PROCESS FOR THE HYDROGENATION OF UNSATURATED ORGANIC COMPOUNDS USING SOLID CATALYSTS

Abstract: Unsaturated organic compounds are hydrogenated by contact under hydrogenation conditions with as catalyst a rare earth oxyhydride having the formula: Tr 1-q G q Ni 5-p M p O y H x (I) wherein Tr is a rare earth element, G is either Th and/or Y, M is a metal selected from the group consisting of Cu, Mn, Al, Fe, Cr, Co, Rh, Ru, Re, Pt, Pd, Ir, Os, Mo, V, Ti, W and mixtures of two or more thereof, q is zero or a number less than or equal to 1, p is zero or a number less than or equal to 5, y is a whole number or decimal number in the range from 0.4 to 6.5, and x is zero or a whole number or decimal number equal to or less than 15.

Description: The present invention relates to a process for the hydrogenation of unsaturated organic compounds using solid hydrogenation catalysts. Solid catalysts, for example nickel-containing catalysts, are known for the hydrogenation of unsaturated organic compounds. Our copending European application publication No. 0208405 published on 14th January, 1987, i.e. after the priority date of 21st November, 1986, claimed for the present application, on an application having a filing date before the aforesaid priority date describes and claims rare earth oxyhydrides of the formula:- RE 1-q G q Ni 5-p M p O y H x wherein RE is a rare earth element or a mixture of rare earth elements, G is either Th and/or Y, M is at least one of Cu, Mn, Al, Fe, Cr or Co, q is zero or a number less than 1, p is zero or a number less than 5, y is an integer or decimal number from 0.4 to 6.5, and x is an integer or a decimal number equal to or less than 15, and their preparation. Whilst no uses for the rare earth oxyhydrides in general are disclosed, there is a passing mention in Example 5 that an oxyhydride having the stoichiometry of MmNi 5 O 1.7-w (WO 3 ) 2w H 8 and a specific surface area of approximately 20 m²/g proved very active in the hydrogenation of isoprene. We have now found that rare earth oxyhydrides are effective as catalysts for the hydrogenation of unsaturated compounds. Accordingly, the present invention provides a process for the hydrogenation of an unsaturated organic compound by contacting the unsaturated organic compound with a solid hydrogenation catalyst under hydrogenation conditions characterised in that the solid hydrogenation catalyst comprises a rare earth oxyhydride having the formula: Tr 1-q G q Ni 5-p M p O y H x (I) wherein Tr is a rare earth element, G is either Th and/or Y, M is a metal selected from the group consisting of Cu, Mn, Al, Fe, Cr, Co, Rh, Ru, Re, Pt, Pd, Ir, Os, Mo, V, Ti, W and mixtures of two or more thereof, q is zero or a number less than or equal to 1, p is zero or a number less than or equal to 5, y is a whole number or decimal number in the range from 0.4 to 6.5, and x is zero or a whole number or decimal number equal to or less than 15 and with the proviso that the process is other than the hydrogenation of isoprene in the presence of an oxyhydride having the stoichiometry MmNi 5 O 1.7-w (NO 3 ) 2w H 8 and a specific surface area of approximately 20 m²/g. Rare earth oxyhydrides are sometimes referred to as intermetallic rare earth compound (IREC) oxyhydrides. By rare earth element is meant elements ranging from lanthanum (atomic number 57) to lutetium (atomic number 71), as well as their mixtures. Among the mixtures, the mixture called Mischmetal (Mm) is particularly recommended, this being a mixture of rare earths having a composition which varies according to the supplier. A Mischmetal is commercially available in the following composition (% by weight): La 33%, Ce 48%, Pr 13%, Nd 4% and other rare earths 2%. A feature of the aforesaid composition is the high cerium (Ce) content. A suitable cerium-free Mischmetal has the following composition: La 63%, Pr 25%, Nd 8%, other rare earths 4%. A suitable Mischmetal-Nickel alloy has the following composition: Ni 68.6%, Fe 0.16%, O₂ 0.05%, Mm 31.3%. A suitable cerium-free Mischmetal-Nickel alloy (MmCe o Ni₅) has the following composition:- Ni 68.2%, Fe 0.21%, O₂ 0.45% and Mm 31.4% A suitable naturally occuring form of Mischmetal is the mineral Bastnasite which has the composition as follows: Ce 48 - 50%, La 32 = 34%, Pr 13 - 14%, Nd 4 - 5%, other rare earths 2%. An advantageous composition of Mischmetal comprises the following constituents: Ce 47 - 50%, La 23 - 34%, Pr 5 - 14%, Nd 4 - 18%, other rare earths 2 - 4%. In all the foregoing compositions, the percentages are expressed by weight. In the formula (I), M is preferably a metal selected from the group consisting of Cu, Mn, Al, Fe, Cr, Co, Rh and Ru. In the formula (I), y is preferably a whole number or decimal number in the range from 1 to 3.5 and x is preferably a whole number or decimal number in the range from 1 to 8. The preferred rare earth oxyhydrides include the oxyhydrides having the following formulae: MmNi₅O y H x (II) CeNi₅O y H x (III) LaNi₅O y H x (IV) PrNi₅O y H x (V) Among the rare earth oxyhydrides free from cerium, the following compound must be mentioned: MmCe o Ni₅O y H x (VI) Among the other interesting rare earth oxyhydrides, the following may be mentioned: CeNi 5-k M k O y H x (VII) Ce 1-s Ni₅G s O y H x (VIII) MmNi 5-k M k O y H x (IX) Mm 1-5 Ni₅G s O y H x (X) In the formulae (II) to (X), Mm is Mischmetal, x and y have the same meaning as in formula (I); k is 0 or a whole number or decimal less than 5; s is 0 or a number less than 1. The rare earth oxyhydrides may be supported on a suitable support. Suitable supports include alumina, silica-alumina, carbon, and the like. The rare earth oxyhydrides of formula (I) useful in the process of the present invention may be prepared from rare earth metals or rare earth metal alloys in a variety of different ways, generally by processes which involve a number of steps. A first process, denoted hereinafter as process (A), comprises the steps as follows: in a first step subjecting an IREC of the formula: Tr 1-g G g Ni 5-p M p (XI) in a closed reactor, preferably an autoclave, to a plurality of hydriding/dehydriding cycles thereby to form a hydride, the hydriding being performed under a hydrogen pressure of from 20 to 200, preferably from 50 to 100 bar, and at a temperature of from 20 to 450°C, preferably about 350°C, and the dehydriding being performed in the same closed reactor at a temperature in the range from 20 to 450°C, in a second step oxidising the hydrided product obtained in the first step, and in a third step chemically reducing the product obtained in the second step. In the first step of the process (A) the hydrogen pressure may be maintained by compensating for the quantity of hydrogen absorbed by the compound of formula (XI). To effect dehydriding, the closed reactor may be placed under subatmospheric pressure and re-heated to the temperature at which hydriding was performed, i.e. a temperature in the range from 20 to 450°C. Following the second dehydriding cycle hydrogen fixing will generally be found to be easier and the pressure may thereafter be reduced. The hydriding/dehydriding may suitably be performed on the IREC in lump or block form, which forms subsequently disintegrate. The specific surface area of the powder thereby formed is observed to increase with the number of hydriding/dehydriding cycles to which it is subjected. Suitably from 4 to 20 cycles may be carried out. In the second step the hydride is obtained in the first step is oxidised, suitably by contact with an oxygen-containing gas or gaseous oxidant, for example air or oxygen, at a temperature in the range from 20 to below 450°C. This may be achieved either by allowing the hydride obtained in the first step to cool in contact with the oxygen-containing gas or gaseous oxidant, the temperature of which is lower than that of the hydride, or by preheating the aforesaid gas to a temperature below that of the hydride before contact therewith. The oxidation may suitably be carried out by heating the hydride in a current of O₂/N₂ for about 15 hours at about 400°C. Generally, the amount of oxygen which can be fixed increases with an increase in the oxidation temperature. Thereafter, the product from the second step is chemically reduced in the third step to produce the rare earth oxyhydride. This may suitably be effected by contacting the product at elevated temperature, preferably at about 300°C, with hydrogen, either under batch or continuous flow conditions. A second process for the production of rare earth oxyhydrides, denoted hereinafter as process (B), comprises the steps as follows: in a first step forming a solution comprising soluble salts of nickel and the other metallic element(s) thermally decomposable to the oxides thereof in such proportions as to satisfy the stoichiometric relationship of formula (I), and thereafter precipitating a mixture of the thermally decomposable salts of nickel and the other element(s), in a second step partially or wholly thermally decomposing the mixture of heat decomposable salts obtained in the first step, and in a third step reducing the product obtained in the second step in the presence of hydrogen. As regards the first step, the solution may suitably be formed by dissolving the salts of the metals thermally decomposable to their oxides in appropriate proportions in a suitable solvent, for example water. A preferred method of forming the solution, however, comprises reacting the rare earth intermetallic compound with a suitable acid. In this manner the solution so-obtained has the stoichiometry dictated by the formula (I). A preferred salt thermally decomposable to the oxide is the nitrate, though other salts may be employed. Thus it is preferred, in the preferred method of performing the first step to react the IREC with aqueous nitric acid. Precipitation of a mixture of the thermally decomposable salts may be achieved in a variety of ways. A suitable method is to evaporate the solution until the salts precipitate out. Alternatively, precipitation may be effected by the addition of a suitable reagent. Suitably precipitation may be accomplished by the addition of a basic solution or other precipitant drop by drop to the solution of salts, preferably the nitrates. As the basic solution there may suitably be used an amine, for example triethylamine, or a carbonate. It is preferred, thereafter, to dry the precipitate so-obtained. This step may suitably be effected in the presence of a support, for example alumina, silica-alumina, carbon, or the like. In this way it has been found possible to produce, for example, LaNi 5 O 1.7 H 10 supported on alumina. In the second step the mixture of heat decomposable salts is partially or wholly decomposed. Partial decomposition may suitably be achieved in the case of nitrate salts, for example, by calcination at a temperature in the range from 400 to 800°C for a period sufficient to achieve partial decomposition, e.g. 15 hours. Total decomposition may suitably be achieved by calcination at 800°C for a period sufficient to achieve total decomposition, e.g. 15 hours. At a calcination temperature of 800°C, there is no nitrate residue, but a reduction in the specific surface area is observed. Calcination is preferably carried out at a temperature above 450°C and below 800°C, more preferably from 500 to 600°C. In the third step the product obtained in the second step is reduced in the presence of hydrogen under appropriate conditions, for example at 300°C under atmospheric pressure. The oxyhydride obtained by calcination at 400°C (i.e. still containing some nitrates) and subsequent reduction at 300°C under hydrogen at atmospheric pressure conforms to the stoichiometry: MmNi 5 O 1.7-w (NO 3 ) 2w H x (XIII) wherein w is less than 0.1. This stoichiometry was calculated by mass balance from thermogravimetric data. This oxyhydride is somewhat unique in that it has a specific surface area of approximately 20m²/g, whilst the oxyhydrides prepared by other methods generally have surface areas of less than 10m²/g. A preferred process for the production of rare earth oxyhydrides, denoted hereinafter as process (C) is a modification of process (B). The modification concerns the first step of process (B) wherein, instead of adding a basic solution to the solution of the salts in order to effect precipitation, the solution of salts is added portionwise to an excess of the base under conditions of efficient mixing, thereby to effect precipitation at constant pH. In all other respects process (C) is identical to process (B). An advantage of process (C) is that the rare earth oxyhydrides so-produced have very high surface areas, for example 100 to 120 m²/g. It can be seen that the processes (A) to (C) enable a product to be obtained in the form of a powder in the first step, the oxidised product, hereinafter to be referred to as the precursor oxide, to be obtained in the second step and the oxyhydride to be obtained in the third step. It will be observed that the amount of hydrogen fixed in the third step increases with the degree of oxidation in the second step. The more oxygen the precursor oxide contains (the higher the content), the more hydrogen it will fix (x increases). During the third step (hydrogenation and formation of the oxyhydride) there is a simultaneous reduction and incorporation of hydrogen atoms. Starting with the precursor oxide of a Mischmetal-Nickely alloy, the following reaction is observable at 300°C and at a hydrogen pressure of 1 bar This reaction, which leads to a reduction in the proportion of oxygen and the inclusion of hydrogen is very different from the standard hydrogenation, since the "hydriding" proportion is irreversible. The hydrogen incorporated in the oxyhydride of formula (XIV), may be used as a reductant when the latter is contacted with compounds capable of being hydrogenated, i.e. unsaturated organic compounds. By contacting the oxyhydride of formula (XIV) with an olefin for example at a temperature of 150°C the following reaction takes place:- By contacting the compound of formula (XV) with hydrogen at atmospheric pressure and at ambient temperature the original oxyhydride of formula (XIV) can be re-formed according to the equation: MmNi 5 O 1.7 + 4H 2 → MmNi 5 O 1.7 H 8 The foregoing reactions form the basis for using rare earth oxyhydrides as hydrogenation catalysts. In fact, the rare earth oxyhydride is able to donate its hydrogen to a reducible compound, replenish itself with hydrogen, again donate its hydrogen, again replenish itself and so on. The catalytic activity of the oxyhydride depends on a number of factors including the values of x and y in the formula (I) and its specific surface are. The specific surface area in turn depends upon the process used for its preparation. The precursor oxides possess a specific surface area of the order of 10 m²/g when prepared by process (A) and of the order of 20 m²/g when prepared by process (B), provided that the calcination temperature is below 600°C. In passing from the precursor oxide form to the oxyhydride form the specific surface area increases considerably, and may attain a value of up to 50 m²/g. As mentioned hereinbefore, it is an advantage of process (C) that it can result in specific surface areas of the order of 100 to 120 m²/g. The unsaturated organic compound may suitably be an olefinically unsaturated compound or an acetylenically unsaturated compound, preferably an olefinically unsaturated compound. The olefinically unsaturated compound may be monoolefinically unsaturated, diolefinically unsaturated, polyolefinically unsaturated or aromatically unsaturated. The unsaturated compound may be an aliphatic, cycloaliphatic or aromtic compound, or a combination thereof. Examples of unsaturated compounds which may be hydrogenated in the process of the present invention include olefins, for example alkenes, cycloalkenes and aralkenes, monocyclic aromatic hydrocarbons, for example benzene and alkylbenzenes, polycyclic aromatic hydrocarbons, for example naphthalene, heterocyclic aromatic hydrocarbons containing nitrogen in the aromatic ring, for example pyridine, or containing sulphur in the aromatic ring, for example thiophene, or a mixture of two or more thereof. The nature of the hydrogenation conditions will depend on the nature of the unsaturated compound to be hydrogenated. These conditions are well established in the art and are further illustrated in the following Examples. It is believed that the hydrogen contained in the oxyhydrides is present either as surface hydrogen, which is immediately available for reaction, or incorporated in the body of the oxyhydride. On contact with unsaturated compounds the oxyhydride it is believed donates the surface hydrogen, which is then replaced by hydrogen from the body. On the other hand, in the presence of added gaseous hydrogen it is believed that everything occurs as though the hydrogen on the surface of the oxyhydride is replaced by the hydrogen deriving from the body of the oxyhydride, which is itself replaced by the external hydrogen. Whilst we do not in any way wish to be held to these beliefs, it is nevertheless possible to operate the process in the absence of added gaseous hydrogen, but the reduction reaction rate decreases with time. However, it is preferred to operate the process in the presence of additional hydrogen. It is an advantage of the use of rare earth oxyhydrides in the process of the invention that in comparison with many prior art hydrogenation catalysts, for example metals and metal oxides, they are appreciably more tolerant to sulphur, or expressed in another way they are appreciably more resistant to sulphur poisoning. Moreover, it has been established that using feeds containing for example pyridine and/or naphthalene the hydrogenation activity relative to naphthalene and the hydrogenolysis activity relative to pyridine is largely independent of the hydrogen pressure. This is important because taken together with the finding that the rare earth oxyhydrides are substantially insensitive to dimethyl disulphide (DMDS) and thiophenes it indicates that it may be possible to hydrogenate naphthalene, pyridine, DMDS, thiophene and other aromatic products during different hydrotreatments of mineral oil-derived feedstocks, for example hydrocracking, hydrodesulphurisation, hydrodenitrification, hydroisomerisation and hydrogenation at low hydrogen pressures. This is to be compared with catalysts currently in use for which it is necessary to operate at high pressures. The process of the present invention will now be further illustrated by the following Examples. Example A Preparation of an Oxyhydride from a Hydride [Illustrative of preparative process (A)] The hydride was produced from MmNi₅. The hydrogenation was carried out in five cycles at 450°C, at a hydrogen pressure of 150 bars. The compound with the formula MmNi₅H₆ was thus obtained. This hydride was then oxidised with air (in a muffle furnace with an O₂/N₂ current) for 15 hours at 450°C, to give the compound with the formula MmNiO 6.76 . This precursor oxide was reduced in a current of H₂, at atmospheric pressure and at 300°C. The oxyhydride with the formula MmNi 5 O 0.76 H 8 was then obtained. Examples B and C Preparation of an Oxyhydride from Nitrates of Nickel and Rare Earths Illustrative of Preparative Process (B) The first stage involved the preparation of a solution of nickel nitrate and rare earth nitrates. either from Ni and Mm, in a stoichiometric ratio of Ni:Mm = 5; or by attacking the metal alloy NmNi₅ with HNO₃ which enables a satisfactory stoichiometric ratio to be obtained directly. The solution was then evaporated at approximately 80°C until the nitrates precipitate. The precipitate was then dried. In the second stage the precipitate was decomposed by eliminating NO₂. The black residue was then calcined. In carrying out Example B calcination was effected at 400°C, which did not allow the nitrates to be completely eliminated. In the course of Example C the precipitate was calcined at 800°C for 15 hours (which completely eliminated the nitrate but reduced the specific area of the intermediate precursor oxide and that of the oxyhydride). In both cases the hydrogenation was effected at 300°C at atmospheric pressure. According to Example B (calcination at 400°C) the oxyhydride with the formula: MmNi 5 O 1.7-w (NO 3 ) 2w H 8 was obtained, where w denotes a value less than 0.1, and according to Example C (calcination at 800°C), the oxyhydride with the formula: MmNi 5 O 1.7 H 8 was obtained. The oxyhydride prepared by process (B) exhibits a specific area approximately twice that of the oxyhydride prepared in Example A from the hydride, provided that too high a temperature (exceeding 700°C) is avoided during calcination. The specific areas measured on the precursor oxides (before reduction by hydrogen) were approximately 20 m²/g for the oxide prepared in Example B, and calcined at 400°C, and approximately 5 m²/g for the oxide prepared in Example C and calcined at 800°C, both obtained from nitrates, and approximately 10 m²/g for the oxide in Example A obtained from the hydride. It was not possible to measure the specific area of the oxyhydrides obtained after the third stage. It appears, however, that these specific areas were increased considerably during the third stage. Example 4 - (Illustrative of Preparative Process (C)) The method comprised five different steps:- 1. Precipitation 2. Filtration 3. Drying 4. Oxidation 5. Sieving Step (I) - Precipitation (a) Materials Peristaltic pump: Masterflex 7016 (Bioblock scientific) Electric stirrer with glass screw Teflon tubing Milli-Q-grade water (Millipore) Ce(NO₃) 3. 6H₂O (cerium(III)nitrate), rectapurgrade (Prolabo) Ni(NO₃) 2. 6H₂O (nickel(II)nitrate), normapurgrade (Prolabo) Triethylamine (for synthesis) (Prolabo) (TEA) (b) Procedure Cerium and nickel nitrates were weighed and dissolved in water until the total concentration of nitrates salts was about 275 g/litre. The nitrates solution was dripped continuously (2.5 ml/minute) into a large excess of continuously stirred TEA (4 litre of TEA minimum per litre of nitrates solution). The stirrer speed was set to give rapid agitation without causing a vortex. Each nitrate solution drop dripping into the TEA reacted quickly and hydroxides precipitated. The precipitate was ejected from the reaction zone and concentrated on the wall of the flask. TEA is not soluble in water. Since the density of TEA is lower than that of water, the upper part of the liquid phase in the vessel remained nearly pure TEA. In accordance the reaction zone contained nearly pure TEA throughout and the drops kept precipitating instantaneously. Step (2) - Filtration Two different methods were used: (a) filtration on a glass filter and washing with methanol in order to eliminate the remaining TEA and subsequent washing with water in order to remove the remaining methanol, and (b) centrifugation at 3000 r.p.m. and washing with methanol repeated twice and thereafter washing the precipitate with fresh water. (3/4) Drying and Oxidation (Calcination) The washed powder from step (2) was first dried at 100°C for 15 hours and thereafter calcined in a quartz reactor at 430°C using an air flow of 40 ml/minute for 24 hours. (5) Sieving For the pilot plant and microreactor experiments only the fraction having particles sized between 37 and 250 microns were selected. EXAMPLES OF CATALYTIC USAGE Examples 1 - 13 These Examples, which are summarised in Table 1 below, relate to the hydrogenation of isoprene at 20°C with H₂ at atmospheric pressure, using oxyhydrides as catalysts. The Examples differ in the initial material, the preparative process, the oxidation temperature and in the specific are at the precursor oxide stage. In Table 1 the columns contain the following information. Column 1 indicates the number of the Example; Column 2 indicates the general formula of the oxyhydride used; Column 3 indicates the preparation process used (A) or (B), the product obtained in step I, which is used as the initial (raw) material for step II (oxidation); Column 4 indicates the oxidation temperature (°C) and the specific area (m²/g) of the precursor oxide; Column 5 indicates the values of y and x, i.e. the molar contents of oxygen and hydrogen; Column 6 indicates the activity of the oxyhydride, expressed in mmols/h/m² (mmols of isoprene obtained per hour and per m² of specific area of the catalyst, measured in the precursor oxide state); and the selectivity, expressed in terms of the result of the hydrogenation of isoprene It will be seen that the first three of these compounds are isopentenes representing an intermediate reduction stage, whilst the last compound is the isopentane representing the final reduction stage. INTERPRETATION OF THE RESULTS The following observations may be made: Catalytic activity varies according to the hydrogen (x) and oxygen (y) content of the oxyhydride. If these values are low (Examples 1, 2, 3, 5), oxhydrides are obtained which behave like hydrides and lead essentially to isopentenes, with practically no isopentane obtained, whereas the compounds where x and y have high values (Examples 6 to 13) give a high proportion of isopentane. It will also be observed that the oxyhydrides prepared by preparative process (B) exhibit a higher specific area, which also favours the production of isopentane. Table I also indicates the size of the specific area, which depends on the oxyhydride preparation process, and particularly on the calcination temperature. If the calcination temperature is too high (800°C for Example 7), less isopentane is produced than in Example 6 (calcination temperature 400°C). Example 14 This Example illustrates the reduction of isopentene by means of an oxyhydride, at a temperature of 150°C, in the absence of hydrogen, using helium as a carrier. This Examples enabled the total hydrogen content and the rate of retrodiffusion of the bulk hydrogen (inside the oxyhydride) to the surface of the oxyhydride to be determined. The reaction is as follows: MmNi 5 O 1.7 H 8 + 4 (olefin) → MmNi 5 O 1.7 + 4 (alkane) This reaction enables the relative rate of hydrogenation to be represented as a function of the relative hydrogen concentration of the oxyhydride. Figure 1 indicates, on the x-axis, the relative hydrogen concentration of the oxyhydride, and on the y-axis the relative rate of hydrogenation. This curve may be divided into three zones, zone I corresponding to the surface hydrogen (+/- 15% of the total hydrogen content). During the initial stage of the hydrogenation, corresponding to this zone I, only isopentane is obtained. Total isopentane hydrogenation requires rapid diffusion of the hydrogen, which may be limited by the retrodiffusion of the mass hydrogen to the surface of the oxyhydride. In zone II, only isopentene (mono-olefin) is obtained, which indicates limited retrodiffusion. In zone III (after 1 hour), when the hydrogen content of the oxyhydride is reduced to 25% of the initial content, the hydrogenation continues but it slows down considerably. Example 15 The isoprene was hydrogenated under the same conditions as in Example 14; except that the intake of isoprene was stopped for approximately 20 minutes after the first hour of reaction. When the isoprene intake was resumed, the relative speed of hydrogenation was shown to have increased substantially, but this increase in speed only lasted a few minutes, then reversed to its value before the isoprene intake was stopped. This test shows that there is retrodiffusion of the mass hydrogen to the surface of the oxhydride. Rare earth oxyhydrides and IREC oxyhydrides may be used advantageously as catalysts for the hydrogenation not only of olefins, but also of other unsaturated compounds, particularly monocyclic aromatic hydrocarbon compounds such as benzene, polycyclic aromatic compounds such as naphthalene, heterocyclic compounds containing nitrogen in their nucleus, such as pyridine, or sulphur in their nucleus, such as thiophene. Example 16 and Comparative Example 17 Hydrogenation of Naphthalene Example 16 illustrates the hydrogenation of naphthalene, in a pilot installation, with hydrogen at a pressure of 160 bars, at a temperature of 100°C, the naphthalene being present in n-heptane at a concentration of 2% (% higher than present in practice). An oxyhydride with the formula: MmNi 5 O 1.7 H 8 is used as the catalyst. Comparative Example 17 illustrates the same hydrogenation as Example 16, the difference being that the oxyhydride used as a catalyst in Example 16 was replaced by a hydride obtained from MmNi₅. The results are shown in Figure 2, the x-axis representing the time expressed in hours, and the y-axis representing the percentage of reduced naphthalene by weight at a given moment, the reduction taking place instantaneously. Curve A corresponds to Example 16, using the oxyhydride as the catalyst, and curve B corresponds to Example 17, using the hydride of MmNi₅ as the catalyst. It is seen that the catalytic activity of the oxhydride is much greater than that of the hydride, and also that this activity remains practically constant, even after a period of 1750 hours (72 days), whilst the catalytic activity of the hydride decreases fairly rapidly with the time on stream. The naphthalene (C₁₀H₈) may be partially reduced to tetralin or tetrahydronaphthalene (C₁₀H₁₂), total reduction leading to the formation of decalin or decahydronaphthalene (C₁₀H₁₈), Example 16, using the IREC oxyhydride as the catalyst, leads to the formation of a mixture of decalin and tetralin, with a higher quantity of decalin, whilst Example 17, using the IREC hydride as the catalyst, gives only tetralin (partial hydrogenation). Example 18 Example 16 was reproduced, the difference here being that the reaction temperature was 350°C, and the initial materials also contained, more than 2% by weight of naphthalene, about 0.1% of dimethyl disulphide (DMDS) by total weight of the mixture. The reduction of the naphthalene was carried out for 150 hours (six days). The catalytic activity is expressed in terms of the percentage conversion of naphthalene (% of reduced naphthalene) on the one hand, and by the hydrogenation activity on the other. The hydrogenation activity also takes into account the degree of reduction of the naphthalene, and is expressed by the relation: Hydrogenation activity = 0.4. (% Tetraline) + (% Decaline) The results are shown in Figure 3. The upper curve C indicates the conversion of the naphthalene (% by weight of reduced naphthalene), the lower curve D expresses the hydrogenation activity, as indicated above. It will be seen that at a temperature of 350°C (curve C, Figure 3), the percentage of reduced naphthalene is almost twice that obtained at 100°C (curve A, Figure 2). It will also be seen that due to the presence of sulphur, the activity of the catalyst is slightly reduced in the course of the first day, then remains practically stable. It will also be seen that, unlike the catalysts consisting of metals or metal oxides, which are quickly contaminated by compounds of sulphur, the oxyhydrides, although reducing their activity at the end of the first day, then maintain a relatively high activity, which remains practically stable, despite the presence of the compounds containing sulphur. Other tests for the reduction of naphthalene containing thiopene (more difficult to use than DMDS) show that the catalytic activity of the oxyhydride is maintained even if the thiophene content attains a value of 1.5% of the naphthalene content. Example 19 and Comparative Example 20 Example 19 illustrates the reduction of naphthalene (2% by weight in n-heptane) in the presence of 0.1% by weight of DMDS at 350°C, at different hydrogen pressures, using as catalyst the oxyhydride having the formula: MmNi 5 O 1.7 H 8 , prepared according to process A. The percentages are expressed in relation to the total weight of the mixture n-heptane + naphthalene + DMDS. Comparative Example 20 illustrates the reduction of the same product, replacing the oxyhydride with a Nickel catalyst on an alumina support, and varying the hydrogen pressure. The percentage conversion of the naphthalene was determined, and the result shown in Figure 4, where the x-axis indicates the logarithm of the hydrogen pressure, and the y-axis the logarithm of the naphthalene conversion. The straight line E represents the percentage conversion of the naphthalene, using the oxyhydride as the catalyst, at hydrogen pressures varying from 80 to 150 bars, and straight line F represents the percentage conversion of the naphthalene using Ni/Al₂O₃ as a catalyst, at hydrogen pressures from 80 to over 200 bars. It will be seen that straight line E is horizontal, i.e. using oxyhydride as a catalyst the percentage conversion of the naphthalene is independent of the hydrogen pressure, whilst straight line F shows that when nickel on an alumina support is used as the catalyst, the conversion of the naphthalene is a function of the square of the hydrogen pressure. The two curves intersect at point P, which corresponds to a hydrogen pressure of 180 bar. In other words, the use of an oxyhydride with the formula MmNi 5 O 1.7 H 8 as a catalyst enables hydrogen to be used at reduced pressure, instead of working at a high hydrogen pressure with a Ni/Al₂O₃ catalyst. Examples 21 - 25 These Examples illustrate the hydrogenation of naphthalene and pyridine in the presence and in the absence of sulphur-containing compounds (DMDS). Use is made of 12.6 g of oxyhydride of the same type as that used in Example 6 for the hydrogenation of isoprene. This oxyhydride, prepared from MmNi₅, dissolved in HNO₃ and calcined at 400°C, had a specific area of 20.3 m²/g in the precursor oxide state. The conversion of the precursor oxide to oxyhydride was carried out, for convenience of handling, at a hydrogen pressure of 150 bar and at a temperature of 300°C. The composition to be hydrogenated contained, in n-heptane, 2% naphthalene, p% pyridine and q% DMDS. The conversion of naphthalene (% of reduced naphthalene) was measured, together with the hydrogenation activity of the naphthalene, expressed by the relation: Hydrogen activity of the naphthalene = 0.4. (% Tetralin) + (% Decalin). The conversion of pyridine (% of reduced pyridine) was also measured. The results are given in Table II, where the columns contain the following information: Column 1 indicates the number of the Example; Column 2 indicates the hydrogen pressure in bar; Column 3 indicates the value of q, i.e. the % by weight of DMDS in the composition to be hydrogenated; Column 4 indicates the value of p, i.e. the % by weight of pyridine in the composition to be hydrogenated; Column 5 indicates the conversion of naphthalene in % by weight; Column 6 indicates the hydrogenation activity of naphthalene in %, Column 7 indicates the conversion of pyridine in %. Example No. P(H₂) (bar) q. (%DMDS) p. (%pyridine) Conversion of Naphthalene (%) Hydrogenation activity of Naphthalene (%) Conv. of Pyridine (%) 21 80 0.1 0 40 17 0 22 80 1 0 44 18 0 23 80 1 1 12 5 58 24 150 0.1 0 41 18 0 25 150 0.1 1 17 7 74 The following observations may be made: The pyridine is completely reduced and converted to ammonia and pentane. No trace is found of piperidine, which constitutes the first stage of pyridine reduction. The naphthalene is hydrogenated in almost the same way in the presence and absence of DMDS, there being no competition between the naphthalene and DMDS during hydrogenation. This result, obtained with an oxyhydride prepared according to process (B) (precipitation of the nitrates) confirms the result obtained in Example 19, where use is made of an oxyhydride prepared according to process (A) (passing through the hydride stage). The two oxyhydrides, one prepared by process (A) and the other by process (B), prove insensitive to DMDS, and even with a relatively high % of DMDS in the charge, the hydrodesulphurisation is total. The hydrogenolysing activity of the catalyst relative to the pyridine is very good, but enters into competition with the hydrogenation activity relative to the naphthalene. Hydrogenolysing activity relative to pyridine is understood to mean the conversion of pyridine to ammonia and pentane. The hydrogenating and hydrogenolysing action of the oxyhydride catalyst hardly varys with hydrogen pressure. This is important because it indicates that it would be possible to hydrogenate naphthalene, pyridine, DMDS, thiophene and other aromatic products during different hydrotreatments of the mineral-oil charges, such as hydrocracking, hydrodesulphurisation, hydroisomerisation and hydrogenation, at low hydrogen pressures, whilst with the other catalysts currently being used it is necessary to work at high hydrogen pressures. The use of oxyhydrides as hydrogenation catalysts is therefore advantageous not only from the technical but also from the economic point of view. Example 26 This Example illustrates the reduction of naphthalene (2% by weight in n-heptane), in the presence of 0.1% by weight of DMDS, at 350°C, at different hydrogen pressures of between 80 and 150 bar, with a feed rate of 20 g/hour and a hydrogen flow rate of 3 litres/hour, the catalyst weight being 24 g. This Example differs essentially from Example 19 in the nature of the catalyst used. In fact MmNi 5 O 1.7 H 8 , prepared by process A (from the corresponding hydride), used in Example 19, was replaced by CeNi 5 O 2 H 4.45 prepared from cerium and nickel nitrates in the proportions 1:5, by process (B), by evaporation and precipitation, followed by calcination at 450°C, then reduction and inclusion of hydrogen at 300°C. The results are shown in Table III. H₂ pressure (bar) Conversion of Naphthalene (%) Hydrogenation Activity of Naphthalene (%) 80 53.2 23.5 100 52.6 23.3 125 55.9 25.8 150 51.8 24.4 These results confirm those in Example 19, namely that the activity of the catalyst does not vary with hydrogen pressure. This example also shows that the catalyst used, which is here a synthetic oxyhydride, obtained by preparative process (B), from nitrates of ace and Ni, and purchased commercially, give results similar to those obtained using as a catalyst an oxyhydride prepared by process (A) from the corresponding hydride. Example 27 (Pilot Plant Hydrogenation) This Example demonstrates the resistance to sulphur poisoning of the rare earth oxyhydrides, since the catalyst used in this Example is submitted to a very high concentration of H₂S. CeNi₅O y H x as produced by preparative process (B) was used as catalyst. Its surface area was 40 m²/g and its hydrogen content (x) was 4.4. A feed (nC₇ + 2% naphthalene + z% pyridine + w% DMDS was hydrogenated in a pilot installation with hydrogen under the following conditions:- T (react.) = 350°C P (H₂) = 80 barg Reactor vol. = 20 cc Feed flow = 20 g/h Hydrogen flow = 2 litres/hour Catalyst weight = 23.1 g The results obtained are shown in Table IV. Pyridine/feed (z %) 2 2 2 0 0 0 2 DMDS/feed (w %) 0.1 1 2 2 15 2 2 Time on stream (h) 225 97 48 142 3 191 64 Naphthalene conv. (% g⁻¹) 1.4 0.26 0.23 0.95 1.2 1.2 0.2 Pyridine conv. (% g⁻¹) 0.8 1.25 1.2 - - - 1.3 Total conv. (% g⁻¹) 2.2 1.51 1.43 0.95 1.2 1.2 1.5 Example 28 This Example demonstrates the effect of hydrogen pressure on the hydrogenation activity of naphthalene, pyridine and quinoline. CeNi₅O y H x produced by preparative procedure (C) was used as catalyst. Its surface area was 72 m²/g and its hydrogen content (x) was 8.0. A feed [(i) nC₇ + 2% naphthalene + 2% pyridine + 2% DMDS (ii) nC₇ + 4% quinoline + 2% DMDS] was hydrogenated in a pilot installation with hydrogen under the following conditions:- T (react) = 350°C P (H₂) = 80 - 150 barg Reactor vol. = 20 cc Feed flow = 20 g/h Hydrogen flow = 2 litres/h Catalyst weight = 18.4 g The results obtained are shown in Table V. Example 29 This Example provides a comparison between a commercial catalyst (ex Procatalyse) and two different rare earth oxyhydride catalysts (one obtained by preparative process (B) and the second by preparative process(C)). The catalysts used were as follows:- A - Commercial catalyst, ex Procatalyse (NiPS₂). B - CeNi₅O y H x wherein x = 4.4 and having a surface area of 40 m²/g prepared by process (B) (nitrates evaporation). C - CeNi₅O y H x wherein x = 8.0 and having a surface area of 72 m²/g prepared by process (C) (TEA precipitation). A feed (nC₇ + 2% naphthalene + 2% pyridine + z% DMDS) was hydrogenated in a pilot plant installation with hydrogen under the following conditions: T (react) = 350°C P (H₂) = 80 barg Reactor vol. = 20 cc Feed flow = 20 g/h Hydrogen flow = 2 litres/h Catalyst weight = ± 20 g The results obtained are shown in Table VI. Example 30 This Example demonstrates the hydrotreatment of a vacuum distillate (D cut Arab medium) in a batch reactor. The catalyst used was CeNi₅OyH x . A feed consisting of a D cut Arab medium vacuum distillate was hydrogenated in a batch reactor under the conditions shown in Table VI.

Claims: A process for the hydrogenation of an unsaturated organic compound by contacting the compound with a solid hydrogenation catalyst under hydrogenation conditions characterised in that the solid hydrogenation catalyst comprises a rare earth oxyhydride having the formula: Tr 1-q G q Ni 5-p M p O y H x (I) wherein Tr is a rare earth element, G is either Th and/or Y, M is a metal selected from the group consisting of Cu, Mn, Al, Fe, Cr, Co, Rh, Ru, Re, Pt, Pd, Ir, Os, Mo, V, Ti, W and mixtures of two or more thereof, q is zero or a number less than or equal to 1, p is zero or a number less than or equal to 5, y is a whole number or decimal number in the range from 0.4 to 6.5, and x is zero or a whole number or decimal number equal to or less than 15 and with the proviso that the process is other than the hydrogenation of isoprene in the presence of an oxyhydride having the stoichiometry MmNi 5 O 1.7-w (NO 3 ) 2w H 8 and a specific surface area of approximately 20 m²/g. A process according to claim 1 wherein the unsaturated organic compound is an olefinically unsaturated compound. A process according to either claim 1 or claim 2 wherein the unsaturated compound is selected from olefins, monocyclic aromatic hydrocarbons, polycyclic aromatic hydrocarbons, heterocyclic aromatic hydrocarbons containing nitrogen in the aromatic ring and heterocyclic aromatic hydrocarbons containing sulphur in the aromatic ring, or a mixture of two or more thereof. A process according to claim 1 wherein the unsaturated organic compound is isoprene. A process according to claim 1 wherein the unsaturated organic compound is naphthalene. A process according to claim 1 wherein the unsaturated organic compound is pyridine. A process according to claim 1 wherein the unsaturated organic compound is thiophene. A process according to claim 1 wherein the hydrogenation process is a hydrotreatment of a mineral oil-derived feedstock. A process according to claim 8 wherein the hydrotreatment is either hydrocracking, hydrodesulphurisation, hydrodenitrification, hydroisomerisation or hydrogenation. A process according to any one of the preceding claims wherein the process is operated in the presence of additional hydrogen. A process according to any one of the previous claims wherein there is used a catalyst of the formula (I) wherein Tr is Mischmetal. A process according to any one of claims 1 to 10 wherein there is used a catalyst of the formula (I) wherein Tr is cerium. A process according to any one of claims 1 to 10 wherein there is used a catalyst of the formula (I) wherein Tr is lanthanum. A process according to any one of claims 1 to 10 wherein there is used a catalyst of the formula (I) wherein Tr is praeseodymium. A process according to any one of claims 1 to 10 wherein there is used a catalyst of the formula (I) wherein Tr is neodymium. A process according to any one of the preceding claims wherein the rare earth oxyhydride is prepared by a process comprising the steps as follows:- in a first step subjecting an IREC of the formula: Tr 1-g G g Ni 5-p M p (XI) in a closed reactor, preferably an autoclave, to a plurality of hydriding/dehydriding cycles thereby to form a hydride, the hydriding being performed under a hydrogen pressure of from 20 to 200, preferably from 50 to 100 bar, and at a temperature of from 20 to 450°C, preferably about 350°C, and the dehydriding being performed in the same closed reactor at a temperature in the range from 20 to 450°C, in a second step oxidising the hydrided product obtained in the first step, and in a third step chemically reducing the product obtained in the second step. A process according to any one of claims 1 to 15 wherein the rare earth oxyhydride is prepared by a process comprising the steps as follows:- in a first step forming a solution comprising soluble salts of nickel and the other metallic element(s) thermally decomposable to the oxides thereof in such proportions as to satisfy the stoichiometric relationship of formula (I), and thereafter precipitating a mixture of the thermally decomposable salts of nickel and the other element(s), in a second step partially or wholly thermally decomposing the mixture of heat decomposable salts obtained in the first step, and in a third step reducing the product obtained in the second step in the present of hydrogen. A process according to any one of claims 1 to 15 wherein the rare earth oxyhydride is prepared by the method of claim 17 in which precipitation of the mixture of the thermally decomposable salts of nickel and the other element(s) is accomplished by adding the solution of salts portionwise to an excess of the base under conditions of efficient mixing, thereby to effect precipitation at constant pH. A process for the production of a rare earth oxhydride of formula (I) which process comprises the steps as follows:- in a first step forming a solution comprising soluble salts of nickel and the other metallic element(s) thermally decomposable to the oxides thereof in such proportions as to satisfy the stoichiometric relationship of formula (I), and thereafter precipitating a mixture of the thermally decomposable salts of nickel and the other element(s) by adding the solution of the salts portionwise to an excess of a basic solution under conditions of efficient mixing, thereby to effect precipitation at constant pH, in a second step partially or wholly thermally decomposing the mixture of heat decomposable salts obtained in the first step, and in a third step reducing the product obtained in the second step in the presence of hydrogen.

Inventors: BONNELLE, JEAN-PIERRE, MARCQ, JEAN PHILLIPPE, PINABIAU, MARYSE
Applicants: THE BRITISH PETROLEUM COMPANY P.L.C.
Application year: 1987
Main classification: C07B35
IPC codes: B01J23, C01B6, C10G49, C07C5