GB2182933A - Catalysis: alkanol synthesis - Google Patents
Catalysis: alkanol synthesis Download PDFInfo
- Publication number
- GB2182933A GB2182933A GB8625655A GB8625655A GB2182933A GB 2182933 A GB2182933 A GB 2182933A GB 8625655 A GB8625655 A GB 8625655A GB 8625655 A GB8625655 A GB 8625655A GB 2182933 A GB2182933 A GB 2182933A
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- GB
- United Kingdom
- Prior art keywords
- ferrite
- alkanols
- process according
- catalyst
- reaction
- Prior art date
- Legal status (The legal status is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the status listed.)
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- C—CHEMISTRY; METALLURGY
- C07—ORGANIC CHEMISTRY
- C07C—ACYCLIC OR CARBOCYCLIC COMPOUNDS
- C07C29/00—Preparation of compounds having hydroxy or O-metal groups bound to a carbon atom not belonging to a six-membered aromatic ring
- C07C29/15—Preparation of compounds having hydroxy or O-metal groups bound to a carbon atom not belonging to a six-membered aromatic ring by reduction of oxides of carbon exclusively
- C07C29/151—Preparation of compounds having hydroxy or O-metal groups bound to a carbon atom not belonging to a six-membered aromatic ring by reduction of oxides of carbon exclusively with hydrogen or hydrogen-containing gases
- C07C29/153—Preparation of compounds having hydroxy or O-metal groups bound to a carbon atom not belonging to a six-membered aromatic ring by reduction of oxides of carbon exclusively with hydrogen or hydrogen-containing gases characterised by the catalyst used
- C07C29/156—Preparation of compounds having hydroxy or O-metal groups bound to a carbon atom not belonging to a six-membered aromatic ring by reduction of oxides of carbon exclusively with hydrogen or hydrogen-containing gases characterised by the catalyst used containing iron group metals, platinum group metals or compounds thereof
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- Chemical & Material Sciences (AREA)
- Organic Chemistry (AREA)
- Chemical Kinetics & Catalysis (AREA)
- Organic Low-Molecular-Weight Compounds And Preparation Thereof (AREA)
Abstract
Carbon monoxide and hydrogen are reacted in the presence of a catalyst to give one or more alkanols, such as alkanols having more than one carbon atom per molecule ('higher alkanols'). The catalyst used is a ferrite, such as a nickel ferrite which may be unsubstituted or substituted, e.g. with Mn, Co or Zn; or cobalt ferrite.
Description
SPECIFICATION
Catalysis: Alkanol synthesis
This invention relates to the catalytic production of alkanols, preferably those having more than one carbon atom per molecule.
Certain alkanols having more than one carbon atom per molecule (termed 'higheralkanols' herein) have potential use as gasoline extenders and in other high value applications. Their production bythecatalysed reaction of carbon monoxide and hydrogen is therefore of interest. However, on an industrial scale, this reaction has been used to manufacture methanol only. Watson and Somarjai in Journai of Catalysis, 74, 282-295 (1982) describes the use of lanthanum rhodate as a catalystforthe hydrogenation of CO under laboratory conditions to give oxygenated products having more than one carbon atom per molecule.
This invention is concerned with the catalytic production ofalkanolsfrom synthesis gas (CO and H2) using a catalyst lacking a precious metal, namely a ferrite catalyst. Ferrites are known as catalysts, (see, for example, M. Pijolat and V. Perrichon, Applied Catalysis, 13,321-333 (1985)), but mostly for the production of hydrocarbons and notfortheproductionofalkanols.
The invention comprises a process for the catalytic production of one or more alkanols by the reaction of carbon monoxide and hydrogen in the presence of a ferrite catalyst.
The process ofthe invention has been found to give rise to methanol, ethanol and otheralkanols asexemplified in the specific examples hereinafter, and also to give rise to minimal production of methane and other hydrocarbons.
It is also possible that the process may give rise to diols.
An example of a ferrite catalystthat may be used is a nickel ferrite which may be substituted orunsubstitu- ted, for example of the general formula: Ni X Mx Fe2O4 where 0 S x < 1, and M is Mn, Co orZn. xis preferably 0.5. Furtherexamples offerritesthat may be used are those of cobalt.
Ferrites, which are sometimes considered as mixed metal oxides of Fe(lll), are known materials and may be purchased commercially or made by methods known in the art.
Several ways of carrying out the invention will now be described by way of example.
The ferrite catalysts were tested in powder form and, before testing, were characterised by: (a) X-ray diffraction (XRD); (b) BETsurface area; and (c) thermogravimetric analysis (TGA). The X-ray pattern of XRD confirmed that the catalysts had the ferrite structure and the TGA showed decomposition of precursor materials where freshly prepared catalysts were used.
The general testing procedure involved placing a ferrite catalyst (1g) in a quartz reaction tube, which was then heated to 280"C in a flowing mixture (25 ml/min) of CO and H2 in the volume ratio of 70% H2: 30% CO.
This temperature was maintained for 24 hours. The product gases were bubbled through distilled water (5 ml) which was later analysed for alcohol content. During testing, gas samples were taken attwo-hourly intervals and analysed for hydrocarbons and CO2.
The above liquid product was analysed by gas chromatography wherein samples (2 FI) were injected onto a Chromosorb 102 column at 140"C on a Perkin Elmer (P.E.) sigma gas chromatograph, calibrated using standard solutions. The above gas samples were also analysed by gas chromatography using a spherecomb column, P.E. F30 gas chromatograph. The results are summarised in the table below.
Products
Ex. Catalyst & et
surface area CH3OH C2HSOH Others {m*~ ) (moleslgcat/ (molesig caV sec x 10-9) sec x 10-9) 1 Ni05Mn05Fe2O4* 1.00 1.19
(66.1) 2 Co0.8Fe2.204 0.52 0.79
(141.1) 3 Ni0.5Zn0.5Fe204 0.54 0.67
(101.0) 4 Cove204 0.29 0.34 ( < 1.0) 5 CoFe2O4 1.00 0.10
(14.7) 6 NiFe204 0.60 0.05 ( < 1.0) * the weight of this catalyst was 0.37 g.
Figures given are percentages by volume. Atick indicatesthatthe named constituent was detected in the product and dash thatthe named constituent was not detected.
The above results showthatferrite catalysts are capable of catalysing the reaction of CO and H2 to give higher alkanols without necessarily producing hydrocarbons.
CLAMS
1. A process for the catalytic production of one or more alkanols by the reaction of carbon monoxide and hydrogen in the presence of a ferrite catalyst.
2. A process according to claim 1 wherein the ferrite catalyst is a substituted or unsubstituted nickel ferrite.
3. A process according to claim 2 wherein the nickel ferrite is of the general formula: Ni1.x Mx Fe204 whern0x < 1,and M is Mn, Co orZn.
4. A process according to claim 3 wherein xis 0.5.
5. A process according to claim 1 wherein the ferrite catalyst is a cobalt ferrite.
6. A process forthe catalytic production of one or more alkanols substantially as described herein with reference to any of the examples.
**WARNING** end of DESC field may overlap start of CLMS **.
Claims (6)
1. A process for the catalytic production of one or more alkanols by the reaction of carbon monoxide and hydrogen in the presence of a ferrite catalyst.
2. A process according to claim 1 wherein the ferrite catalyst is a substituted or unsubstituted nickel ferrite.
3. A process according to claim 2 wherein the nickel ferrite is of the general formula: Ni1.x Mx Fe204 whern0x < 1,and M is Mn, Co orZn.
4. A process according to claim 3 wherein xis 0.5.
5. A process according to claim 1 wherein the ferrite catalyst is a cobalt ferrite.
6. A process forthe catalytic production of one or more alkanols substantially as described herein with reference to any of the examples.
Priority Applications (1)
Application Number | Priority Date | Filing Date | Title |
---|---|---|---|
GB8625655A GB2182933B (en) | 1985-11-14 | 1986-10-27 | Catalysis : alkanol synthesis |
Applications Claiming Priority (2)
Application Number | Priority Date | Filing Date | Title |
---|---|---|---|
GB858528109A GB8528109D0 (en) | 1985-11-14 | 1985-11-14 | Catalysis |
GB8625655A GB2182933B (en) | 1985-11-14 | 1986-10-27 | Catalysis : alkanol synthesis |
Publications (3)
Publication Number | Publication Date |
---|---|
GB8625655D0 GB8625655D0 (en) | 1986-11-26 |
GB2182933A true GB2182933A (en) | 1987-05-28 |
GB2182933B GB2182933B (en) | 1989-12-20 |
Family
ID=26290011
Family Applications (1)
Application Number | Title | Priority Date | Filing Date |
---|---|---|---|
GB8625655A Expired GB2182933B (en) | 1985-11-14 | 1986-10-27 | Catalysis : alkanol synthesis |
Country Status (1)
Country | Link |
---|---|
GB (1) | GB2182933B (en) |
-
1986
- 1986-10-27 GB GB8625655A patent/GB2182933B/en not_active Expired
Also Published As
Publication number | Publication date |
---|---|
GB2182933B (en) | 1989-12-20 |
GB8625655D0 (en) | 1986-11-26 |
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Legal Events
Date | Code | Title | Description |
---|---|---|---|
746 | Register noted 'licences of right' (sect. 46/1977) | ||
732E | Amendments to the register in respect of changes of name or changes affecting rights (sect. 32/1977) | ||
PCNP | Patent ceased through non-payment of renewal fee |
Effective date: 19961027 |