CN1064346C - Direct synthesis method of dimethyl carbonate - Google Patents
Direct synthesis method of dimethyl carbonate Download PDFInfo
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- CN1064346C CN1064346C CN95120056A CN95120056A CN1064346C CN 1064346 C CN1064346 C CN 1064346C CN 95120056 A CN95120056 A CN 95120056A CN 95120056 A CN95120056 A CN 95120056A CN 1064346 C CN1064346 C CN 1064346C
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- methanol
- magnesium
- carbon dioxide
- reaction
- dimethyl carbonate
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- Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
- Y02—TECHNOLOGIES OR APPLICATIONS FOR MITIGATION OR ADAPTATION AGAINST CLIMATE CHANGE
- Y02P—CLIMATE CHANGE MITIGATION TECHNOLOGIES IN THE PRODUCTION OR PROCESSING OF GOODS
- Y02P20/00—Technologies relating to chemical industry
- Y02P20/141—Feedstock
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- Organic Low-Molecular-Weight Compounds And Preparation Thereof (AREA)
Abstract
The present invention provides a method for synthesizing dimethyl carbonate by carbon dioxide, a potential carbon resource, as basic raw materials. Firstly, magnesium and methanol react to generate magnesium methoxide, and the carbon dioxide and the methanol are in gas liquid reaction to generate the dimethyl carbonate under the action of the magnesium methoxide. The method has the process conditions that the content of the magnesium accounts for 3% to 9% of the weight percentage of the methanol, the reaction temperature of the magnesium and the methanol is 200 DEG C, and the reaction time is one hour. The pressure of the carbon dioxide is from 10 to 50 kg/cm<2>, the temperature of the gas liquid reaction is from 120 to 200 DEG C, and the time of the gas liquid reaction is from 1 to 11 hours. The preparation method has the advantages of simple process, easy operation, single product, no secondary environmental pollution and good economical and social benefit.
Description
Theinvention relates to a preparation method of an organic compound, in particular to a method for directly synthesizing dimethyl carbonate from carbon dioxide and methanol.
Carbon dioxide is both a potential carbon source and a major cause of environmental problems such as greenhouse effect. Numerous researchers have studied the comprehensive utilization of carbon dioxide. U.S. patent 3, 657, 310 entitled: synthesis of aliphatic carbonates, alkali metal salts of monomethyl carbonate are disclosed prepared by reacting carbon dioxide with an alkali metal methoxide. And then the methyl ester of methyl carbonate is prepared by the methylation of monohalogenated methane. This process has not been developed industrially because of the use of expensive and dangerous metallic sodium and highly toxic monohalogenated methane as raw materials. Another approach is U.S. patent No. 4,661,609 entitled: the co-synthesis of ethylene glycol and dimethyl carbonate, the ester exchange method disclosed, is that firstly carbon dioxide and alkylene oxide react to obtain cyclic carbonate, and then the cyclic carbonate and methanol undergo ester exchange reaction to obtain dimethyl carbonate. The method needs two-step reaction and two-step separation process, and has complex process and high preparation cost.
The invention aims to avoid the defects of the background technology and create a method for directly synthesizing dimethyl carbonate by carbon dioxide, which has the advantages of simple process, low cost and no secondary environmental pollution.
The object of the invention is achieved by the following measures:
a direct synthesis method of dimethyl carbonate is characterized in that magnesium and methanol are firstly reacted to generate magnesium methoxide, and then carbon dioxide and methanol are subjected to gas-liquid reaction to generate dimethyl carbonate under the action of the magnesium methoxide, wherein the reaction equation is as follows: the process conditions are as follows: (1) the magnesium content accounts for 3-9% of the weight of the methanol; (2) reaction temperature of magnesium with methanol: 200 ℃, reaction time: 1 hour; (3) the pressure of the carbon dioxide is 10-50 Kg/cm2(4) The reaction temperature of the gas-liquid reaction of the carbon dioxide and the methanol under the action of the magnesium methoxide is 120-200 ℃ (5) the reaction time of the gas-liquid reaction of the carbon dioxide and the methanol under the action of the magnesium methoxide is 1-11 hours, compared with the background art, the invention has the following advantages: 1. the preparation process is simple, convenient to operate, single in product and low in cost.
2. The preparation process of the invention does not produce secondary environmental pollution, has rich raw material sources and fully utilizes the potential carbon resource of carbon dioxide.
3. The invention has good industrialization prospect, the dimethyl carbonate is not only used as a methylation reagent, a carbonylation reagent and an organic synthesis intermediate, but also can be used as a novel fuel additive, can replace methyl tert-butyl ether, and has remarkable effect on improving the octane number and the oxygen content of the fuel.
Therefore, the invention has good economic benefit and social benefit.
The invention is further illustrated by the following examples:
example 1:
weighing 10 g of magnesium metal, adding the magnesium metal into an autoclave, mixing the magnesium metal with 200 ml of methanol, sealing the autoclave, reacting the mixture for 1 hour at 200 ℃, cooling the autoclave, and introducing 30 Kg/cm2Reacting the carbon dioxide gas at 180 ℃ for 5 hours, cooling, removing residual gas, distilling and separating to obtain the product, wherein the yield of the dimethyl carbonate is 16.4 percent (mol ratio) of the carbon dioxide raw material gas.
Example 2:
weighing 5 g of magnesium metal, adding the magnesium metal into an autoclave, mixing the magnesium metal with 200 ml of methanol, sealing the autoclave, reacting the mixture for 1 hour at 200 ℃, cooling the autoclave and introducing 30 Kg/cm2Reacting the carbon dioxide gas at 140 ℃ for 2 hours, cooling, removing residual gas, and obtaining a product by distillation and separation, wherein the yield of the dimethyl carbonate is 4.46 percent (mol ratio) of the carbon dioxide raw material gas.
Example 3
Weighing 13 g of magnesium metal, adding the magnesium metal into an autoclave, mixing the magnesium metal with 200 ml of methanol, sealing the autoclave, reacting the mixture for 1 hour at 200 ℃, cooling the autoclave and introducing 10 Kg/cm2Reacting the carbon dioxide gas at 200 ℃ for 8 hours, cooling, removing residual gas, and obtaining a product by distillation and separation, wherein the yield of the dimethyl carbonate is 15.9 percent (mol ratio) of the carbon dioxide raw material gas.
Example 4:
weighing 10 g of magnesium metal, adding into an autoclave and 200 ml of methanolMixing, sealing, reacting at 200 deg.C for 1 hr, cooling, and introducing 50Kg/cm2Reacting the carbon dioxide gas at 160 ℃ for 10 hours, cooling, removing residual gas, and obtaining a product by distillation and separation, wherein the yield of the dimethyl carbonate is 10.1 percent (mol ratio) of the carbon dioxide raw material gas.
Claims (1)
- The direct synthesis process of dimethyl carbonate features that magnesium and methanol are first reacted to produce magnesium methoxide, and then carbon dioxide and methanol are reacted under the action of magnesium methoxide to produce dimethyl carbonate, with the reaction equation as follows:
the process conditions are as follows:(1) the total amount of magnesium accounts for 3-9% of the weight of the methanol;(2) the reaction temperature of the reaction of magnesium and methanol is 2O0 ℃, and the reaction time is 1 hour;(3) the pressure of the carbon dioxide gas is 10-50 Kg/cm2；(4) The reaction temperature of the gas-liquid reaction of the carbon dioxide and the methanol under the action of the magnesium methoxide is l 20-200 ℃;(5) the reaction time of the gas-liquid reaction of the carbon dioxide and the methanol under the action of the magnesium methoxide is 1-1 l hour.
Priority Applications (1)
| Application Number | Priority Date | Filing Date | Title |
|---|---|---|---|
| CN95120056A CN1064346C (en) | 1995-11-27 | 1995-11-27 | Direct synthesis method of dimethyl carbonate |
Applications Claiming Priority (1)
| Application Number | Priority Date | Filing Date | Title |
|---|---|---|---|
| CN95120056A CN1064346C (en) | 1995-11-27 | 1995-11-27 | Direct synthesis method of dimethyl carbonate |
Publications (2)
| Publication Number | Publication Date |
|---|---|
| CN1131660A CN1131660A (en) | 1996-09-25 |
| CN1064346C true CN1064346C (en) | 2001-04-11 |
Family
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Family Applications (1)
| Application Number | Title | Priority Date | Filing Date |
|---|---|---|---|
| CN95120056A Expired - Fee Related CN1064346C (en) | 1995-11-27 | 1995-11-27 | Direct synthesis method of dimethyl carbonate |
Country Status (1)
| Country | Link |
|---|---|
| CN (1) | CN1064346C (en) |
Families Citing this family (2)
| Publication number | Priority date | Publication date | Assignee | Title |
|---|---|---|---|---|
| CN106478421B (en) | 2015-08-31 | 2019-09-13 | 亚申科技(浙江)有限公司 | DMC Processes |
| WO2017093472A1 (en) | 2015-12-02 | 2017-06-08 | Ait Austrian Institute Of Technology Gmbh | Method and device for the continuous production of organic carbonates from co2 |
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1995
- 1995-11-27 CN CN95120056A patent/CN1064346C/en not_active Expired - Fee Related
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| Publication number | Publication date |
|---|---|
| CN1131660A (en) | 1996-09-25 |
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