# Patent

## Title
Synthesis of dimethyl carbonate from carbon dioxide and methanol

## Abstract

A method for producing dimethyl carbonate from methanol and carbon dioxide using a heterogeneous catalyst is described. The heterogeneous catalyst provides both acidic sites and basic sites. The reaction can be carried out at atmospheric pressure and relatively low temperatures.

## Background
CROSS REFERENCES TO RELATED APPLICATIONS
This application claims priority upon U.S. provisional application Ser. No. 61/302,675 filed Feb. 9, 2010.


FIELD OF THE INVENTION
The present invention relates to methods of producing dimethyl carbonate from carbon dioxide and methanol. The methods utilize a particular class of heterogeneous catalysts.
BACKGROUND OF THE INVENTION
Catalysts play a key role in increasing the efficiency of chemical synthesis and processing by lowering the reaction temperature and pressure, increasing product yield, and reducing by-product formation. Development of environmentally benign synthesis processes that eliminate toxic feed stocks, combine process steps, and result in a net reduction of pollutants and energy use rests on, to a great extent, the ability for innovation in the design of synthesis pathways and their catalyst.
CO2 utilization is an important process from the viewpoint of green chemistry. The objective of CO2 utilization is to design an efficient chemical process for conversion of captured CO2 to useful products. CO2 can participate in many chemical reactions that lead to useful products. Among these reaction processes is the dimethyl carbonate (DMC) synthesis.
DMC is an important raw material with versatile applications as a nontoxic substitute for toxic and corrosive agents such as dimethyl sulfate, dimethyl halides, and phosgene in methylation and carbonylation processes. In addition, phasing out methyl tert-butyl ether (MTBE) has led to consideration of DMC as an environmentally friendly, oxygenated fuel additive, i.e. octane enhancer, due to its high octane number, low toxicity, and quick biodegradabillity. DMC has an oxygen content three times that of MTBE (53 wt % vs. 18 wt %) so that on a weight basis only one third as much DMC is required to achieve the same oxygen level as MTBE.
DMC is a very good blending component, which has very high oxygen content (53 wt %) for environmental gasoline. Recently, automotive emission testing with DMC indicated that DMC is a more effective oxygenate than MTBE. DMC reduced total hydrocarbon and CO emission more than MTBE at the same weight percent of oxygen in the fuel. Therefore approximately 4.5 times less volume of DMC is required as compared to MTBE at the same weight percent oxygen in the fuel. Formaldehyde emission was also lower with DMC than with MTBE. DMC also exhibits good blending with octane.
DMC is classified as slightly toxic and is a more effective oxygenate than MTBE at the same weight percent oxygen in the fuel. In addition, DMC has a low emission of CO and NOx in automobile exhaust. The solubility of DMC in water is slight, whereas the solubility of MTBE is 4.3 wt %, which leads to MTBE accumulating in ground water.
Developing an environmentally friendly process and an effective catalyst is key for creating an economical and efficient technology for converting CO2 to DMC.
The DMC amount needed by a typical major refiner company to increase the oxygen content of its gasoline by 1 wt % is approximately 10,000 bbl/day. However, the total worldwide production capacity of DMC is estimated at about 1000 bbl/day.
Currently, DMC is primarily produced by oxidative carbonylation of methanol over CuCl. The main problems with this process are the low per-pass conversion, corrosion by chloride, and the presence of chloride in the DMC product. Another route for DMC production is oxidative carbonylation using nitric oxide. The major concern with this process is the use of nitric oxide. DMC can also be synthesized by (i) the reaction of methanol with phosgene, (ii) oxidative carbonylation of methanol by CO and O2 with the use of Cu and/or Pd catalysts, and (iii) co-production of DMC and ethylene glycol through the transesterification of ethylene carbonate with methanol. These routes use poisonous, flammable, and corrosive material such as phosgene, hydrogen chloride, carbon monoxide, and nitric oxide. Also, they carry potential explosion hazards.
An oxidative carbonylation process for producing DMC from CO2 and methanol has been developed. In this reaction route, a copper chloride catalyst system is used. The reaction is basically a redox system in which copper catalyst, as cuprous chloride, is oxidized by elemental oxygen, in the presence of methanol, to cupric methoxychloride, which is then reduced with carbon monoxide to form dimethyl carbonate and to restore the cuprous chloride. Both reactions take place simultaneously. The reactions of the process can be summarized as follows:




  
    
      
        
          
            2
            ⁢
            CuCl
          
          +
          
            2
            ⁢
            
              CH
              3
            
            ⁢
            OH
          
          +
          
            
              1
              2
            
            ⁢
            
              O
              2
            
          
        
        ->
        
          
            2
            ⁢
            
              Cu
              ⁡
              
                (
                
                  OCH
                  3
                
                )
              
            
            ⁢
            Cl
          
          +
          
            
              H
              2
            
            ⁢
            O
          
        
      
    
    
      
        (
        I
        )
      
    
  
  
    
      
        
          
            2
            ⁢
            
              Cu
              ⁡
              
                (
                
                  OCH
                  3
                
                )
              
            
            ⁢
            Cl
          
          +
          CO
        
        ->
        
          
            
              CH
              3
            
            ⁢
            
              OCOOCH
              3
            
          
          +
          
            2
            ⁢
            CuCl
          
        
      
    
    
      
        (
        II
        )
      
    
  




The overall reaction is:




  
    
      
        
          
            2
            ⁢
            
              CH
              3
            
            ⁢
            OH
          
          +
          CO
          +
          
            
              1
              2
            
            ⁢
            
              O
              2
            
          
        
        ->
        
          
            
              CH
              3
            
            ⁢
            
              OCOOCH
              3
            
          
          +
          
            
              H
              2
            
            ⁢
            O
          
        
      
    
    
      
        (
        III
        )
      
    
  




The process is believed to take place in a series of liquid-filled continuous stirred tank reactors, operating at approximately 393 K (120° C.) and a pressure of 27 atmospheres (2735 KN/m2). Since the oxygen is the limiting reagent, it must be fed at a carefully controlled rate. The maximum content of oxygen must not exceed 4 mol % at any point in the system to avoid the potential for explosion.

The main problems with this process are the low per-pass conversion, corrosion by chloride, and the presence of chloride in the DMC product.
A similar oxidative carbonylation route to the previous strategy has been developed. In this technology, nitric oxide (NO) is used as a redox coupling agent for the formation of dimethyl oxalate (DMO) and dimethyl carbonate (DMC). This technology has been developed and commercialized mainly to produce DMO. The DMO catalyst system was modified later to give high selectivity to DMC. A 4500 metric ton/year plant for DMC synthesis has been built. The reaction conditions of the process are in the range of 1-20 atmospheres and 323-423 K (50 to 150° C.), where the catalysts used were equimolar amounts of palladium chloride and a second metal chloride (Fe or Cu). These catalysts were co-impregnated on an active carbon support. The reactions of the process are thought to proceed as follows:
In a first step, methanol is reacted with oxygen and NO to form methyl nitrite (MN) and water:




  
    
      
        
          
            2
            ⁢
            
              CH
              3
            
            ⁢
            OH
          
          +
          
            2
            ⁢
            NO
          
          +
          
            
              1
              2
            
            ⁢
            
              O
              2
            
          
        
        ->
        
          
            2
            ⁢
            
              CH
              3
            
            ⁢
            ONO
          
          +
          
            
              H
              2
            
            ⁢
            O
          
        
      
    
    
      
        (
        IV
        )
      
    
  




In a second step, gaseous methyl nitrite reacts with a mole of carbon monoxide over the bimetallic catalyst to form DMC and restore the original NO:

2CH3ONO+CO→CH3OCOOCH3+2NO  (V)

The overall reaction is:




  
    
      
        
          
            2
            ⁢
            
              CH
              3
            
            ⁢
            OH
          
          +
          CO
          +
          
            
              1
              2
            
            ⁢
            
              O
              
                2
                ⁢
                
                  
                
              
            
          
        
        ->
        
          
            
              CH
              3
            
            ⁢
            
              OCOOCH
              3
            
          
          +
          
            
              H
              2
            
            ⁢
            O
          
        
      
    
    
      
        (
        VI
        )
      
    
  




This latter technology has particular advantages over the first noted strategy. A major advantage of the latter system lies in a dual reactor scheme, where the feed methanol and the water by-product never pass over the metal chloride catalyst. On the other hand, in the former system, water deactivation of the catalyst limits conversion to 15-20%. By separating the water from feed gas, the per pass conversion of the methyl nitrite can approach 100% without significant catalyst deactivation. Also, the latter process takes particular advantage of the fact that the redox reagent is a gas in both of its states as NO and CH3ONO. The similar species in the former process are solids, i.e. CuCl and Cu(OCH3)Cl. The simplicity of vapor/liquid separation compared to solid/liquid separation benefits the latter process. However, extreme care must be considered when mixing the three reactants (methanol, nitric oxide and oxygen) to stay outside the explosion limits of the reaction. Methyl nitrite is also highly reactive and must be handled with care. The use of the latter route also results in additional toxicity concerns due to the use of nitric oxide.
It is also known to form dimethyl carbonate (DMC) by a transesterification reaction between ethylene carbonate and methanol, with ethylene glycol as a co-product:

C2H4CO3+2CH3OH→CH3OCOOCH3+C2H4(OH)2  (VII)

It also is possible to produce DMC by the methanolysis of urea. The tin-catalyzed reaction of methanol with urea to give DMC is a well known synthesis. The reactions of the process can be illustrated as follows:

(NH2)2CO+CH3OH→H2NCOOCH3+NH3  (VIII)

H2NCOOCH3+CH3OH→CH3OCOOCH3+NH3  (IX)

The overall reaction can be presented as follows:

(NH2)2CO+2CH3OH→CH3OCOOCH3+2NH3  (X)

However, this reaction is not thermodynamically favorable as the ideal gas free energy change (ΔG) for this reaction is +3.2 kcal/mol at 373K (100° C.). The first methanolysis step (reaction VIII) to methyl carbamate is favored, but dimethyl carbonate (reaction IX) is not favored. Moreover, the chemistry is thermodynamically unfavorable and an additional driving force will be required in order to achieve reasonable conversion levels.

Two other technologies also have attractive possibilities for DMC production. These are: (i) the use of supported copper on carbon catalyst, which occurs in the gas phase and avoids the need for solid-liquid separation, but the catalyst deactivation is a major problem; and (ii) the alkylene carbonate routes which are attractive because they start with two relatively low cost materials, i.e. ethylene and carbon dioxide.
The direct synthesis of DMC starting from alcohols and carbon dioxide was studied since the 1980s. This route for DMC synthesis from inexpensive feedstocks such as CO2 and methanol (as shown below) is challenging:

2CH3OH+CO2→(CH3O)2CO+H2O  (XI)

It has been reported that DMC can be produced from CO2 and methanol in the presence of various catalysts, such as dialkylin dialkoxides, tin(IV), tetra-alkoxides, titanium(IV) tetra-alkoxides, bases, a mixture of palladium(II) chloride and copper(II) acetate, and thallium(I) hydroxide and alkali metal iodides. However, these reaction systems are homogeneous, which present three major problems: (a) difficulty in catalyst recovery, (b) reaction conditions of high pressure, and (c) rapid deactivation of the catalyst by process excursions.
Recently, catalytic DMC synthesis starting from carbon dioxide and methanol has been studied over zirconia (ZrO2) catalysts. The effectiveness of this catalyst was attributed to the presence of both acidic and basic sites. It was proposed that basic sites are required to activate methanol and CO2, and that acidic sites are required to supply methyl groups from methanol in the last step of the reaction mechanism. However, the selectivity and yield of this reaction was far from satisfactory.
Accordingly, a need exists for an improved process for producing dimethyl carbonate. Specifically, it would be desirable to provide an economical process for producing dimethyl carbonate from carbon dioxide and methanol, without the numerous problems associated with currently known strategies.
SUMMARY OF THE INVENTION
The difficulties and drawbacks associated with previously known reaction techniques and catalysts addressed in the present methods and catalysts.
In one aspect, the invention provides a method for producing dimethyl carbonate. The method comprises providing effective amounts of methanol and carbon dioxide to a reaction vessel. The method also provides reacting methanol and carbon dioxide in the presence of a heterogeneous catalyst in the reaction vessel to produce dimethyl carbonate.
In another aspect, the invention provides a method for producing dimethyl carbonate using a heterogeneous catalyst. The method comprises providing an effective amount of methanol to a reaction vessel. The method also comprises providing an effective amount of carbon dioxide to the reaction vessel. And, the method comprises reacting the methanol and the carbon dioxide in the presence of a heterogeneous catalyst to thereby produce dimethyl carbonate. The heterogeneous catalyst provides acidic reaction sites and basic reaction sites.
As will be realized, the invention is capable of other and different embodiments and its several details are capable of modifications in various respects, all without departing from the invention. Accordingly, the drawings and description are to be regarded as illustrative and not restrictive.



BRIEF DESCRIPTION OF THE DRAWINGS
FIGS. 1A-1D are SEM images of a catalyst system 5% Rh/Al2O3.
FIGS. 2A-2B are EDX spectra for 5% Rh/Al2O3.
FIGS. 3A-3D are SEM images of a catalyst system 5% Rh/Al2O3 (sol-gel).
FIGS. 4A-4B are EDX spectra for 5% Rh/Al2O3 (sol-gel).
FIGS. 5A-5D are SEM images of a catalyst system 5% Rh/SiO2.
FIG. 6 is an EDX spectrum of a particle in 5% Rh/SiO2.
FIG. 7A-7D are SEM images of a catalyst system of 5% Rh/ZSM-5.
FIG. 8 is an EDX spectrum of a particle in 5% Rh/ZSM-5.
FIGS. 9A-9D are SEM images of a catalyst system of 5% Rh-20% K/Al2O3.
FIG. 10 is an EDX spectrum of a particle in 5% Rh-20% K/Al2O3.
FIGS. 11A-11D are SEM images of a catalyst system of 52% Ni/Al2O3—SiO2.
FIGS. 12A-12D are SEM images of a catalyst system of 5% Mo2C/Al2O3.
FIG. 13 is an EDX spectrum of a particle in 5% Mo2C/Al2O3.
FIGS. 14A-14C are graphs illustrating the conversion of methanol, selectivity of DMC and formation rate of DMC, respectively, as a function of temperature using 5% Rh/Al2O3 catalyst.
FIGS. 15A-15C are graphs illustrating the conversion of methanol, selectivity of DMC, and formation rate of DMC, respectively, as a function of temperature using 5% Rh/Al2O3 (sol-gel) catalyst.
FIGS. 16A-16C are graphs illustrating the conversion of methanol, selectivity of DMC, and formation rate of DMC, respectively, as a function of temperature using 5% Rh/SiO2 (sol-gel) catalyst.
FIGS. 17A-17C are graphs illustrating the conversion of methanol, selectively of DMC, and formation rate of DMC, respectively, as a function of temperature using 5% Rh/ZSM-5 catalyst.
FIGS. 18A-18C are graphs illustrating the conversion of methanol, selectively of DMC, and formation rate of DMC, respectively, as a function of temperature using 5% Rh-20% K/Al2O3 catalyst.
FIGS. 19A-19C are graphs illustrating the conversion of methanol, selectively of DMC, and formation rate of DMC, respectively, as a function of temperature using 5% Rh-20% Ce/Al2O3 catalyst.
FIGS. 20A-20C are graphs illustrating the conversion of methanol, selectively of DMC, and formation rate of DMC, respectively, as a function of temperature using 5% Rh-20% Ni/ZSM-5 catalyst.
FIGS. 21A-21C are graphs illustrating the conversion of methanol, selectively of DMC, and formation rate of DMC, respectively, as a function of temperature using sol-gel catalyst.
FIGS. 22A-22C are graphs illustrating the conversion of methanol, selectivity of DMC, and formation rate of DMC, respectively, as a function of temperature using 5% Mo2C/Al2O3 catalyst.
FIGS. 23A-23B are graphs illustrating the conversion of methanol and the selectivity of DMC as a function of temperature using supported Mo2C catalysts.
FIGS. 24A-24B are graphs illustrating DMC formation rate over 5% Mo2C/Al2O3 for different catalyst weights and different reactant ratios.
FIGS. 25A-25B are graphs illustrating DMC decomposition over 5% Mo2C/Al2O3 at different temperatures.
FIGS. 26A-26B are graphs illustrating methanol conversion and DMC/DME selectivity over pure Mo2C.
FIGS. 27A-27B are graphs illustrating methanol conversion and DME selectively over pure Al2O3.
FIG. 28 is a graph of IR spectra of gaseous methanol, CO2, DMC, and DME.
FIG. 29 is a graph of MS intensity during methanol-CO2 TPR as a function of temperature.
FIG. 30 is a graph of IR spectra during methanol-CO2 TPR over Rh/Al2O3.
FIG. 31 is a graph of IR spectra during methanol TPR over Rh/Al2O3.
FIG. 32 is a graph of IR spectra during CO2 TPR over Rh/Al2O3.
FIG. 33 is a graph of IR spectra during DMC TPR over Rh/Al2O3.
FIG. 34 is a graph of IR spectra during a methanol-CO2 reaction over 5% Mo2C/Al2O3.
FIG. 35 is a graph of methanol conversion and DMC/DME selectivity during a methanol-CO reaction over 5% Rh/ZSM-5.
FIG. 36 is a graph of CO2 conversion and CO selectivity during CO2 decomposition over 5% Rh/ZSM-5.
FIGS. 37A-37B are schematic illustrations of two schemes for catalyst screening and activity studies, and TPR studies.



DETAILED DESCRIPTION OF THE EMBODIMENTS
Certain heterogeneous catalyst systems that provide both acidic sites and basic sites for various reaction species have been discovered which enable the production of dimethyl carbonate from methanol and carbon dioxide. The catalyst systems are typically supported, however the invention includes certain unsupported catalyst systems. The methods for forming dimethyl carbonate can be performed at relatively low temperatures. Although the present invention and its various and assorted preferred aspects are primarily described herein in terms of producing dimethyl carbonate, it will be appreciated that the invention may also encompass the production of other alkyl carbonates and thus, is not specifically limited to dimethyl carbonate.
It has also been surprisingly discovered that the removal of water produced as a by-product in the synthesis of dimethyl carbonate is a key to accomplishing a high conversion by shifting the equilibrium to dimethyl carbonate. Dehydration is successfully carried out by circulating the reaction mixture through a dehydrating tube packed with molecular sieve 3 Å. Under effective dehydrations, the DMC yield is almost linearly dependent on: reaction time, catalyst amount, methanol concentration, and CO2 pressure.
Methanol adsorption and dissociation also play an important role in the DMC synthesis from methanol and CO2. Adsorption and decomposition of methanol is likely influenced by the surface structure of the catalyst, i.e., structure-sensitive reaction. Numerous studies have suggested that the primary step in methanol dissociation is rupture of the O—H and C—O bonds. As a result, formation of methoxy species (CH3O) and other products has been reported. The methoxy species decomposes to carbon monoxide and hydrogen at higher temperatures. Although not wishing to be limited to any particular theory, it is believed that the presence of oxygen on the catalyst surface seems to promote CH3OH dissociation and formation of a methoxy species, which undergoes decomposition instead of associative desorption as CH3OH.
Investigations of methanol adsorption and decomposition have been performed on Cu/SiO2, ZrO2, and CuO/ZrO2. It has also been reported that methanol adsorption on Cu/SiO2 at 295K (22° C.) resulted in the formation of methoxy species on both Cu and SiO2. Heating the adsorbed species to 393 K (120° C.) led to the loss of methoxy species on Cu and the appearance of formate species on Cu. Further heating to 538 K (265° C.) produced gas-phase and adsorbed methyl formate, as well as CO2 and CO. It has also been shown that methanol decomposition on Cu/SiO2 produces adsorbed methoxy, formaldehyde, methylenebisoxy, and formate groups on Cu upon methanol adsorption at 303 K (30° C.). For zirconia, it was reported the appearance of methoxy species upon exposure to methanol at 298 K (25° C.). During temperature-programmed desorption of adsorbed methanol, CO, CH4, CH3OH, and CH2O peaks were observed at 453 K (180° C.). CO, CO2, CH4, H2, and H2O were observed at 773 K (500° C.), and additional CO and CO2 formation was observed at 863 K (590° C.). Methoxy decomposition was found to occur at 523-573 K (250 to 300° C.), with the formation of CO and CO2 at higher temperatures.
A bifunctional catalysis on CuO/ZrO2 has been observed during methanol adsorption and decomposition, where zirconia provides adsorption sites for reaction intermediates and Cu is proposed to facilitate the transfer and utilization of hydrogen. Methanol adsorption on CuO/ZrO2 and ZrO2 was shown to result in the formation of methoxy species on zirconia at 298 K (25° C.), which are converted to formate and carbonate species on zirconia and finally to gas-phase CO, CO2, H2, and H2O at higher temperatures. It was observed that the transformation of methoxy species to formate and carbonate species occurs at lower temperatures when Cu is present. The spillover of hydrogen from Cu was envisioned to restore OH groups on zirconia, which react with methoxy, resulting in formate and carbonate formation. In the absence of Cu, OH groups on zirconia are depleted, resulting in less efficient methoxy conversion.
In accordance with the present invention, various catalyst systems have been discovered for use in synthesizing dimethyl carbonate. Preferably, these catalyst systems are heterogeneous and provide both acidic sites and basic sites. The catalyst is preferably Rh, Rh—K, Ni, Mo2C, Pd, Pt, Re, MoO3, and combinations thereof. More specifically, these catalyst systems include, but are not limited to Rh-supported catalysts, Ni-supported catalysts, Pd-supported catalysts, Pt-supported catalysts, Re-supported catalysts, Mo2C-supported and unsupported catalysts, and MoO3-supported and unsupported catalysts.
A wide variety of supports can be used in the preferred catalysts. For example, the support can be one or more of SiO2, Al2O3, ZSM-5, V2O5, TiO2, ZrO2, and combinations thereof. In certain embodiments of the invention, the support is formed by a sol-gel method.
More specifically, it has been discovered that Rh/Al2O3, and Ni/SiO2—Al2O3 are active towards the DMC synthesis. In addition to Rh/Al2O3, and Ni/SiO2—Al2O3, the Mo2C/Al2O3 catalyst (proved to be successful in a coupling reaction) has been evaluated and was found to be active towards the DMC synthesis from methanol and CO2. Additional preferred catalyst systems in accordance with the invention include, but are not limited to Rh/Al2O3 (sol gel), Pd/Al2O3 (sol gel), Pt/Al2O3 (sol gel), Ni/Al2O3 (sol gel), Rh/SiO2, Rh/ZSM-5 and Rh—K/Al2O3. Moreover, additional preferred catalyst systems include, but are not limited to Pd/V2O5, Pd/TiO2, Pd/TiO2—V2O5, Pd/TiO2—ZrO2, Pt/Al2O3, Re/Al2O3, MoO3/Al2O3, MoO3/ZSM-5, and MoO3/SiO2.
The surface morphology and physical properties were examined for different catalyst samples that showed activity towards DMC synthesis from methanol and CO2. The surface area and pore size data are summarized in Table 1. A weak C peak was observed in almost all spectra and was not considered for compositional calculations. The SEM and EDX results are also summarized herein. Details as to various procedures and analytical techniques are set forth herein in the Examples section.
5% Rh/Al2O3 
FIGS. 1 and 2 show the SEM images and EDX spectra for 5% Rh/Al2O3 catalyst. Specifically, FIG. 1A is an SEM image of fresh 5% Rh/Al2O3 sample. FIG. 1B is an SEM image of used 5% Rh/Al2O3 sample. FIG. 1C is an SEM image of fresh 5% Rh/Al2O3 sample, illustrating a detailed view of a particle. FIG. 1D is a detailed view of used 5% Rh/Al2O3 sample. The sample showed very fine irregular and coarse semi-spherical particles with long fibers. The particle size range was <10 to 150 μm. The particle surface close up views showed that it was composed of compacted fine particles of irregular shape. FIG. 2A is an EDX spectrum of a particle in 5% Rh/Al2O3 used sample. FIG. 2B is an EDX spectrum of fibers in 5% Rh/Al2O3 used sample. EDX analysis of particles showed the presence of Al, O and Rh. EDX analysis of fibers showed the presence of elements consistent with glass. Al and O, are expected of an alumina sample. Minor concentrations of C and Clare also present. C is a common impurity found in alumina and is very difficult to remove. However, C will not affect Rh in such low concentrations.
5% Rh/Al2O3 (Sol Gel)
FIGS. 3 and 4 show the SEM images and EDX spectra for 5% Rh/Al2O3 (sol-gel) catalyst. Specifically, FIG. 3A is an SEM image of 5% Rh/Al2O3 (sol-gel). FIG. 3B is another SEM image of 5% Rh/Al2O3 (sol-gel). FIG. 3C is a detailed view of 5% Rh/Al2O3 (sol-gel) showing a particle and fiber. And, FIG. 3D is a detailed view of 5% Rh/Al2O3 (sol-gel) showing a particle. The catalyst showed very fine particles of irregular shape with high content of long fibers. The particle size range was <10 to 100 μm. The particle surface close up views showed the presence of fine particles and layer like structure especially in coarser particles. FIG. 4A is an EDX spectrum of a particle in 5% Rh/Al2O3 (sol-gel). FIG. 4B is an EDX spectrum of fibers in 5% Rh/Al2O3 (sol-gel). EDX analysis of fibers showed the presence of elements consistent with glass.







TABLE 1







Catalysts Characterization











BET Surface Area

CI


Sample
(m2/g)
Particle Size (Å)
wt (%)













5% Rh/Al2O3 (fresh)
135.5
247
1.2


5% Rh/Al2O3 (used)
140.3
131
0.0


5% Rh/Al2O3 (sol gel)
359.3
78.3
3.1


5% Rh/SiO2
277.4
91.4
2.9


5% Rh/ZSM-5
283.8
14.8
4.4


5% Rh—20% K/Al2O3
48.5
161.7
4.8


52% Ni/Al2O3—SiO2
228
96.9
NA


5% Mo2C/Al2O3
97.4
143.6
0.0









5% Rh/SiO2 

FIGS. 5 and 6 show the SEM images and EDX spectra for 5% Rh/SiO2 catalyst. Specifically, FIG. 5A is an SEM image of 5% Rh/SiO2. FIG. 5B is an SEM image of 5% Rh/SiO2. FIG. 5C is a detailed view of a particle in 5% Rh/SiO2, and, FIG. 5D is an SEM image of 5% Rh/SiO2 showing a single particle. The sample showed sharp edged particles of irregular shape with variable size. The particle size range was <10 to 500 μm. The particle surface close up views showed the presence of fine surface particles. FIG. 6 is an EDX spectrum of a particle in 5% Rh/SiO2. EDX analysis of particles showed the presence of Si, O, Cl and Rh.
5% Rh/ZSM-5
FIGS. 7 and 8 show the SEM images and EDX spectra for 5% Rh/ZSM-5 catalyst. Specifically, FIG. 7A is an SEM image of 5% Rh/ZSM-5. FIG. 7B is another SEM image of 5% Rh/ZSM-5. FIG. 7C is an SEM image of 5% RH/ZSM-5 illustrating a detailed view of particles, and, FIG. 7D is an SEM image of 5% Rh/ZSM-5 showing a detailed view of a single particle. The sample showed spherical and irregular round edged particles of variable size. The particle size range was <10 to 400 μm. The particle surface close up views showed the presence of high concentration of fine surface particles. FIG. 8 is an EDX spectrum of a particle in 5% Rh/ZSM-5. EDX analysis of particles showed the presence of Si, O, Al, Cl and Rh.
5% Rh-20% K/Al2O3 
FIGS. 9 and 10 show the SEM images and EDX spectra for 5% Rh-20% K/Al2O3 catalyst. Specifically, FIG. 9A is an SEM image of 5% Rh-20% K/Al2O3. FIG. 9B is an SEM imaging showing individual particles in 5% Rh-20% K/Al2O3. FIG. 9C is an SEM image showing a detailed view of particles in 5% Rh-20% K/Al2O3. And, FIG. 9D is an SEM image of a single particle in 5% Rh-20% K/Al2O3. The sample showed sharp edged particles of irregular shape having variable sizes. The particle size range was <10 to 500 μm. The particle surface close up views showed the presence of fine surface particles and cracks. FIG. 10 is an EDX spectrum of particles in 5% Rh-20% K/Al2O3. EDX analysis of particles showed the presence of Al, O, Cl and K.
52% Ni/Al2O3—SiO2 
FIG. 11 shows the SEM images for 52% Ni/Al2O3—SiO2 catalyst. Specifically, FIG. 11A is an SEM image of 52% Ni/Al2O3—SiO2. FIG. 11B is a detailed view of a particle in 52% Ni/Al2O3—SiO2. FIG. 11C is a further detailed view of a particle surface in 52% Ni/Al2O3—SiO2, and, FIG. 11D is an SEM image of 52% Ni/Al2O3—SiO2 further illustrating the particle surface. The sample was composed of sharp edged and irregular shaped particles having variable sizes. The close up views of individual particles showed that the particle surface contained agglomerated fine particles of variable sizes and shapes. The close up views of fine particles also showed the presence of similar morphology to that of coarser particles.
5% Mo2C/Al2O3 
FIGS. 12 and 13 show the SEM images and EDX spectra for 5% Mo2C/Al2O3 catalyst. Specifically, FIG. 12A is an SEM image of 5% Mo2C/Al2O3. FIG. 12B is another SEM image of 5% Mo2C/Al2O3. FIG. 12C is an SEM image of Mo2C/Al2O3 illustrating a detailed view of a particle. And, FIG. 12 is an SEM image of a particle and its surface in 5% Mo2C/Al2O3. The sample showed very fine particles of irregular shape with variable sizes. The particle size range was <10 to 250 μm. The particle surface close up views showed the presence of fine particles. FIG. 13 is an EDX spectrum of a particle in 5% Mo2C/Al2O3. EDX analysis of particles showed the presence of Al, O and Mo.
A series of activity studies were conducted, as follows.
Rh—Containing Catalysts
5% Rh/Al2O3 
FIGS. 14A-14C show the conversion of methanol, selectivity of DMC, and formation rate of DMC, respectively, as a function of temperature during the reaction of methanol-CO2 over 5% Rh/Al2O3 catalyst. The catalyst was prepared by incipient impregnation and had a surface area of 140.3 m2 and a pore volume of 0.92 cm3/g.
FIG. 14A shows that the conversion of methanol increases with temperature and that of CO2 was almost constant. The unchanged conversion of CO2 is due to its formation during the reaction. At 353 K (80° C.), the methanol conversion is as low as approximately 4%. With an increase in the temperature, the methanol conversion significantly rises from 14% to 95%, but at the same time undesirable reactions, i.e. decomposition of methanol, become dominant. A great quantity of CO appeared at 393 K (120° C.), which indicates that decomposition of methanol and CO2 promoted by H-containing compounds also occurs on the surface, thus hindering the DMC formation. The methanol conversion reaches a maximum (98%) at 553 K (280° C.). The increase in the methanol conversion was accompanied by a decrease in the DMC selectivity, an increase in that of dimethyl ether (DME), and an increase in the formation rate of DMC as shown in FIGS. 14B and 14C, respectively.
At temperatures higher than 400 K (127° C.), the DMC selectivity and yield was far from satisfactory. Weak acidity is very important in the selective DMC synthesis since the expectable by-product DME is easily formed on the rather strong acid sites. When DME is formed together with H2O, no DMC was observed due to the more favorable hydrolysis reaction of DMC.
Evidently, the results shown in FIGS. 14A-14C demonstrate that: (i) low temperature is more favorable for DMC formation and this is because the reaction is exothermic, (ii) DMC synthesis from methanol and CO2 is a reversible reaction, and (iii) DMC selectivity is limited by the equilibrium of (reaction XII), which shifts the reaction to the left to avoid the formation of water.

CH3OH+CO2→(CH3O)2CO+H2O  (XII)

Water produced during the reaction can react further with methanol to produce CO2 and H2 likely via the reforming reaction of methanol (reaction XIII).

CH2OH+H2O→CO2+3H2  (XIII)

Removal of water from the reaction system by circulating the reaction mixture through a dehydrating tube enhanced the methanol conversion and DMC selectivity at high temperatures. DMC decomposition and methanol dehydration to DME represents a major loss of the DMC selectivity.
5% Rh/Al2O3 (Sol-Gel)
FIGS. 15A-15C show the conversion of methanol, selectivity of DMC, and formation rate of DMC as a function of temperature during the reaction of methanol/CO2 over 5% Rh/Al2O3 (sol-gel) catalyst. The catalyst was prepared by sol-gel method and had a surface area of 359.3 m2 and a pore volume of 1.41 cm3/g. It was reported that an alumina support synthesized through a sol-gel method has superior properties, such as high purity and homogeneity at a molecular scale and well controlled acidic and basic sites.
The methanol conversion and DMC selectivity at low temperature were 15% and 100%, respectively. The DME formation escalated at 433 K (160° C.) while that of DMC was decreasing. The difference between this catalyst and that prepared by impregnation, i.e. FIGS. 14A to 14C, is the earlier formation of DME on Rh/Al2O3 (sol-gel) at 440 K (167° C.) (25 nmol/g·sec) as compared to 473 K (200° C.) over Rh/Al2O3.
5% Rh/SiO2 
FIGS. 16A-16C show the conversion of methanol, selectivity of DMC, and formation rate of DMC as a function of temperature during the reaction of methanol-CO2 over 5% Rh/SiO2 catalyst. The catalyst had a surface area of 277.4 m2. The methanol conversion decreases with temperature while DMC selectivity increased and reached 40% level at 393 K (120° C.). However, DME selectivity reached 100% at 473 K (200° C.).
5% Rh/ZSM-5
FIGS. 17A-17C show the conversion of methanol, selectivity of DMC, and formation rate of DMC as a function of temperature during the reaction of methanol/CO2 over 5% Rh/ZSM-5 catalyst. The catalyst had a surface area of 283.8 m2. The methanol conversion increased continuously and reached 98% at 473 K (200° C.). The highest DMC selectivity obtained was 63% at 393 K (120° C.) and that of DME was 62% in the range 433-513 K (160-240° C.) (as shown in FIG. 17B). The formation rate of DMC was 6 nmol/g·sec at 353-373 K (80-100° C.), while the DME formation rate was zero at 373 K (100° C.) (as shown in FIG. 17C).
5% Rh-20% K/Al2O3 
FIGS. 18A-18C show the conversion of methanol, selectivity of DMC, and formation rate of DMC as a function of temperature during the reaction of methanol/CO2 over 5% Rh-20% K/Al2O3 catalyst. The catalyst had a surface area of 48.5 m2. Addition of K as a promoter to Rh/Al2O3 catalyst had a negative effect on the methanol conversion and DMC selectivity. Similar effects occurred when Ce or Ni were added to Rh-supported catalysts (as shown in FIGS. 19 and 20). These effects were due to a decrease in the surface area (as shown in Table 1) and dilution of the Rh sites by K, Ce, or Ni. However, it will be appreciated that in certain applications, it may be desirable to incorporate one or more of these promoters in a heterogeneous catalyst.
Sol-Gel Catalysts
FIGS. 21A-21C show the conversion of methanol, selectivity of DMC, and formation rate of DMC as a function of temperature during the reaction of methanol-CO2 over catalysts prepared by sol-gel method. The results were similar to those catalysts of Rh prepared by wetness impregnation method where DMC was formed at a low temperature and methanol conversion. The methanol light-off temperature, i.e. the temperature at which 50% conversion was achieved, was Pd=407 K (134° C.), Pt=443 K (170° C.), Ni=466 K (193° C.) indicating that Pd was the most active catalyst as compared to Pt and Ni. The Pd catalyst shows better DMC selectivity (the DMC selectivity decreased in the following order: Pd>Pt>Ni). Ni catalyst showed high selectivity towards DME as compared to Pd and Pt. The sol-gel method was used to give well defined surface acidity/basicity. The surface area and pore volume were higher for those catalysts prepared by sol-gel method as compared to those prepared by an impregnation method.
Mo2-Containing Catalysts
5% Mo2C/Al2O3 
FIGS. 22A-22C show the conversion of methanol, selectivity of DMC, and formation rate of DMC as a function of temperature during the reaction of methanol-CO2 over 5% Mo2C/Al2O3 catalyst. The catalyst had a surface area of 97.4 m2. Over this catalyst, the DMC formed with a selectivity of 100% between 353 K (80° C.) and 393 K (120° C.), while on Rh/Al2O3 it was only 55% at 353 K (80° C.). On this catalyst, 433K (160° C.) proved to be the threshold temperature, where DME production is dominant as in the case of Rh. At higher temperatures (513 K (240° C.) to 553 K (280° C.)), hydrogen, CO, methane, and ethane were produced as a result of the decomposition of methanol and CO2.
FIGS. 23A-23B show the effect of support on the conversion of methanol and selectivity of DMC, as a function of temperature during the reaction of methanol-CO2 over supported Mo2C catalysts. It was found that DMC selectivity did not reach 100% even at 353-393 K (80-120° C.) on all supports with the exception of Al2O3 and ZSM-5. When ZrO2 and V2O5 were used as supports, DMC selectivity increased to a small extent with the rise of the temperature and was not accompanied by an increase in methanol conversion. The DMC yield (Y) was in the following order: YAl2O3=27, YSiO2=15.2, YV2O5=13.8, YZSM-5=11, YZrO2=4.7, YTiO2=2.4. This indicates that the support greatly affects the DMC selectivity through the stabilization of surface methoxy groups in the environment of adsorbed CO2.
FIGS. 24A-24B show the effects of catalyst weight and reactants ratio on the DMC formation rate during the reaction of methanol-CO2 over 5% Mo2C/Al2O3 catalyst at 393 K (120° C.). The rate of DMC formation decreased from 3.3 nmol/g·sec at 0.5 g to 0.9 nmol/g·sec at 2 g. This may indicate that on a relatively large quantity of the catalyst, the decomposition of DMC becomes more dominant. This is clearly demonstrated following the decomposition of DMC over 5% Mo2C/Al2O3 (FIGS. 25A-25B). It has been reported that the DMC decomposition is the main reason of the decrease of DMC formation at high temperature. The activation energy of DMC decomposition is lower than that of the reaction of methanol and CO2 at the given conditions.
In yet another series of investigations, conversion of methanol and formation and selectivity of DMC was investigated for various Pd-containing catalysts, Re-containing catalysts, and MoO3-containing catalysts. The results of these investigations are set forth below in Tables 2 to 11.







TABLE 2







DMC Formation Using 5% Pd/V2O5










Temperature
DMC Selectivity
DMC Formation rate
Methanol


(° C.)
(%)
[nmol/gsec]
conversion (%)













80
100
0.26
12.00


120
48
1.70
13.00


160
12
0.70
18.00


200
0
0
65.00


240
0
0
66


280
0
0
99
















TABLE 3







DMC Formation Using 5% Pd/TiO2










Temperature
DMC Selectivity
DMC Formation rate
Methanol


(° C.)
(%)
[nmol/gsec]
conversion (%)













80
100
0.56
9.00


120
4
0.33
11.00


160
0
0
20.00


200
0
0
68.00


240
0
0
98


280
0
0
99
















TABLE 4







DMC Formation Using 5% Pd/TiO2—V2O5











DMC





Selectivity
DMC Formation rate
Methanol


Temperature (° C.)
(%)
[nmol/gsec]
conversion (%)













80
76
0.7
2.00


120
0
0
4.00


160
0
0
21.00


200
0
0
70.00


240
0
0
96


280
0
0
98
















TABLE 5







DMC Formation Using 5% Pd/TiO2—ZrO2











DMC





Selectivity
DMC Formation rate
Methanol


Temperature (° C.)
(%)
[nmol/gsec]
conversion (%)













80
50
0.60
3.00


120
38
1.40
5.00


160
6
0.00
8.00


200
0
0
15.00


240
0
0
56


280
0
0
97
















TABLE 6







DMC Formation Using 5% Re/Al2O3










Temperature
DMC
DMC Formation rate
Methanol


(° C.)
Selectivity (%)
[nmol/gsec]
conversion (%)













80
35
0.60
11.00


120
100
1.40
13.00


160
3
0.00
16.00


200
0
0
81.00


240
0
0
92


280
0
0
97
















TABLE 7







DMC Formation Using 5% MoO3/Al2O3











DMC





Selectivity
DMC Formation rate
Methanol


Temperature (° C.)
(%)
[nmol/gsec]
conversion (%)













80
100
0.22
2.00


120
100
2.2
4.00


160
30
6
15.00


200
0.15
0.18
62.00


240
0
0
85


280
0
0
85
















TABLE 8







DMC Formation Using 5% MoO3/ZSM-5 (SiO2:Al2O3 = 30)











DMC





Selectivity
DMC Formation rate
Methanol


Temperature (° C.)
(%)
[nmol/gsec]
conversion (%)













80
0
0.00
7.00


120
7
1.50
8.00


160
0
0.00
82.00


200
0
0.00
87.00


240
0
0.00
88


280
0
0.00
99.7
















TABLE 9







DMC Formation Using 5% MoO3/SiO2











DMC





Selectivity
DMC Formation rate
Methanol


Temperature (° C.)
(%)
[nmol/gsec]
conversion (%)













80
100
0.26
11.00


120
100
8.00
12.00


160
96
26.00
14.00


200
42
13.00
22.00


240
7.6
2.40
34


280
1
0.80
54
















TABLE 10







DMC Formation Using 10% MoO3/SiO2











DMC





Selectivity
DMC Formation rate
Methanol


Temperature (° C.)
(%)
[nmol/gsec]
conversion (%)













80
100
0.36
12.00


120
100
10.00
13.00


160
92
30.00
22.00


200
30
9.00
28.00


240
3.3
1.60
40


280
0.45
0.35
61
















TABLE 11







DMC Formation Using 50% MoO3/SiO2











DMC





Selectivity
DMC Formation rate
Methanol


Temperature (° C.)
(%)
[nmol/gsec]
conversion (%)













80
100
0.30
12.00


120
100
6.00
13.00


160
95
22.00
18.00


200
34
13.00
35.00


240
11
8.00
51


280
4
2.00
62









While DME and CO2 were detected as the only DMC decomposition products, it may be concluded that the reaction on this catalyst takes place in a very similar way to the mechanism described for DMC synthesis over ZrO2 (shown below in reaction XIV). The effectiveness of ZrO2 was attributed to the presence of both acidic and basic sites. It was proposed that basic sites are required to activate methanol and CO2, and that acidic sites are required to supply methyl groups from methanol in the last step of the reaction mechanism. The evidence from infrared spectroscopy, suggests that methoxy species are formed during adsorption of methanol on basic sites and rapidly converted to methyl carbonate species. Accordingly, CO2 is activated and both oxygens of CO2 take part in the formation of the DMC.




Reaction XIV: Proposed Mechanism for DMC Synthesis Over ZrO2.
The results at different gas contents (FIG. 24B) demonstrate that DMC synthesis is affected by gas contents only to a small extent. The number of methoxy and activated CO2 groups forming on the surface is the determining factor in the DMC formation.
In the case of pure Mo2C (FIGS. 26A-26B), the results obtained were similar to those for 5% Mo2C/Al2O3. The 100% DMC selectivity measured at the beginning of the reaction at 353 K (80° C.) (methanol conversion=2.7%) had decreased with temperature. Unlike the case of a supported catalyst, products from the decomposition of methanol (methane, formaldehyde) were detected at 393 K (120° C.). With a further increase of temperature, CO produced from the decomposition of CO2 and methanol was also observed. From this it can be concluded that the support plays an important role in stabilizing and providing the surface with adsorbed methoxy group. This idea is also backed by the measurement taken on the Al2O3 support (FIGS. 27A-27B). At low temperatures (353-393 K) (80-120° C.), no product was detected on the support. With an increase in temperature (433-553 K) (160-280° C.), the decomposition products (hydrogen, CO, DME) appeared with DME as the favored product.
TPR of Methanol/CO2 
5% Rh/Al2O3 
FIG. 28 shows the IR spectra of gaseous methanol, CO2, DMC, and dimethyl ether (DME). The IR spectra show different IR features for each component, which were used to discern the overlapping of adsorbates with gaseous species during the DMC synthesis from methanol and CO2.
FIG. 29 shows the MS intensity of the effluent from the IR reactor during the methanol-CO2 TPR as a function of temperature. FIG. 29 shows that the decrease in methanol MS intensity was accompanied by an increase (formation) in that of DMC and CO2. The formation of DMC reached a maximum at 541 K (268° C.). Above 541 K (268° C.), the CO2 MS intensity continues to increase while those of methanol and DMC decreased. The decay in the MS intensity of DMC could be due to (i) thermodynamics or (ii) deactivation of the catalyst by water. Although both factors are important, the former is more notable. The dissociation and reaction of methanol caused a decrease in its MS intensity.
FIG. 30 shows the IR spectra of adsorbates during the methanol/CO2 TPR as a function of temperature. The IR spectra of adsorbed methanol and CO2 at 303 K (30° C.) show broad bands centered at 3596, 2945, and 2350 cm−1 due to O—H, C—H in CH3O (methoxy species), and CO2, respectively. Increasing the temperature to 363 K (90° C.) resulted in appearance of bands at 2049 and 1921 cm−1. The bands centered at 2148, 1648, 1589, and 1450 cm−1 appeared at 463 K (190° C.). The bands at 1450 and 1589 cm−1 were assigned to C—H in CH3O (methoxy species) and OCO (formate), respectively. The appearance of bands at 2049 and 2148 cm−1 was due to the formation of adsorbed CO on reduced Rh sites in a linear mod(Rh—C≡0) and gaseous CO, respectively. The band at 1648 cm−1 can be assigned to the methoxy carbonate species (CH3OCOO-M). The methoxy carbonate species on the surface of alumina was previously observed. It has been reported that the methoxy carbonate species was formed by the reaction between adsorbed methoxy species and CO2 more easily than by the reaction between adsorbed CO2 and methanol. This is probably because methanol can desorb CO2 that adsorbed on the surface.
Formation of linear CO and gaseous CO indicates that methanol and/or CO2 was dissociated over Rh surface. Spectroscopic studies on supported catalysts have shown that methanol dissociated to form linear CO, CO(g), and CO2(g), whereas CO2 exhibited no evidence for its dissociation.
In order to elucidate the mechanism of the formation of linear CO, CO(g), and CO2(g), separate TPR experiments for methanol, CO2, and DMC (FIGS. 31 to 33, respectively) were carried out. The IR spectra during the methanol TPR (FIG. 31) shows that linear CO and CO(g) appeared at 443 K (170° C.), and the appearance of CO2(g) started at 603 K (330° C.). Similarly, the TPR of DMC (FIG. 33) shows that linear CO (see the difference spectra presented in the inset in FIG. 32), CO(g), and CO2(g) were formed.
The CO2 TPR (FIG. 32) shows no IR evidence of linear CO and CO(g). Absence of linear CO and CO(g) during the CO2 TPR are in agreement with the results of CO2 adsorption on various catalysts. It was reported that CO2 dissociation enhanced only in the presence of adsorbed hydrogen. The following mechanism is valid for the formation of linear CO, CO(g), and CO2 during the methanol dissociation in the present study:

CH3OH(g)→CH3OHads  (XV)

CH3OHads→CH3OadsHads  (XVI)

CH3Oads→COads+3Hads  (XVII)

COads→CO(g)  (XVIII)

COads+OHads→CO2(ads)+Hads  (XIX)

CO2(ads)→CO2(g)  (XX)

Reaction Mechanism

FIG. 34 shows the IR spectra during methanol-CO2 reaction over 5% Mo2C/Al2O3 catalyst at 393 K (120° C.). The IR spectrum of gaseous DMC was included to elucidate the DMC formation. Introduction of methanol-CO2 (2:1, 12 cm3/min) resulted in appearance of gaseous methanol centered at 2888, 2061, 1036 cm−1 and CO2 centered at 2345 cm−1. After 3 min, new bands at 1742 cm−1 appeared due to gaseous DMC and 1596 and 1484, 1458 cm−1 due to methoxy carbonate species. The intensity of the band 1742 cm−1 increased with time and reached a maximum at 21 minutes. The decrease in the IR intensity of the 1742 cm−1 band was accompanied by emergence of a gaseous CO band centered at 2138 cm−1 and an increase the IR intensity of methoxy carbonate species at 1458 cm−1.
In the direct synthesis of DMC from methanol and CO2, it is important to activate methanol and CO2 by basic sites and to supply the methyl species from methanol by acidic site as follows:

CH3OH→CH3O−(ads)+H+(ads)(Basic site)  (XXI)

CO2→CO2(ads)(Basic site)  (XXII)

CH3O−(ads)+CO2(ads)→CH3OCO−(ads)(Basic site)  (XXIII)

CH3OH→CH3+(abs)+OH−(abs)(Acidic site)  (XXIV)

CH3OCO−2(ads)+CH3+(ads)→(CH3O)2CO  (XXV)

H+(ads)+OH−(ads)→H2O  (XXVI)

It is believed that the initial adsorption of CH3OH on catalyst surface occurs via the interaction of the O atom of CH3OH with a coordinately unsaturated Lewis acid center on the surface, which results in the formation of methoxy species. This process led to disappearance of surface OH groups and release of water.
DMC could be formed via: (i) insertion of adsorbed CO into two methoxy species or (ii) reaction of adsorbed CO2 with methoxy species to form methoxy carbonate (reaction XXIII), which then reacts with methyl species (reaction XXV). It is believed that methoxy carbonate species are formed predominantly via CO2 addition to methoxy species when CH3OH and CO2 are passed concomitantly over the catalyst. To clarify this issue, the methanol-CO reaction was performed, during which DMC was not formed (FIG. 35). This suggests that insertion of adsorbed CO into two methoxy species to form DMC does not occur. The low conversion of CO2 during its decomposition (FIG. 36) indicates that CO2 participates in the reaction without dissociation into adsorbed CO and adsorbed O, which support the occurrence of reaction XXIII. The reaction of adsorbed CO2 with methoxy species was supported by IR evidence and methanol-CO2 reaction over different catalysts and support.
The CO2 insertion into the M-OCH3 bonds (reaction XXIII) has been reported for methoxy-containing complexes based on Mg or Ca. It has been proposed that the first step in the insertion of CO2 into a M-OCH3 bond involves an electron donor-acceptor interaction in which the alkoxy oxygen lone pairs act as the donor and the CO2 carbon atom as the acceptor.
Conclusions
In this work, DMC synthesis was studied using a vapor phase flow reactor system in the presence of various catalysts. The effects of reaction conditions, promoters, and method of preparation on the catalyst performance were evaluated in terms of methanol conversion and DMC selectivity.
The following conclusions are apparent from the results of the present work.
Low temperatures, e.g. 353-433 K (80-160° C.), are favorable for DMC formation. However, DMC can generally be produced at a temperature within the range of from about 80° to about 280° C.
Among the various catalysts employed, Rh—, and Mo2C— supported catalysts showed the best catalytic performance in the DMC synthesis.
The Temperature-Programmed Reaction (TPR) showed that methanol was dissociated into methoxy species and linear CO.
Adsorbed methoxy species and the activated CO2 play an important role in the DMC synthesis and their population is the determining factor in DMC formation.
The effectiveness of any catalyst for DMC synthesis is attributed to the presence of both acidic and basic sites. Basic sites are required to activate methanol and CO2, and acidic sites are required to supply methyl groups from methanol in the last step of the reaction mechanism.
DMC forms via reaction of adsorbed CO2 with methoxy species to form methoxy carbonate ((CH3O)CO2 (active adsorbate), which then reacts with methyl species to form DMC.
DMC formation is a reversible process, which became less pronounced with the increase of temperature.
As far as DMC yield is concerned, the Al2O3 support was the most effective in the case of Mo2C catalyst.
The reason for inferiority of certain catalysts prepared by a sol-gel method could be due to the presence of water in the reaction system and not to the absence of well controlled acidic and basic sites.
Loss of surface chloride was the reason of the catalyst system deactivation in the DMC synthesis.
Removal of water is necessary to shift the reaction toward the DMC formation.
The preferred methods for producing DMC can be carried out in a flow system, i.e. a continuous or semi-continuous system. Preferably, the methods are performed at pressures of from about 0.9 atmospheres to about 1.5 atmospheres. In certain embodiments, the methods are performed at about 1 atmosphere pressure.
EXAMPLES
Catalyst Preparation
Two methods of catalyst preparation were used in the present work:
Impregnation Method
Impregnation is an important and widely used method in preparing catalysts. It is the simplest method of producing catalyst. It allows an accurate adjustment of salt, and the active components/support ratio.
Impregnation is achieved by filling the pores of a support with a solution of a metal salt from which the solvent is subsequently evaporated. The technique can be classified as dry or wet impregnation based on the initial state of the support.
Sol-Gel Method
The sol-gel process is a technique for the preparation and fabrication of inorganic oxides of extremely high purity and homogeneity. The word sol implies a dispersion of colloidal in a liquid. Colloids are in turn described as solid particles with dimensions in the range of 10 to 1000 Å, each with from about 103 to about 109 atoms. When the viscosity of a sol increases sufficiently, usually by the loss of its liquid phase and or polymerization of the solid particles, it becomes a porous solid body, which is termed a gel.
Rh-, Pd-, Pt-Supported Catalysts
The Rh-, Pd-, Pt-containing catalysts with different promoters, e.g., Ce, K, Ni, were prepared by incipient wetness impregnation onto Al2O3, SiO2, ZrO2, V2O5, TiO2, ZSM-5 or carbon. The catalyst was dried overnight in air at room temperature and calcined by flowing air at 673 K (400° C.) for 3 hours and then reduced by flowing H2 at 673 K (400° C.) for 3 hours.
MoO3 and Mo2C-Supported Catalysts
MoO3-containing catalysts were prepared by impregnating Al2O3, SiO2, ZrO2, V2O5, TiO2, or ZSM-5 (Sigma-Aldrich Chemicals) with a basic solution of ammonium heptamolybdate to yield different weight percentage of MoO3 (Sigma-Aldrich Chemicals). The suspension was dried at 373 K (100° C.) and calcined at 863 K (590° C.) for 5 hours.
Supported Mo2C catalysts were prepared by the carburization of calcined the supported MoO3 catalysts by ethane. MoO3-containing samples were heated under 10% (v/v) C2H6/H2, from room temperature to 900 K (627° C.) at a heating rate of 0.8 K min−1. After preparation, the catalysts were cooled down to room temperature under argon. The carbides were passivated in flowing 1% O2/Ar at 300 K (27° C.). Before the catalytic experiments, the samples were treated with H2 at 873 K (600° C.) for 1 hour to remove any excess carbon.
Catalysts Prepared by Sol-Gel Method
Alumina is formed through preparing hydrolyzed aluminum precursors, where stirring and pH control affect the properties. The synthesis step is followed by aging, solvent washing, drying and dehydration. The Rh/Al2O3, Pt/Al2O3, Pd/Al2O3, and Ni/Al2O3 samples were prepared and denoted as Rh/, Pd/, Pt/, Ni/Al2O3 (sol-gel). 13.5 g from aluminum tri-sec-butoxde (ASB) (from Sigma-Aldrich Chemicals) was dissolved in 73.3 g of 2-butanol (from Scharlau Chemicals). The mixture was continuously stirred till the ASB dissolved completely (designated as solution 1). The chloride form of Rh, Pd, Pt, or Ni (Sigma-Aldrich Chemicals of Barcelona, Spain) was dissolved in water and mixed with solution 1 for 1 hour. The sample was covered and allowed to be in open air for 24 h at room temperature before it was dried at 353 K (80° C.) for 24 hours. Before any experiment, the catalyst sample was calcined at 823 K (550° C.) and reduced at 673 K (400° C.)
Catalyst Characterization
Scanning Electron Microscopy (SEM)
SEM provides direct topographical images of the solid structure, which are formed by back-scattered primary electrons. In this method, the overall contrast is due to differential absorption of photons or particle (amplitude contrast) and more importantly diffraction phenomena (phase contrast). SEM can provide magnification powers of greater than three hundred thousand. Powdered samples were attached to 12.5 mm diameter aluminum stubs via double sticking 12 mm diameter carbon tabs. The particles were viewed by SEM (Cambridge S360 from Cambridge Scientific Instruments Co. of the UK) operated at the following settings: Accelerating Voltage=20 kV, Working Distance=15 mm, and Image Resolution: Ultrafine. The images were recorded in secondary electron imaging mode (SE) at different magnifications.
Energy Dispersive X-ray Spectroscopy (EDX)
SEM-EDX was used for elemental analysis of the catalyst to investigate the presence of any impurities or contaminants that might adversely affect the catalyst. Multiple particles were analyzed for elemental composition by EDX (Oxford ISIS300, Instrument ID: EDX-1) attached to SEM. EDX analysis was performed on flat regions (where possible) in area mode at settings: Accelerating Voltage=20 kV and Working Distance=25 mm. The elemental composition of metals was estimated by EDX system software and pure metal standard spectra.
Surface Area, Pore Volume, and Pore Size
The physical properties of the catalysts (i.e., surface area, pore volume, and pore size) were determined by Quantachrome Autosorb automated gas adsorption system using nitrogen gas.
Experimental System
The experimental system shown in FIGS. 37A-37B included (i) a gas flow section with a 4-port switching valve and 6-port pulsing valve, (ii) an in situ IR reactor with/without catalyst, and (iii) an analysis section.
Analysis Section
The analysis section included an IR spectrometer to measure the adsorption intensity and vibrational frequency (wavenumber, cm−1) of adsorbed and gaseous species on the catalyst surface, a gas chromatograph to measure the steady-state gas phase concentrations of the effluent, and a mass spectrometer to measure the transient effluent concentrations of gaseous products. The flow rates of the gasses were controlled by mass flow controllers (Omega 750 from Omega of Stamford, Conn.).
Infrared Spectrometer
The effluent gases from the reactor were sent to an environmental chamber (IR reactor cell) placed in the FTIR compartment. The steady-state and transient IR spectra were collected by a Thermo Nicolet Nexus 670 FTIR spectrometer equipped with a MCT detector that was cooled with liquid nitrogen. A high pressure/high temperature chamber (see FIGS. 37A-37B) fitted with ZnSe windows, was utilized as an IR reactor cell for in situ reaction studies. The IR reactor cell was heated by a temperature controller. The lines from the bubbler to the IR reactor were wrapped with heating tape and insulated with general purpose insulating wrap. For steady-state spectra, 64 scans were co-added at a resolution of 4 cm−1. Co-adding a large number of scans increased the signal to noise ratio (S/N), but required longer sampling time, resulting in the loss of the transient information.
Gas Chromatograph
The effluent gases of the IR reactor cell were sent to a Varian CP-3800 gas chromatograph (GC) for determination of the steady-state effluent concentrations of methanol, CO2, and DMC. The gas chromatograph contained a thermal conductivity detector (TCD) and flame ionization detector (FID).
Mass Spectrometer
The effluent gases of the IR reactor cell were also sent to the mass spectrometer PRISMA QMS-200 M quadruple with a continuous secondary electron multiplier (SEM). Careful selection of the mass/charge (m/e) signals for the gaseous products is required to prevent overlapping of the responses. Prior to the investigation, Helium was used to purge the sampling line. A four-port valve allowed for an efficient switch from Helium to the reactor effluent. Helium was fed to the 1⁄8 inch sampling line to prevent air from entering the mass spectrometer and oxidizing the filament when the mass spectrometer sampling valve is open for uptaking the sample gases. The gaseous stream from the 1⁄8 inch line entered a capillary line that is 2 mm OD and 0.15 mm ID, and then a two-stage differentially pumped gas inlet system (Balzers GES-010) for continuously drawing the gas sample into a medium vacuum of approximately 0.7 mbar by a rotary vane pump. The valve to the mass spectrometer vacuum chamber had an aperture that allowed about 2% of the gas in the medium vacuum to enter. After entering through the sampling valve, the sample gas was transported to the quadruple analyzer. Data acquisition was conducted by the QUADSTAR-522 software package for collection of mass spectrometric data. This program allows for the measurement of up to 200 m/e ratios as a function of time. The gaseous MS responses for m/e ratios corresponding to methanol (m/e=29, 31, 32), CO2 (m/e=44, 22, 28), and DMC (m/e=45, 59, 90) were monitored.
Catalysts Screening and Testing
FIG. 37A shows the schematic used in the catalyst screening and testing. A 500 mg of catalyst was loaded into a tubular reactor (I.D. of 8 mm) inside a GC furnace, and reduced with H2 or calcined with air depending on the nature of catalyst. A total of 12 cm3/min of CO2/He (1:9 cm3/min) was passed through a bubbler containing methanol and sent to the reactor. The reaction was carried out at 363 K (90° C.), 383 K (110° C.), 403 K (130° C.), to 573 K (300° C.) for 40 minutes at each temperature level. The effluent of reactor was sent to the empty IR reactor cell and the GC to determine the amount of DMC. The selectivity for reaction products, Si and Formation molar flow rate of DMC were defined as:



  
    
      Selectivity
      ⁢
      
        
      
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The Temperature-Programmed Reaction (TPR) Studies

The TPR is a useful technique to scan a wide range of temperatures under which a reaction may take place. It may also provide information about active adsorbate(s) that participate in the reaction and spectator adsorbate.
FIG. 37B shows the schematic used in the TPR studies. The catalyst powder (40 mg) was placed into the IR reactor cell, and an additional catalyst (160 mg) was placed into a tubular reactor to increase the reactant conversion and product formation for GC and MS measurements. A total of 12 cm3/min of CO2/He (1:9 cm3/min) was passed through a bubbler containing methanol and sent to the IR reactor with catalyst.
Prior to TPR, the catalyst was reduced by H2 at 673 K (400° C.) for 2 hours and IR background spectra were collected while the catalyst was cooled in He flow from 673 K (400° C.) to 303 K (30° C.). CO2 and He were flowed into a methanol bubbler then to the reactor. The effluent of reactor was sent to the GC and the MS. Upon the MS intensities of gaseous species becoming constant, the temperature was increased from 303 K (30° C.) to 673 K (400° C.) at 8 K/minute. The background spectra were subtracted from IR spectra collected during the TPR.
Many other benefits will no doubt become apparent from future application and development of this technology.
All patents, published applications, and articles noted herein are hereby incorporated by reference in their entirety.
It will be understood that any one or more feature or component of one embodiment described herein can be combined with one or more other features or components of another embodiment. Thus, the present invention includes any and all combinations of components or features of the embodiments described herein.
As described hereinabove, the present invention solves many problems associated with previously known catalysts and methodologies. However, it will be appreciated that various changes in the details, materials and arrangements of parts, which have been herein described and illustrated in order to explain the nature of the invention, may be made by those skilled in the art without departing from the principle and scope of the invention, as expressed in the appended claims.

## Claims

1. A method for producing dimethyl carbonate, the method comprising:
providing effective amounts of methanol and carbon dioxide to a reaction vessel;
reacting methanol and carbon dioxide at atmospheric pressure in the presence of a heterogeneous catalyst in the reaction vessel to produce dimethyl carbonate;
wherein the heterogeneous catalyst is selected from the group consisting of Pd/Al2O3, Pt/Al2O3, Ni/Al2O3, Ni/SiO2—Al2O3, Mo2C/Al2O3, Pd/V2O5, Pd/TiO2, Pd/TiO2—V2O5, Pd/TiO2—ZrO2, Pt/Al2O3, Re/Al2O3, MoO3/Al2O3, MoO3/ZSM-5, and MoO3/SiO2.

2. The method of claim 1, wherein the support of the catalyst is formed by a sol-gel method.

3. The method of claim 1 wherein the reaction is performed at a temperature of from about 80° to about 280° C.

4. The method of claim 1 wherein water is produced as a by-product in the production of dimethyl carbonate, the method further comprising:
removing at least a portion of the water to thereby increase production of dimethyl carbonate.

5. The method of claim 4 wherein the removing at least a portion of the water is performed by circulating a reaction mixture through a dehydrating tube.

6. A method for producing dimethyl carbonate using a heterogeneous catalyst, the method comprising:
providing an effective amount of methanol to a reaction vessel;
providing an effective amount of carbon dioxide to the reaction vessel;
reacting the methanol and the carbon dioxide at atmospheric pressure in the presence of a heterogeneous catalyst to thereby produce dimethyl carbonate;
wherein the heterogeneous catalyst provides acidic reaction sites and basic reaction sites; and
wherein the heterogeneous catalyst is selected from the group consisting of Pd/Al2O3, Pt/Al2O3, Ni/Al2O3, Ni/SiO2—Al2O3, Mo2C/Al2O3, Pd/V2O5, Pd/TiO2, Pd/TiO2—V2O5, Pd/TiO2—ZrO2, Pt/Al2O3, Re/Al2O3, MoO3/Al2O3, MoO3/ZSM-5, and MoO3/SiO2.

7. The method of claim 6 wherein the support of the catalyst is formed by a sol-gel method.

8. The method of claim 6 wherein the reaction is performed at a temperature of from about 80° to about 280° C.

9. The method of claim 6 wherein water is produced as a by-product in the production of dimethyl carbonate, the method further comprising:
removing at least a portion of the water to thereby increase production of dimethyl carbonate.

10. The method of claim 9 wherein the removing at least a portion of the water is performed by circulating a reaction mixture through a dehydrating tube.

11. A method for producing dimethyl carbonate, the method comprising:
providing effective amounts of methanol and carbon dioxide to a reaction vessel;
reacting methanol and carbon dioxide at atmospheric pressure in the presence of a heterogeneous catalyst in the reaction vessel to produce dimethyl carbonate, wherein the heterogeneous catalyst includes a catalyst and a support, and the heterogeneous catalyst is selected from the group consisting of Pd/Al2O3, Pt/Al2O3, Ni/Al2O3, Ni/SiO2—Al2O3, Mo2C/Al2O3, Pd/V2O5, Pd/TiO2, Pd/TiO2—V2O5, Pd/TiO2—ZrO2, Pt/Al2O3, Re/Al2O3, MoO3/Al2O3, MoO3/ZSM-5, and MoO3/SiO2.