected into the system
through the septum cap followed by opening the system to the gas burette
while closing the exit stopcock. The contents inside the reactor were agitated
by fixing it to a shaking machine. The reaction was monitored by the rise in
the level of the liquid in the hydrogen burette as a function of time13,14.
At the end of each reaction, the catalyst was separated by filtration and the
products were identified by IR, HPLC and GC-MS techniques.
3.3.2 Hydrogenation reaction of Schiff bases
Polymer-supported palladium-imidazole complex and its homogeneous
analogue Pd(Imz)2Cl2 was tried as catalysts for hydrogenation of
benzylideneaniline (to N-benzylaniline) in ethanol. The homogeneous
complex was unstable and during the course of the reaction metal got
separated from the solution15.
(*Udayakumar V., Gayathri V., et. al., J. Mol. Catal. A: Chem., 317 (2010) 111-117)
94
Table 3.1 Schiff bases
Benzylideneaniline (Bza)
Melting point ;
Found 49°C,
Expected 48°C
HC
N
p-Chlorobenzylideneaniline (p-ClBza)
Melting point;
Found 63°C,
Expected 64°C
HC
N
Cl
p-Methoxybenzylideneaniline (p-MeOBza)
Melting point;
Found 59°C,
Expected 61°C
p-Hydroxybenzylideneaniline (p-OHBza)
Melting point;
Found 191°C,
Expected 190°C
HC
N
OH
p-Nitrobenzylideneaniline (p-NBza)
Melting point;
Found 91°C,
Expected 90°C
HC
N
NO2
Hence the hydrogenation reactions were not carried out using the
homologous analogue. Whereas the polymer-supported palladium-imidazole
catalyst could be successfully used for the reduction of benzylideneaniline
and its derivatives. It was found that during the reaction metal does not
leach out from the polymer support and was found to be intact even after
recycling for six times (Fig 3.1). All the reactions were conducted in ethanol
at 596 mm Hg of hydrogen pressure12,16. Initial rate of hydrogenation of
various Schiff bases are presented in Fig. 3.2.
96
The percentage conversion of various Schiff bases as determined by HPLC
analysis, relatives rates of hydrogenation and TON (Turnover number) are
presented in Table 3.2.
0
2
4
6
8 p-OHBza
p-NBza
p-MeOBza
p-ClBza
Bza
Substrate
Fig. 3.2 Initial rates of hydrogenation of various Schiff bases using
polymer-supported palladium imidazole catalyst.
3.3.3 Kinetics and reaction mechanism
The kinetics of hydrogenation of the benzylideneanilines was studied
by following the hydrogen uptake at 596 mm Hg hydrogen pressure. The
rate of hydrogenation was calculated from the slope after plotting the
volume of hydrogen uptake by the substrate as a function of time. Initial
rates of hydrogenation of various Schiff bases and their TON have been
determined (Table 3.2). A blank reaction was also carried out in the absence
of the catalyst.
98
The results of hydrogenation reaction carried out using different
solvents indicated that the polar solvents are more favorable than non-polar
solvents and ethanol is most suitable among the solvents studied
(Table 3.3).
Table 3.3 Initial rates of hydrogenation of Schiff bases in various
solvents.
Solvent Initial rate x 10-4
(mol dm-3min-1)
Ethanol 8.77
Methanol 8.48
Toluene 5.25
Tetrahydrofuran 1.10
Benzene 2.11
Acetone 3.52
The dependency of the initial rates of hydrogenation on variables like
catalyst, substrate concentration and temperature was studied for all the
substrates.
a) Effect of catalyst concentration
The influence of catalyst concentration on the rate of hydrogenation
was carried out over a range of 14.8 x 10-4 to 14.8 x 10-3 mol dm-3 Pd at
constant substrate concentration of 33.3 x10-3 mol dm-3 at a temperature of
30oC with 596 mm Hg hydrogen pressure using ethanol as solvent12. Initial
rates are tabulated in Table 3.4 and the plot of log(initial rate) against
log[Catalyst] in the range of 14.8 x 10-4 to 74.2 x 10-4 mol dm-3 Pd is
depicted in Fig. 3.3.
99
Table 3.4 Initial rate of hydrogenation of Schiff bases with different
catalyst concentrations, constant [substrate] = 33.3 x 10-3,
596 mm Hg pressure of hydrogen at 303 K in 30 mL of ethanol.
[Catalyst] x10-4 (mol/dm-3 )
Pd
Initial rate x 10-4 (mol dm-3 min-1)
Bza
Initial rate x10-4 (mol dm-3 min-1)
ClBza
Initial rate x10-4 (mol dm-3 min-1)
OHBza
Initial rate x 10-4 (mol dm-3 min-1 )
MeOBza
14.8 3.08 2.40 3.00 5.20
29.6 5.04 4.61 5.00 5.66
44.4 6.01 5.49 5.20 6.10
59.2 8.77 5.53 6.81 6.64
74.2 7.22 9.46 10.60 6.87
-2.9 -2.8 -2.7 -2.6 -2.5 -2.4 -2.3 -2.2 -2.1
-3.7
-3.6
-3.5
-3.4
-3.3
-3.2
-3.1
-3.0
p-MeOBza
p-ClBza
Bza
log[catalyst]
Fig. 3.3 Plot of log (Initial rate) against log [catalyst].
= Benzylideneaniline = p-chlorobenzylideneaniline
-methoxy benzylideneaniline
Order of the reaction determined from the slope of the plot showed
that all the substrates followed fractional order kinetics. However the range
of concentration in which the catalyst follows the fractional order on the rate
is not the same for all the substrates. This may be due to the change in
structure of the substrate molecules. As the rate of hydrogenation of
hydroxy derivative is closer to that of chloro derivative the former has not
100
-2.6 -2.4 -2.2 -2.0 -1.8 -1.6 -1.4
-3.7
-3.6
-3.5
-3.4
-3.3
-3.2
-3.1
p-MeOBza
p-OHBza
p-ClBza
Bza
log[substrate]
been included in the plot. Above 74.2 x 10-4 mol dm-3 Pd concentration,
initial rate was found to be independent of catalyst concentration and it
followed zero order kinetics indicating that for the studied substrate 74.2 x
10-4 mol dm-3 Pd is sufficient to hydrogenate and higher concentration of
catalyst may not be required. Hence the rate becomes independent of
catalyst concentration.
b) Effect of substrate concentration
The influence of substrate concentration on the rate of the reaction
was studied in the range of 3.3 x10-3 to 66.6x10-3 mol dm-3 of substrate at
30oC and at 596 mm Hg hydrogen pressure with a constant catalyst
concentration of 59.2 x 10-4 mol dm-3 Pd for all the substrates in ethanol12.
The plot of log(initial rate) against log[substrate] in the range 3.3 x10-3 to
33.3 x10-3 mol dm-3 of substrate is given in Fig. 3.4. The initial rates of
hydrogenation are tabulated in Table 3.5.
Fig. 3.4 Plot of log (Initial rate) against log [substrate].
= Benzylideneaniline p-hydroxybenzylideneaniline
= p-methoxybenzylideneaniline; -chlorobenzylideneaniline
101
Order of the reaction in this concentration range for all the
substrates was found to be fractional. However the range of concentration
where the substrate follows a fractional order on the rate is not the same for
all the substrates. This may be due to change of substituents in substrate
molecules and coordinating ability of the catalyst towards different
derivatives. Initial rate was independent of substrate concentration above
33.3 x 10-3 to 66.6 x 10-3 mol dm-3 and followed zero order17. This could be
attributed to the fact that as the catalyst concentration is kept constant, all
the catalyst would have been used and no catalyst is available for higher
concentration of the substrate.
Table 3.5 Initial rate of hydrogenation of Schiff bases with different
substrate concentrations, constant [Catalyst] = 59.2 x10-4, 596
mm Hg pressure of hydrogen at 303 K in 30 mL of ethanol.
[Substrate]
x 10-3
(mol/dm-3)
Initial rate x 10-4
(mol dm-3 min-1 )
Bza
Initial rate x 10-4
(mol dm-3 min-1 )
ClBza
Initial rate x 10-4
(mol dm-3 min-1 )
OHBza
Initial rate x 10-4
(mol dm-3 min-1 )
MeOBza
3.3 4.21 2.04 2.40 2.21
8.3 5.29 2.71 4.21 2.76
16.6 6.77 3.69 4.98 4.17
25.0 7.82 3.83 6.40 4.86
33.3 8.77 5.53 6.81 6.64
c) Mechanism of hydrogenation of Schiff bases
Based on the results obtained from the kinetics experiments, a
probable mechanism is proposed for the hydrogenation reaction1 (Scheme
3.2). The polymer bound catalyst binds reversibly with the substrate. In the
102
Pd2+
N
C
R
H RI
Pd2+
N
C
R
H RI
K
+
N
C
R
H RI
N
C
R
H RI
Pd4+
H H
Pd2+
H2
k1
Slow
Pd4+
H
N
C
R
H RI
Pd4+
H H
H
N
C
R
H RI
Fast
Pd2+
N
C
R
H
H
H
RI
Pd4+
H
N
C
R
H
H
RI
Fast+
-complex reacts with hydrogen to form a dihydrido complex
which finally gives the amine.
Catalyst Substrate -Complex (intermediate)
-Complex Dihydrido complex
Dihydrido complex -Complex
- Complex Catalyst Amine
Scheme 3.2 Probable mechanism for hydrogenation of Schiff bases.
The rate law derived for the above mechanism is given in equation 1.
Total Total
1
Unreacted Unreacted
Equation 1
Where K is the equilibrium constant for reversible reaction and k1 is the
velocity constant for the rate determining step. This equation explains that
103
at low concentration, the reaction follows fractional order with respect to
catalyst and substrate concentration. But at higher concentration the rate is
independent of catalyst and substrate concentration.
d) Dependency of the rate on the temperature of the reaction
Rate of hydrogenation reactions for all the substrates were studied
in the range of 30 to 45oC with a constant catalyst concentration of
59.2 x 10-4 mol dm-3 Pd, substrate concentration of 33.3 x 10-3 mol dm-3 in
ethanol at 596 mm Hg pressure of hydrogen. The rate of the reaction was
found to be dependent on temperature (T) of the system (Table 3.6). Values
of activation energy calculated from the slope of Arrhenius plot (Fig. 3.5) and
activation entropy of reactions are tabulated in the Table 3.7. Results
revealed that activation energy decreased after substituting -NO2, -OH, -Cl
or -MeO group on to the para position of aldehyde ring of benzylideneaniline.
The lower activation entropy indicates that the substrate molecules are
bonded to the catalyst surface and they have lost all translational degrees of
freedom and probably gained only three vibrational degrees of freedom.
Further, activation of the substrate with the catalyst may be due to
localization of the substrate on the catalyst surface and this localized
interaction may be necessary for the hydrogenation reaction since a double
bond (C=N) involved is in the middle of the substrate molecule.
104
3.2x10-3
3.2x10-3
3.2x10-3
3.3x10-3
3.3x10-3
-3.2
-3.1
-3.0
-2.9
-2.8
p-MeOBza
p-OHBza
p-ClBza
Bza
1/T
Fig. 3.5 Effect of temperature - Arrhenius plot.
Benzylideneaniline p-hydroxy benzylideneaniline
= p-methoxybenzylideneaniline -chloro benzylideneaniline
Table 3.6 Initial rate of hydrogenation of Schiff bases at different temperatures with [catalyst] = 59.2 x 10-4 mol/dm3 Pd, [substrate] = 33.3 x 10-3 mol/dm3 , 596 mm Hg pressure of hydrogen, in 30 mL of ethanol.
Temperature (K)
Initial rate x 10-4 (mol dm-3 min-1)
Bza
Initial rate x 10-4 (mol dm-3 min-1)
ClBza
Initial rate x 10-4 (mol dm-3 min-1)
OHBza
Initial rate x 10-4 (mol dm-3 min-1 )
MeOBza
303 8.77 5.53 6.81 6.64
308 10.70 6.03 8.08 7.21
313 13.20 6.25 9.86 8.14
318 16.41 6.63 10.48 8.12
Table 3.7 Activation energy, Activation entropy values for hydrogenation of benzylideneaniline and its derivatives using polymer-supported palladium-imidazole catalyst.
Substrate Activation energy
(kJ/mol)
Activation entropy
(J/Kmol)
Benzylideneaniline 34 -200
p-Chlorbenzylideneaniline 9 -286
p-Hydroxybenzylideneaniline 24 -233
p-Methoxybenzylideneaniline 12 -276
p-Nitrobenzylideneaniline 31 -212
105
e) Effect of substituents on the rate of hydrogenation
To determine the effect of substitution at the para position of
benzylideneaniline on hydrogenation, few derivatives with -NO2, -Cl, -OH
and -MeO groups were chosen. Earlier studies have shown that the
introduction of substituents at para position of the amine ring of the
benzylideneaniline has very little effect on the hydrogenation rate18. In our
studies it has been observed that the insertion of substituents on to the
para position of aldehyde ring of benzylideneaniline reduced the activation
energy markedly (Scheme 3.1, Table 3.7). When p-nitrobenzylideneniline
was used as the substrate, both C=N and nitro group were hydrogenated
simultaneously (Fig 3.6) and the catalyst does not show selectivity towards
C=N. Hence the effect of nitro group substitution on the rate could not be
determined. Similar observation was made by Arthur Roe et.al.12.
Effect of substituents on the rate of hydrogenation of
benzylideneaniline was studied by varying the para substituents with
different groups like -OH, -MeO, and Cl16. It was observed that the rate of
hydrogenation was slower upon substitution with these groups. When
log(initial rate) was plotted ag para) it
was a straight line (Fig.3.7) indicating that the substituents do not have
significant effect on the rate of the reaction.
107
-0.4 -0.3 -0.2 -0.1 0.0 0.1 0.2 0.3
-3.26
-3.24
-3.22
-3.20
-3.18
-3.16
c
b
a
-OH
-Cl
-MeO
Substituent constant
Fig. 3.7 Effect of para substituents on the initial rate of hydrogenation
a: p-Hydroxybenzylideneaniline; b: p-Methoxybenzylideneaniline;
c: p- Chlorbenzylideneaniline.
3.3.4 Recycling efficiency of the catalyst
In order to test metal leaching from the catalyst, metal estimation
was carried out at the end of first cycle and at the end of sixth cycle of the
reaction. Percentage of metal in the catalyst remained almost constant even
after six cycles. (At the end of first cycle 9.9% Pd and at the end of sixth
cycle 9.8% Pd). Metal estimation for the reaction mixture was also carried
out to make sure that there is no loss of metal from the catalyst. From this
analysis it is evident that there is no leaching of metal from the catalyst.
Recycling ability of the catalyst was studied by carrying out reactions over
six cycles at a constant catalyst concentration of 59.2x10-4 mol dm-3 Pd,
substrate concentration of 33.3x10-3 mol dm-3 and temperature 30oC with
596 mm Hg of hydrogen pressure. The initial rate remained almost constant
for over six cycles without any loss in efficiency of the catalyst (Table 3.8).
108
Table 3.8 Recycling efficiency of polymer-supported palladium imidazole
complex catalyst.
Initial rate x 10-4
(mol dm-3 min-1 )
Fresh 8.77
First cycle 8.66
Second cycle 8.30
Third cycle 8.30
Fourth cycle 8.30
Fifth cycle 8.24
Sixth cycle 8.20
3.4 Hydrogenation of benzylideneaniline and its derivatives using
polymer-supported palladium 2-methylimidazole complex
catalyst
Hydrogenation of benzylideneaniline and its para-substituted
derivatives using polymer-supported palladium 2-methylimidazole catalyst
(Scheme 3.1) was carried out under similar conditions as followed for
palladium-imidazole catalyst (Section 3.3.1) and kinetic studies were carried
out as described in section 3.3.3. Initial rates of hydrogenation are depicted
in Fig. 3.7 and tabulated in Table 3.9 along with TON and percentage
conversions as determined by HPLC analysis. When homogeneous analogue
of polymer-supported palladium-2-methylimidazole [Pd(meImz)2Cl2]
(meImz = 2-Methyl imidazole) was used as catalyst, metal got separated
from the solution and hence it could not be used as catalyst.
110
Fig. 3.7 Initial rates of hydrogenation of various Schiff bases using
polymer supported palladium-2-methylimidazole catalyst.
3.4.1 Kinetic studies and reaction mechanism
a) Effect of catalyst concentration
The influence of catalyst concentration on the rate of hydrogenation
was carried out over a range 14.8x10-4 to 11.9 x10-3 mol dm-3 Pd at constant
substrate concentration of 33.3 x10-3 mol dm-3 at a temperature of 30oC with
596 mm Hg hydrogen pressure using ethanol as solvent12 (Table 3.10). The
plot of log(initial rate) against log[Catalyst] in the range of 14.8x10-4 to
74.2x10-4 mol dm-3 Pd is depicted in Fig. 3.8. Order of the reaction
determined from the slope of the plot showed that all the substrates followed
fractional order kinetics. Above 74.2x10-4 mol dm-3 Pd concentration, initial
rate was found to be independent of catalyst concentration and it followed
zero order kinetics.
111
Table 3.10 Initial rate of hydrogenation of Schiff bases with different
catalyst concentrations, constant [substrate] = 33.0 x 10-3,
596 mm Hg pressure of hydrogen at 303 K in 30 mL of ethanol.
[Catalyst] x10-4
(mol/dm3 ) Pd
Initial rate x 10-4
(mol dm-3 min-1)
Bza
Initial rate x 10-4
(mol dm-3 min-1)
ClBza
Initial rate x 10-4
(mol dm-3 min-1)
OHBza
Initial rate x 10-4
(mol dm-3 min-1 )
MeOBza
14.8 5.68 2.31 4.63 4.10
29.6 7.17 3.43 5.38 4.73
44.4 8.31 4.12 5.92 5.15
59.2 9.46 4.84 6.31 5.68
74.2 9.99 5.17 7.04 6.16
-2.9 -2.8 -2.7 -2.6 -2.5 -2.4 -2.3 -2.2 -2.1
-3.65
-3.60
-3.55
-3.50
-3.45
-3.40
-3.35
-3.30
-3.25
-3.20
-3.15
-3.10
-3.05
-3.00
Hydroxy
chloro
Methoxy
Bza
log[Catalyst]
Fig. 3.8 Plot of log (Initial rate) against [catalyst].
Benzylideneaniline = p-Chloro benzylideneaniline
= p-Methoxy benzylideneaniline - hydroxy benzylideneaniline
112
b) Effect of substrate concentration
The influence of substrate concentration on the rate of the reaction
was studied in the range of 3.3x10-3 to 66.7x10-3 mol dm-3 of substrate at
30°C and 596 mm Hg hydrogen pressure with a constant catalyst
concentration of 59.2x10-4 mol dm-3 Pd for all the substrates in ethanol12.
The plot of log(initial rate) against log[substrate] in the range 3.3 x 10-3 to
33.3 x 10-3 mol dm-3 is given in Fig. 3.9 and the initial rates of
hydrogenation is tabulated in Table 3.11. Order of the reaction in this
concentration range for all the substrates was found to be fractional. Above
33.3 x 10-3 to 66.7 x 10-3 mol dm-3 initial rate was independent of substrate
concentration and followed zero order13. This could be attributed to the fact
that as the catalyst concentration is kept constant, all the catalyst would
have been used and no catalyst is available for higher concentration of the
substrate.
c) Mechanism of hydrogenation of Schiff bases
The mechanism of hydrogenation of Schiff bases followed by polymer-
supported 2-methylimidazole catalyst and rate equation proposed based on
the kinetic experimental results was observed to be similar as described in
Scheme 3.2 and equation 1.
Total Total
1
Unreacted Unreacted
Equation 1
113
-2.6 -2.4 -2.2 -2.0 -1.8 -1.6 -1.4
-3.75
-3.70
-3.65
-3.60
-3.55
-3.50
-3.45
-3.40
-3.35
-3.30
-3.25
-3.20
-3.15
-3.10
-3.05
log[Substrate]
Table 3.11 Initial rate of hydrogenation of Schiff bases with different
substrate concentrations, constant [Catalyst] = 59.2 x10-4,
596 mm Hg pressure of hydrogen at 303 K in 30 mL of ethanol.
[Substrate] x 10-3
(mol/dm3)
Initial rate x 10-4
(mol dm-3 min-1 )
Bza
Initial rate x 10-4
(mol dm-3 min-1 )
ClBza
Initial rate x 10-4
(mol dm-3 min-1 )
OHBza
Initial rate x 10-4
(mol dm-3 min-1 )
MeOBza
3.3 3.58 1.89 2.63 3.05
8.3 4.42 2.94 3.68 3.68
16.6 5.78 4.21 4.73 4.42
25.0 6.83 4.73 5.68 5.05
33.3 9.46 4.84 6.31 5.68
Fig. 3.9 Plot of log (Initial rate) against [Substrate].
Benzylideneaniline = p-Chlorobenzylideneaniline
= p-Methoxy benzylideneaniline = p-Hydroxybenzylideneaniline
114
d) Dependency of the rate on temperature of the reaction
Rate of hydrogenation for all the substrates were studied in the
range of 30 to 50°C with a constant catalyst concentration of 59.2 x 10-4 mol
dm-3 Pd, substrate concentration of 33.3 x 10-3 mol dm-3 in ethanol at 596
mm Hg pressure of hydrogen. The rate of the reaction was found to be
dependent on temperature (T) of the system (Table 3.12). Values of
activation energy calculated from the slope of Arrhenius plot (Fig. 3.10) and
activation entropy of reactions are tabulated in the Table 3.13. Results
revealed that activation energy decreased after substituting -OH, -Cl or
-MeO group on to the para position of aldehyde ring of benzylideneaniline.
The lower activation entropy indicates that the substrate molecules are
bonded to the catalyst surface and they have lost all translational degrees of
freedom and probably gained only three vibrational degrees of freedom.
Further, activation of the substrate with the catalyst may be due to
localization of the substrate on the catalyst surface and this localized
interaction may be necessary for the hydrogenation reaction since a double
bond (C=N) involved is in the middle of the substrate molecule.
115
Table 3.12 Initial rate of hydrogenation of Schiff bases at different
temperatures with constant [catalyst] = 59.2 x 10-4 mol/dm3
Pd, [substrate] = 33.3 x 10-3 mol/dm3, 596 mm Hg pressure of
hydrogen, in 30 mL of ethanol.
Temperature
(K)
Initial rate x 10-4
(mol dm-3 min-1)
Bza
Initial rate x 10-4
(mol dm-3 min-1)
OHBza
Initial rate x 10-4
(mol dm-3 min-1 )
MeOBza
303 9.46 6.31 5.68
308 11.6 8.17 7.76
313 13.2 10.1 9.36
318 15.0 13.4 11.3
323 16.8 15.2 13.2
3.1x10-3
3.2x10-3
3.2x10-3
3.3x10-3
3.3x10-3
-3.30
-3.25
-3.20
-3.15
-3.10
-3.05
-3.00
-2.95
-2.90
-2.85
-2.80
-2.75
1/T
Fig. 3.10 Effect of temperature - Arrhenius plot. log (Initial rate) ><1/T.
= p-Methoxybenzylideneaniline;
p-Hydroxybenzylideneaniline. Benzylideneaniline.
116
Table 3.13 Activation energy, activation entropy for hydrogenation of
benzylideneaniline and its derivatives using
polymer-supported palladium-2-methylimidazole catalyst.
Substrate Activation energy
(kJ/mol)
Activation entropy (J/Kmol)
Benzylideneaniline 21 -275
p-Hydroxybenzylideneaniline 31 -246
p-Methoxybenzylideneaniline 33 -236
p-Chlorobenzylideneaniline 15 -298
e) Effect of substituents on the rate of hydrogenation of
benzylideneaniline
Effect of substituents on the rate of hydrogenation of
benzylideneaniline was studied by varying the para substituents with
different groups like OH, -MeO, and Cl. Results revealed that the rate of
hydrogenation decreased upon substitution with these groups due to steric
crowding around C=N. The plot of log(Initial rate) against Hammet
para) was a straight line (Fig.3.11). When
p-nitrobenzylideneaniline was used as substrate, both C=N and nitro group
were hydrogenated simultaneously indicating that the catalyst was not
selective towards C=N.
117
-0.4 -0.3 -0.2 -0.1 0.0 0.1 0.2 0.3
-3.32
-3.30
-3.28
-3.26
-3.24
-3.22
-3.20
C
Cl
-MeO
b
a
-OH
Substituent constant
Fig. 3.11 Effect of para substituents on the initial rate of hydrogenation
Plot of log (Initial rate) >< Hammett nstant.
a: p-Hydroxybenzylideneaniline , b:p-Methoxybenzylideneaniline
c: p- Chlorbenzylideneaniline
3.4.2 Recycling studies
Recycling studies carried out using benzylideneaniline as substrate at
a constant catalyst concentration of 59.2x10-4 mol dm-3 Pd,
benzylideneaniline concentration of 33.3x10-3 mol dm-3 and temperature
30°C with 596 mm Hg of hydrogen pressure revealed that the catalyst have
excellent recycling efficiency over six cycles without leaching of metal from
the polymer-support.
118
Table 3.8 Recycling efficiency of the catalyst
Initial rate x 10-4
(mol dm-3 min-1)
Fresh 9.46
First cycle 9.40
Second cycle 9.32
Third cycle 9.30
Fourth cycle 9.28
Fifth cycle 9.28
Sixth cycle 9.10
3.5 Conclusion
Reactivity of the two synthesized catalysts has been evaluated by
comparing the initial rates of hydrogenation of Schiff bases under identical
conditions. Both catalysts could be used for hydrogenation of C=N group at
ambient temperature and pressure to synthesize corresponding amines. In
general polymer-supported imidazole catalyst showed better catalytic
activity than polymer-supported 2-methylimidazole catalyst for
hydrogenation of substituted benzylideneanilines (Table 3.9). Percentage
conversion, activation energy was relatively higher in case of palladium-
imidazole catalyst when compared to palladium-2-methylimidazole catalyst.
Substrates followed the same reaction mechanism (Scheme 3.2) and similar
rate equation (Equation 1) for both the catalysts. Both the catalysts have an
excellent recycling efficiency over six cycles without leaching of metal from
the polymer-support.
120
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