heterogeneous catalysis for green chemistry dr. m. sankar cardiff catalysis institute school of...
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Heterogeneous Catalysis for
Green Chemistry
Dr. M. Sankar
Cardiff Catalysis Institute
School of Chemistry
Cardiff University
Cardiff, UK.
02/01/2010
Cardiff Catalysis Institute
Overview of this Presentation
Organic Carbonates using CO2
Synthesis of Cyclic Carbonates
Synthesis of Dimethyl Carbonates
Selective oxidation using Gold nanocrystals based Catalysts
Oxidation of Benzyl Alcohol using Au-Pd Supported on TiO2
Oxidation of Glycerol using supported monometallic Catalysts.
Mt. Kilimanjaro (Africa ). Ice cap is shrinking
Columbia glacier AlaskaGlacier National Park 1914-1997
2008
Global Warming – Visible Effects
CO2 Emission & Possible Solution
Sequestration Utilization
M. A. Scibioh, B. Viswanathan Proc.Indn.Natl.Acad.Sci., 70A (3), 2004.
Various Chemical Transformations using CO2
Monomers Aprotic Organic Solvents Fine Chemical Intermediates
Cyclic Carbonate
Methylating Agent
Carbonylating Agent
Oxygenated fuel additive
Substitute for MTBE
Dimethyl Carbonate
Specific Reactions of Interest
O
R
O
R
O
C
O
CO2+
OO
O
MeOH MeO OMe
OOH
HO++
Cyclic Carbonate
Dimethyl Carbonate
Synthesis of Cyclic Carbonates
O
R
O
R
O
C
O
CO2+
+
Catalytic System-ICatalytic System-I
Na12[WZn3(H2O)2(ZnW9O34)2]46H2O(Zn-W-Sandwich Polyoxometalate)
Dimethylaminopyridine
N
N(CH3)2
Experimental conditions: 0.4 MPa CO2, 10 ml CH2Cl2,
0.0026 mmol of Zn-POM, DMAP = 3 mole equivalent Zn POM
Typical Reaction Data
Substrate Product Temp(deg C)
Time (Hrs)
Conv (%)
Selectivity(%)
140 3 98 98
160 9 96 97
160 12 99 97
O O
O
ClCl
O
O
CH3
O O
O
CH3
O
H
O O
O
H
Experimental conditions: 0.4 MPa CO2, 0.0026 mmol of Zn-POM, DMAP = 3
mole equivalent Zn POM
Data Continued…….
Substrate Temp(deg C)
Time (Hrs)
Conv (%)
Selectivity(%)
140 3 98 98
(without solvent)
140 3 99 98
(Recovered POM)
140 3 99 98
Cl
O
Cl
O
Cl
O
Experimental conditions: 0.4 MPa CO2, 10 ml CH2Cl2,
0.0026 mmol of Zn-POM, DMAP = 3 mole equivalent Zn POM
Data Continued…..
Substrate Sub: Cat ratio
Temp(deg C)
Time (Hrs)
Conv (%)
Selectivity(%)
10,000 140 3 97 98
25,000 140 3 98 98
50,000 140 3 84 98
Cl
O
Cl
O
Cl
O
2 0 0 3 0 0 4 0 0 5 0 0
B e f o r e
A f t e r
W a v e l e n g t h , n m
1200 800 400
After
Before
Wavenumber, cm-1
Structural Integrity of Zinc - Polyoxometalate
Proposed mechanism
+
_
O
ZnO CO2
, O
R
N
N(CH3)2
OZn
O
CO O O
RN
N(CH3)2
OZn
O
CO O
O
R
OZn
O
OC
O
O
R
N
N(CH3)2
-
Very high Substrate Vs Catalyst Ratio
Reaction without organic solvent – atom economy
Applicable to a range of epoxides
Polyoxometalate part is Recoverable and reusable
First ever Polyoxometalate based catalyst system
for this particular reaction
Highlights
M. Sankar, N. Tarte, P. Manikandan, Appl. Catal. A. 276 (2004) p.217. US Patent - 6,924,379 Indian Patent - Granted
Catalytic System-IICatalytic System-II
Si
Si-O
Si-O
Si-O
NN
Si
Si-OH
Si-O
Si-O
NN
OH
I II
and/or
Si
EtO
EtO
EtO
NHN
Si-OH
Si-OH
Si-OH
+
Silica
Cl +
Chloropropyl triethoxy silane Imidazole
L. T. Aany Sofia, Asha Krishnan, M. Sankar, N. K. Kala Raj, P. Manikandan, P. R. Rajamohanan, and T. G. Ajithkumar* J. Phys. Chem. C 113 (2009), 21114.
Si
Si-O
Si-O
Si-O
NN Si
Si-OH
Si-O
Si-O
NN
OH
Si-NMR of Fumed Silica Si-NMR of Functionalised Silica
Solid State NMR Characterization
Si
Si-O
Si-O
Si-O
NN
13C NMR of Functionalised Silica
0 5 10 15 200
20
40
60
80
100
p(CO2): 10 bar
120oC
70oC
90oC
Ep
oxid
e C
on
vers
ion
, (%
)
Time (h)
Cl CO2
O+
OO
O
Cl
1 2 3 40
20
40
60
80
100
: Epoxide Conv, : Cyclic Carbonate, : Others
Con
vers
ion
/ Sel
ectiv
ity,
%
Number of Catalytic Cycles
Reaction Data
Temperature Effect Recycle Studies
Catalyst Epoxide Temp/Time Epox Conv CC Selec
Si-Imid ECH 120 °C/4 h 98 98
No Catalyst ECH 120 °C/4 h <5 0
Si-Imid PO 130 °C/10 h 99 99
Si-Imid BO 130 °C/10 h 99 94
Si-Imid SO 130 °C/10 h 79 97
O
Cl
OO O
ECH PO BO SO
Catalyst Activity
150 120 90 60 30 0
*: CC**
*
ppm
Structural Stability – MAS-NMR
-180 -150 -120 -90 -60 -30 0
13C
29Si
Fresh
Recovered
Fresh
Recovered
Proposed - Mechanism
N
N
CO O
O
R
O
CO
O
R
O
R
Si
Si-O
Si-O
Si-O
NN
_
+
M.Sankar et.al., (Manuscript under preparation)
Highlights
Single Site – Heterogeneous Catalyst
Recoverable and Reusable
Easy to synthesize
Relatively mild reaction condition
CO2 : 6-10 bar, Temp: 90-130 ºC, Time: 4-10 h
Yield : > 96 %, Solvent: No Recoverable & Reusable: Yes
R = H, Cl, CH3
Cyclic Carbonate
R CO2
O+
OO
O
R
Zn-POM/DMAP
(or) Si-Imid
Summary
OO
O
MeOH MeO OMe
OOH
HO++
Synthesis of Dimethyl carbonate
Exp. Cond. EC/PC : 50mmol, Methanol : 500mmol
Catalyst: 1gm p-Xylene : 1gm Time: 5hrs
Sl.No.
Subs Catalyst TempoC
DMC Yield(%)
1 EC Na2WO4.2H2O 25 79
2 EC Na2WO4.2H2O
(I-Recov)
25 78
3 PC Na2WO4.2H2O 25 23
4 EC CaWO4 25 79
5 EC Li2WO4 25 66
6 EC K2WO4 25 71
7 EC Na2VO3 25 79
Catalytic System-I
Catalysis Data
0 1 2 3 4 50
20
40
60
80
10 °C 25 °C 50 °C 100 °C
DMC
Yield
(%)
Time (h)
Effect of Temperature
0 2 40
20
40
60
80
With MgO
After catalyst filteration at 1 h
With Catalyst
DM
C Y
ield
(%)
Time (h)
Heterogeneous Catalyst
20 40 60 80
4000 3500 3000 2500 2000 1500 1000
(b)
(a)
Fresh
Recovered
Wavenumber (cm-1)
Powder XRD
IR
Structural Integrity of Sodium Tungstate
1200 1000 800
Wavenumber (cm-1)
4000 3500 3000
(b)
(a)
1100 1000 900
FT-IR
Raman
1062
1030
8 min
6 min
4 min
2 min
0 min
Adsorbed CH3O-
CH3OH
Adsorbed CH3O -
Active Intermediate: IR and Raman Studies
O
O
O
MeO-
MeO-
OH
OH
O
O
O-
OMe
MeOH
O-
OH
O
O-
O
OMe
MeO
MeO
O
MeOH
O
OH
OMe
OMe
-O
O
OH
O
OMe MeO-+
++
Proposed Mechanism DMC formation
M. Sankar, N. Madhavan Nair, K.V.G.K. Murty, P. Manikandan, Appl. Catal. A. 312 (2006) p.108.
US Patent – Applied Indian Patent - Applied
Highlights
Active at room temperature
No CO2 pressure – pot reaction
Recoverable & Reusable
No complicated synthesis
Selective Oxidation using “Green” Oxidants
Introduction: Au and Au-Pd nanoparticles based catalysts have been reported to be very effective for :
Epoxidation of Alkenes: Hutchings et.al., Nature (2005).
Direct synthesis of Hydrogen Peroxide: Hutchings et.al., Science (2009).
Oxidation of Primary Alcohols: Hutchings et.al., Science (2006),
In this Presentation:
Oxidation of Benzyl Alcohol : Mechanistic Investigation
Oxidation of Bio-renewable Feedstocks : Glycerol Oxidation
0 2 4 6 8 10 12 14 16 18 20 22 240
10
20
30
40
50
60
70
80
90
100
Time/h
Be
nzy
alc
oh
ol c
on
vers
ion
/%
0
10
20
30
40
50
60
70
80
90
100
Be
nza
lde
hyd
e se
lectivity/%
Benzyl alcohol conversion and selectivity in benzaldehyde with the reaction time at 100 oC, 0.2 MPa O2 pressure: () Au/TiO2, ()Pd/TiO2, () Au-Pd/TiO2; solid symbols – conversion, open symbols – selectivity Science 2006AuPd nanoparticles prepared by impregnation1-50 nm Au-rich core, Pd-rich surface
Oxidation of Benzyl Alcohol using Au-Pd supported on TiO2
Aim is to understand the origin of Toluene in the “Solventless” oxidation of Benzyl alcohol and thereby “switching off” the toluene production
Experimental
50 ml Glass Reactor
Stirred at 1000 rpm – No mass transport limitations
Analysed by GC using mesitylene as external standard
Rates of the reaction were calculated for the first 10% conversion level
Catalyst Synthesis:
(Au-Pd)/TiO2, Au/TiO2, Pd/TiO2 by Sol-immobilization technique1
Catalytic Reaction (3 phase system: solid/liquid/gas)
1 J.A. Lopez-Sanchez, N. Dimitratos, P. Miedziak, E. Ntainjua, J.K. Edwards, D. Morgan, A.F. Carley, R. Tiruvalam, C.J. Kiely and G.J. Hutchings, Phys.Chem. Chem. Phys, 2008, 10, 1921.
Initial rates of reaction under oxygen at 80oC
Catalyst Benzyl Alcohol Benzaldehyde Toluene
d[BzOH]/dt( 10-7 mol s-1)
R2 d[Ald]/dt( 10-7 mol s-1)
R2 d[Tol]/dt( 10-7 mol s-1)
R2
1%(Au-Pd)/TiO2 -5.420 ± 0.46 0.986 4.810 ± 0.46 0.982 0.755 ± 0.151 0.950
0.5%Au/TiO2 -0.032 ± 0.0047 0.989 0.0316 ± 0.0044 0.990 0.000237 ± 0.0001 0.921
0.5%Pd/TiO2 -0.376 ± 0.09 0.947 0.359 ± 0.0857 0.948 0.00158 ± 0.0064 0.869
Catalyst: 0.02g Benzyl Alcohol: 1g O2: 1 bar Stirring: 1000rpm
Initial rates of reaction under He at 80oC
Catalyst Benzyl Alcohol Benzaldehyde Toluene
d[BzOH]/dt( 10-7 mol s-1)
R2 d[Ald]/dt( 10-7 mol s-1)
R2 d[Tol]/dt( 10-7 mol s-1)
R2
1%(Au-Pd)/TiO2 - 0.795 ± 0.043 0.959 0.422 ± 0.024 0.966 0.373 ± 0.027 0.941
0.5%Au/TiO2 -0.0367 ± 0.0032 0.992 0.0373 ± 0.002 0.997 0.000494 ± 0.000114 0.951
0.5%Pd/TiO2 - 0.404 ± 0.130 0.910 0.260 ± 0.078 0.921 0.144 ± 0.056 0.877
Catalyst: 0.02g Benzyl Alcohol: 1g He: 1 bar Stirring: 1000rpm
Monometallic versus Bimetallic Catalysts
No reaction in the absence of catalyst
Reaction of PhCH2OH versus PhCD2OH
0 1 2 3 4 5 6 7 8 9 108.4
8.5
8.6
8.7
8.8
8.9
9.0
Time/ 103s
BzO
H /
10
-3 m
ole
s
H BzOH
D BzOH
Rate of disappearance of benzyl alcohol ▲(Proton) ● (Deuterated) under 1 bar He
Under Oxygen (1 bar)
Substrate Benzyl Alcohol Benzaldehyde Toluene
d[BzOH]/dt( 10-7 mol s-1)
R2 d[Ald]/dt( 10-7 mol s-1)
R2 d[Tol]/dt( 10-7 mol s-1)
R2
PhCH2OH -5.42 ± 0.46 0.986 4.808 ± 0.46 0.982 0.755 ± 0.15 0.950
PhCD2OH -2.05 ± 0.14 0.993 1.867 ± 0.13 0.993 0.222 ± 0.03 0.974
KIE 2.65 2.58 3.41
Substrate: 1g Catalyst: 0.02g O2: 1bar Stirring: 1000 rpm Temp: 80oC
Deuterium NMR (coupled) of the reaction mixture (inset toluene peak magnified)
10 8 6 4 2 0
1.2 0.9 0.6
-CDO(Singlet)
CDCl3
BzOH
-CD3/CD
2H (Doublet)
-CD3/CD
2H Peak
Chemical Shift (ppm)
GC- Mass analysis of the reaction mixture – Comparison of protonated toluene and deuterated toluene part alone shown for clarity.
Effect of atmosphere on the initial rate of reaction
Gas/Press Benzyl Alcohol Benzaldehyde Toluene
d[BzOH]/dt( 10-7 mol s-1)
R2 d[Ald]/dt( 10-7 mol s-1)
R2 d[Tol]/dt( 10-7 mol s-1)
R2
He -0.795 ± 0.04 0.959 0.422 ± 0.02 0.966 0.373 ± 0.03 0.941
Air -2.288 ± 0.17 0.989 1.454 ± 0.09 0.992 0.832 ± 0.09 0.976
O2 / 1 bar -5.420 ± 0.46 0.986 4.808 ± 0.46 0.982 0.755 ± 0.15 0.950
O2 / 2 bar -6.440 ± 0.29 0.996 5.803 ± 0.29 0.996 0.595 ± 0.05 0.987
O2 / 3 bar -6.313 ± 0.38 0.995 5.862 ± 0.35 0.995 0.464 ± 0.06 0.980
Benzyl Alcohol : 1g Catalyst: 0.02g Temp: 80oC Stirring: 1000 rpm Pressure: 1bar
0.0 0.1 0.2 0.3 0.4 0.5 0.6 0.7 0.80
1
2
3
4
5
6
7
8
1 / VOH
1 / VAld
1 / VTol
1/[BzOH] mol / Kg
1/ V
To
l/ 10
7 m
ol /
Kg
s-1
Effect of dilution with o-xyleneLineweaver-Burk plot of initial rates versus formal concentration of benzyl alcohol
Derive vmax & Kd
Kd ald << Kd tolActive site for the two products
Appears to be different
PhCH2HC
HO Ph HC
PhHOO
O.H
COO. Ph H
H
HO H
H
PHe PO1
PO2
Speculation on mechanism & structure of precursor states
PhCH2OHPhCH2OH
CATPHe
PhCHO
PhCH3
PhCH2OH/O2
CAT
PO1
PO2
PhCHO
PhCH3
O2
He
M. Sankar et.al., Faraday Discussions, 2009 (In Press)
Glycerol Oxidation – Possible Products
Oxidation of Glycerol in an autoclave reactor using O2 or aq. H2O2
M.Sankar, N. Dimitratos,D. W. Knight, A. F. Carley,R. Tiruvalam,C. J. Kiely, D.Thomas,and G. J. Hutchings*, ChemSusChem, 2010 (In press)
Acknowledgements
Dr. P. Manikandan, NCL Pune
Prof. Graham J Hutchings, Cardiff University
Prof. David W Knight, Cardiff University
Prof. Donald Bethell, Liverpool University
Dr. S. Sivasanker, NCCR, Chennai
Prof. B. Viswanathan, NCCR, Chennai
EPSRC & CSIR