年產(chǎn)1.5萬噸碳酸二甲酯化工廠的設(shè)計(jì)

年產(chǎn)1.5萬噸碳酸二甲酯化工廠的設(shè)計(jì),年產(chǎn)1.5萬噸碳酸二甲酯化工廠的設(shè)計(jì),年產(chǎn),碳酸,二甲,酯化,工廠,設(shè)計(jì) Synthesis of Dimethyl Carbonate from Methyl Carbamate and Methanol with Zinc Compounds as Catalysts Wenbo Zhao, , Feng Wang, , Weicai Peng, , Ning Zhao, Junping Li, Fukui Xiao, Wei Wei,* , and Yuhan Sun* , State Key Laboratory of Coal ConVersion, Institute of Coal Chemistry, Chinese Academy of Sciences, Taiyuan 030001, Peoples Republic of China, and Graduate UniVersity of Chinese Academy of Sciences, Beijing 100039, Peoples Republic of China Various zinc compounds were used as the catalysts for the synthesis of dimethyl carbonate (DMC) from methyl carbamate (MC) and methanol in a batch reactor. Among them, ZnCl 2 showed the highest catalytic activity and led to the DMC yield of 33.6% under the optimal conditions. In addition, a possible reaction mechanism was proposed based on Fourier transform infrared (FTIR) and X-ray diffraction (XRD) characterization results. 1. Introduction Dimethyl carbonate (DMC) as an environmentally benign building block has attracted much attention in recent years. 15 It can replace phosgene, dimethyl sulfate, chloromethane, and methyl chloroformate as carbonylation, methylation, esterifi- cation or, ester interchange reagent, and it can also be used as additive for gasoline, flavoring agent of foodstuff, electronic chemical, etc. Thus, the effective synthesis of DMC becomes more and more important. The current processes reported mainly include phosgenation of methanol, oxidative carbonylation of methanol, ester exchange, and esterification of carbon dioxide with methanol, which all suffer from the corresponding short- comings such as being poisonous, being easily explosive, having a complex reaction course, and having extremely low conversion. Recently, a new route of the DMC synthesis from urea and methanol has been developed for low-cost and facile separation of production. 6 In this synthesis approach, the intermediate methyl carbamate (MC) is produced first and further converted to DMC by reaction with methanol. The first step of the reaction is fast and highly selective even without catalysts, because urea can decompose easily to ammonia and isocyanic acid. The latter, as an active intermediate, can further react with solvent methanol to produce MC. However, the second step of the reaction, MC to DMC, is more difficult than the first step. 79 The ammonia accumulated in the first step will restrict the shift of the reaction equilibrium to DMC, since it is also the byproduct of the second step. Consequently, dividing this reaction into two isolated steps will be a more promising approach toward the synthesis of DMC. The key to the two-step technics is to effectively promote the second reaction, which is the rate-control step for the reaction of urea methanolysis, with proper catalyst. A lot of catalysts such as bases, organic tin, metal oxide, and zinc compounds have been tested in a batch reactor toward the direct reaction of urea and methanol or its analogues. 1018 However, as to the isolated second reaction, only a few studies have been reported about the exploitation of catalyst up to now. In this regard, organic tin compound was considered as a favorable catalyst for this reaction in previous literature, but it was not promising from the viewpoint of the environment because of its strong toxicity. 19 Our group found that CaO was the best one among solid base catalysts tested since it activated methanol effectively with its strongest basicity, but the DMC yield on it was still far from satisfactory. 7 In this work, the synthesis of DMC from MC and methanol was investigated over many zinc compound catalysts in a batch reactor. Furthermore, the reaction conditions were explored in detail with ZnCl 2 as the model catalyst for its excellent catalytic performance. 2. Experimental Section 2.1. Preparation of Catalyst. Zn(CH 3 COO) 2 and Zn(NO 3 ) 2 were obtained by evacuating Zn(CH 3 COO) 2 2H 2 Oat110C for 20 h and Zn(NO 3 ) 2 6H 2 O at 115 C for 24 h, respectively. Other chemicals and catalysts were commercial analytic reagents without further purification. 2.2. Catalytic Reaction. The reaction was conducted in a 350 mL stainless steel autoclave reactor equipped with electric heating, a reflux column, and a magnetic stirrer under the assigned conditions. In a typical process, 0.1 mol of MC, 2.0 mol of methanol, and 7.4 mmol of catalyst were put into autoclave first and then were rapidly heated to the desired temperature and kept for a certain time with magnetic stirring. The stirring speed was 600 ( 50 rpm, and the temperature error was 1.00 g. The effect of reaction temperature is illustrated by Figure 4. The conversion of MC was consistently enhanced with the increase of temperature, but the DMC yield reached its peak at 190 C and then decreased. In theory, the high temperature was appropriate for synthesis of DMC, since this reaction was an endothermic reaction. 20 However, higher temperature also shortened the time needed to reach the maximum DMC concentration and accelerated the rate of further reaction. Accordingly, although byproduct NMMC could not be detected at 170 C, as the temperature increased, its yield increased significantly at the cost of DMC consumption. Simultaneously, the thermal decomposition of DMC may aggravate gradually. Therefore, the suitable reaction temperature should be controlled below 190 C. Figure 5 demonstrates the effect of reaction time. The DMC yield increased at the first 10 h and reached its maximum of 33.6%, and then the consumption of DMC in the further reaction surpassed gradually the formation of DMC from MC. Thus, 10 h was the optimal reaction time for the reaction of MC with methanol. The detailed reaction kinetics for these three experi- mental factors still awaits further exploration. 3.4. Possible Mechanism. As a transition metal element, divalent Zn 2+ ion with d 10 electrons could coordinate with nitrogen, oxygen, and sulfur or phosphorus atom to reach the stable construction of 18 electrons. 2830 Thus, the nitrogen atom of amino and the two oxygen atoms of carbonyl and methoxy in the MC molecule all had a chance to coordinate with Zn 2+ ion. Their electron densities computed by Hyperchem7.5 based on AM1 semiempirical method were -0.416, -0.404, and -0.286 of negative charge, respectively. This meant that the nitrogen atom was more possible than the oxygen atom to coordinate with Zn 2+ ion. Furthermore, the hybridized orbital of nitrogen atom would change from sp 2 to sp 3 once it coordinated with Zn 2+ ion, and correspondingly, the -delo- Figure 2. FTIR spectra of methanol interacted with ZnCl 2 1, methanol; 2, 80 C; 3, 130 C; 4, 170 C. Figure 3. Effect of catalyst amount on DMC and NMMC yield and MC conversion: reaction temperature, 190 C; reaction time, 10 h; MC, 7.5 g; methanol, 64 g. Figure 4. Effect of reaction temperature on DMC and NMMC yield and MC conversion: reaction time, 10 h; amount of catalyst, 1.00 g; MC, 7.5 g; methanol, 64 g. Figure 5. Effect of reaction time on DMC and NMMC yield and MC conversion: reaction temperature, 190 C; amount of catalyst, 1.00 g; MC, 7.5 g; methanol, 64 g. Ind. Eng. Chem. Res., Vol. 47, No. 16, 2008 5915 calized bond of amide disappeared. Considering the FTIR spectra results, a possible mechanism for catalyst ZnCl 2 was proposed as shown in Scheme 1. At first, by the coordination of 2 equiv of MC through the nitrogen atom of amide, 1 equiv of Zn 2+ ion reached the stable construction of 18 electrons (the two chloride atoms would provide one pair of electrons each). In the Zn(NH 2 COOCH 3 ) 2 Cl 2 complex, the amino bond of ligand MC was weakened, which facilitated the nucleophilic attack of methanol. Then, a lone pair of electrons of oxygen in methanol could form a bond to the electrophilic carbonyl carbon, and at the same time, the relatively weak -bond of the carbonyl group broke; consequently, both electrons moved to the oxygen and provided the third lone pair of electrons and a negative charge. It was noteworthy that the oxygen in methanol gained a positive charge, since it had effectively lost an electron by sharing its lone pair with carbon in the new bond. Such a zwitterion intermediate might be stabilized by another Zn 2+ ion. Then, the proton of O-H moved to nitrogen, and the lone pair of electrons on oxygen returned to reform the carbonyl -bond. As a result, the C-N bond broke with both electrons moving onto the nitrogen to produce the corresponding complex Zn(NH 3 ) 2 Cl 2 and DMC. Because of the strong nucleophilic ability of MC and the liberation of NH 3 , the NH 3 in the complex was substituted by MC to finish the catalytic circle. Notably, a white crystal, which was proved to be Zn(NH 3 ) 2 Cl 2 by XRD (see Figure 6), was precipitated after the reaction solution was cooled to 0 C in our experiment. It showed the same catalytic activity as ZnCl 2 (entry 11), which powerfully supported the above reaction mechanism. In addition, it was obvious that the higher ZnCl 2 amount, the higher reaction temperature and the longer reaction time, would give rise to the higher yield of complex Zn(NH 2 COOCH 3 ) 2 Cl 2 . Thus, the MC conversion was observed to increase monotonically along with those variables. However, the yield of DMC did not always increase as described in the reaction mechanism because of the side-reactions of DMC. 4. Conclusions Among the zinc compound catalysts for the synthesis of DMC from MC and methanol, ZnCl 2 and ZnBr 2 showed the highest activity, probably due to their favorable solubility in methanol. Their high catalytic performance only originated from Zn 2+ ion. FTIR spectra and XRD characterization indicated that MC was activated by Zn 2+ through the coordination of the nitrogen atom. In addition, the reaction time, reaction temperature, and catalyst amount had a strong effect on the performance of model catalyst ZnCl 2 . The MC conversion and DMC yield under the optimal conditions reached 50.9% and 33.6%, respectively. Acknowledgment The authors acknowledge the financial support from State Key Program for Development and Research of China (No. 2006BAC02A08). Literature Cited (1) Shaikh, A. A.; Sivaram, S. Organic Carbonates. Chem. ReV. 1996, 96 (3), 951. (2) Tundo, P. New Developments in Dimethyl Carbonate Chemistry. Pure Appl. Chem. 2001, 73 (7), 1117. (3) Ono, Y. 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Chem. 2002, 41 (12), 3239. ReceiVed for reView March 6, 2008 ReVised manuscript receiVed May 8, 2008 Accepted May 12, 2008 IE8003732 Ind. Eng. Chem. Res., Vol. 47, No. 16, 2008 5917