IRON OXIDE/MAGNESIUM OXIDE COMPOSITES AND METHOD FOR DESTRUCTION OF CHLORINATED HYDROCARBONS USING SUCH COMPOSITES

Abstract: Finely divided composite materials are provided comprising a first metal oxide (e.g., MgO) at least partially coated with an extremely thin layer of a second metal oxide such as Fe2O3. The composites have a high surface area and are very effective for the destructive adsorption of undesirable fluids in gaseous or liquid form, such as chlorocarbons and clorofluorocarbons. In use, a fluid stream including undesirable fluids are contacted with the composites of the invention, such as through the use of a filter containing the composite as a part of the filter media thereof.

Description: IRON OXIDE/MAGNESIUM OXIDE COMPOSITES AND METHOD FOR DESTRUCTION OF CHLORINATED HYDROCARBONS USING SUCH COMPOSITES Background of the Invention 1. Field of the Invention The present invention is broadly concerned with finely divided (preferably nanoscale) composite materials which have significant utility in the destruction of chlorocarbons, fluorocarbons and other toxic or undesir¬ able fluids. More particularly, the invention pertains to composite materials including first metal oxide particles, preferably MgO, at least partially coated with an extreme¬ ly thin layer of a second metal oxide such as Fe 2 0 3 . Composites in accordance with the invention have greatly enhanced abilities to destructively adsorb undesirable fluids such as gases or liquids. 2. Description of the Prior Art The increasing amounts of chlorocarbons and chlorofluorocarbons in the environment has given rise to the need to find easy and effective ways to destroy these gases without producing toxic byproducts . The most widespread groups of chlorinated compounds are the poly- chlorinated biphenyls (PCBs) which have extremely high thermal stabilities and are used as lubricants, heat transfer fluids, plasticizers, and transformer fluids; and cleaning solvents such as CC1 4 , CHC1 3 , and C 2 C1 4 . Addi¬ tionally, large stores of obsolete or overaged pesticides, herbicides, mixed wastes and nerve gases exist around the world, and the safe and effective destruction of these materials is of increasing concern. These considerations have prompted a number of investigations to determine the most feasible way of handling and destroying various undesirable substances . Some of these destructive techniques involve incineration 95/27679 PC17US95/03562 or catalytic oxidation. Another approach depends on surface active reagents that strip heteroatoms from the toxic gases and allow only the release of non-toxic hydrocarbons or carbon oxides. For example, the destruc- tive adsorption of organophosphorus compounds on MgO causes the phosphorus atoms to be immobilized as a strong¬ ly bound residue, with the only volatile organic products being CH 3 OH and HCOOH. This same chemistry has been applied to the destruction of chlorocarbons using reac- tants such as MgO or CaO. While destructive adsorption techniques appear promising and have favorable thermodynamics, the cost thereof has been considerable, owing principally to the fact that, to be effective, the adsorptive reagents must be very finely divided for maximum surface area. More¬ over, these reactions are non-catalytic and depend entire¬ ly upon molecular reactions at the surface of the re¬ agents. This is accordingly a real and unsatisfied need in the art for improved destructive adsorption reagents which have enhanced destructive efficiencies. Summary of the Invention The present invention overcomes the problems outlined above and provides finely divided composite materials useful for the destructive adsorption of a wide variety of undesirable fluids (i.e., materials in either gaseous or liquid form) , such as chlorocarbons, chloro- fluorocarbons, polychlorinated biphenyls, pesticides, herbicides, mixed wastes and nerve gases. Broadly speak¬ ing, the composites of the invention comprise finely divided particles of a first metal oxide selected from the group consisting of MgO, CaO, A1 2 0 3 , Sn0 2 , Ti0 2 , and mix¬ tures thereof, these particles being at least partially coated with a quantity of a second metal oxide selected fro the group consisting of Fe 2 0 3 , Cu 2 0, NiO, CoO and mixtures thereof. In preferred forms, the first metal oxide is advantageously selected from the group consisting of MgO and CaO, whereas the second oxide is preferably Fe 2 0 3 . For most efficient usages, the particles of the first metal oxide should be single crystallites or polycrystallite aggregations and should have an average size of up to about 20 nm, and more preferably from about 4-10 nm; the second metal oxide should be in the form of an extremely thin layer or coating applied onto the surface of the first metal oxide, giving an average overall size for the composite of up to about 21 nm, and more preferably from about 5-11 nm. The bulk composites of the invention should have an average surface area of at least about 100 m 2 /g, and more preferably from about 300-500 m 2 /g. Generally, the first metal oxide should be present in substantial excess relative to the second oxide. Thus, the first metal oxide comprises from about 90-99% by weight of the total composite material, and more preferably from about 95-99% by weight. Correspondingly, the second metal oxide should comprise from about 1-10% by weight of the total composite, and more preferably from about 1-5% by weight. The coverage of the first oxide by the second oxide should be quite extensive, e.g., at least about 75% of the surface area of the first metal oxide particles should be covered with the second oxide, and more preferably from about 90-100% of this surface area should be covered. The composites of the invention are preferably fabricated by first forming the very finely divided first particulate material using known aerogel techniques. Thereafter, the second material is applied onto the surface of the first oxide as an extremely thin layer, e.g., a monolayer having a thickness on the order of less than 1 nm. For example, MgO nanoscale particles can be prepared, and are then treated with an iron salt such as iron III (acetylacetonate) 3 with the ligands being driven off by heating. The composites of the invention can be used for the destruction of unwanted fluids, especially gases in a gas stream, although the invention is not limited to destruction of gases. The method may involve passing a fluid stream through a filtering device including the composite material therein. In practice, the concentra¬ tion of the unwanted fluids should be from about 0.3-1.3 g of the unwanted fluids for each gram of the composite material used for destructive adsorption. Generally, to be effective, the composites hereof should be heated during contact with the fluids to be destructively ad¬ sorbed. This elevated temperature should be at least about 300°C, and more preferably from about 400-600°C, in the case of materials such as the chlorocarbons, fluoro¬ carbons and nerve gases. In order to destructively adsorb other materials such as the PCBs, higher temperatures may be required on the order of 600-800°C. Although not wishing to be bound by any theory, it is believed that the second or outer oxide plays a catalytic role in the destructive adsorption process, via a mechanism referred to as spillover catalysis. For example, when CC1 4 attacks the surface of an MgO/Fe 2 0 3 composite, it is believed that a disassociative adsorption occurs, probably with the intermediacy of chemisorbed CC1 2 . At this point, C0C1 2 may form as an intermediate which goes on to react in a similar mode to produce C0 2 and FeCl x . However, the important point is that the FeCl x formed must quickly exchange (spillover) Cl " with 0 2" in such a way that Cl " is driven into the bulk of the first oxide while 0 2~ comes to the surface. Brief Description of the Drawings Figure 1 is a schematic representation of the apparatus used in the production of Fe 2 0 3 /MgO composites of the invention; Fig. 2 is a schematic representation of appara¬ tus used in the chlorocarbon decomposition tests using the composites of the invention; Fig. 3 is the infrared spectra of the gaseous products of CC1 4 reacted with MgO (Graph a) and Fe 2 0 3 /MgO (Graph b) , at a sample/CCl 4 molar ratio of 3:1; Fig. 4 is the infrared spectra of the gaseous products of CC1 4 reacted with MgO (Graph a) and Fe 2 0 3 /MgO (Graph b) , at a sample/CCl 4 molar ratio of 6:1; Fig. 5 is the infrared spectra of the gaseous products of CC1 4 reacted with MgO (Graph a) and Fe 2 0 3 /MgO (Graph b) , at a sample/CCl 4 molar ratio of 10:1; Fig. 6 is the infrared spectra of the gaseous products of CC1 4 reacted with MgO (Graph a) and Fe 2 0 3 /MgO (Graph b) , at a sample/CCl 4 molar ratio of 13:1; Fig. 7 is a gas chromatograph plot illustrating the percentage composition of gaseous products from the reaction between 0.1 g MgO and CC1 4 with respect to the microliters CC1 4 injected at 400°C sample temperature; and Fig. 8 is a gas chromatograph plot illustrating the percentage composition of gaseous products from the reaction between 0.1 g Fe 2 0 3 /MgO and CC1 4 with respect to the microliters CC1 4 injected at 400°C sample temperature. Detailed Description of the Preferred Embodiments The following examples illustrate preferred embodiments of the invention and use thereof . It is to be understood, however, that these examples are presented by way of illustration only and nothing therein should be taken as a limitation upon the overall scope of the inven- tion. Example 1 A. Preparation of MgO Highly divided nanoscale MgO samples were prepared by the autoclave treatment described by Utamapanya et al. , Chem. Mater., 3:175-181 (1991) . In this procedure, 10% by weight magnesium methoxide in methanol solution was prepared and 83% by weight toluene solvent was added. The solution was then hydrolyzed by addition of 0.75% by weight water dropwise while the solution was stirred and covered with aluminum foil to avoid evaporation. To insure completion of the reaction, the mixture was stirred overnight. This produced an aerogel which was treated in an autoclave in using a glass lined 600 ml capacity Parr miniature reactor. The gel solution was placed within the reactor and flushed for 10 minutes with nitrogen gas, whereupon the reactor was closed and pressurized to 100 psi using the nitrogen gas. The reactor was then heated up to 265°C over a 4 hour period at a heating rate of l°C/min. The temperature was then allowed to equilibrate at 265°C for 10 minutes. At this point, the reactor was vented to release the pressure and vent the solvent (final reactor pressure was about 700 psi) . Finally, the reactor was flushed with nitrogen gas for 10 minutes. This produced fine white powdery magnesium hydroxide having a surface area on the order of 1000 m 2 /g which was then thermally converted to MgO as explained below. B. Preparation of Fe-,0./MgO Composites The Mg(OH) 2 particles were first thermally converted to MgO, followed by deposition of iron oxide to provide the complete composite. The apparatus employed for this operation is set forth in Fig. 1. This apparatus 10 includes a reactor 12 for holding a quantity of the powdered magnesium hydroxide, with a shiftable magnetic stirrer 14 positioned below the reactor and operable to rotate a stirrer bar 16. The apparatus further includes a mercury-filled 50 ml gas burette 18, manometers 20 and 21, a helium source 22 coupled with a molecular sieve 13X trap 24, and a septa 26 operably coupled with reactor 12. A vacuum line 28 is also provided which is coupled via conduit and valve assembly 30 to the remainder of the apparatus 10 as shown. Also, the reaction 12 is equipped with an external, electrically controlled heater 31. The initial thermal conversion of magnesium hydroxide to MgO was carried out by heating the magnesium hydroxide in reactor 12 under dynamic vacuum conditions at an ascending temperature rate to a maximum temperature of 500°C, which was held for 6 hours. Most of the dehy¬ dration was found to occur at temperatures between 200°C and 320°C. IR and X-ray diffraction studies confirmed virtually complete conversion of the Mg(OH) 2 to MgO. Iron oxide was deposited on the nanoscale MgO particles by carrying out a direct reaction between activated MgO and iron III (acetylacetonate) 3 , in tetrahydrofuran at room temperature under helium (1 atm.) . In a typical preparation, 0.3 g of Mg(OH) 2 was heated under vacuum (10 ~3 Torr.) in the reactor 12 at an ascending temperature rate of l°C/min. to 500°C, which was held for 6 hours to assure complete conversion to MgO, followed by cooling to room temperature. The evacuated system was then filled with He at 1 atm. pressure, and stirring was commenced using stirrer 14 and bar 16, the latter being magnetically shifted to the bottom of reactor 12. Two ml of 0.25 M iron III (acetylacetonate) 3 in THF solution (previously prepared under argon by dissolving 4.5 g of iron III (acetylaceton¬ ate) 3 in 50 ml THF) was introduced to the reactor 12 by a syringe through a septa 26. The amount of iron III (acetylacetonate) 3 solution used provided the MgO surfaces with 1.4 iron III (acetylacetonate) 3 molecules for each surface OH group. The concentration of surface OH groups for the autoclave-prepared MgO was found to be 3.6 OH groups/nm 2 . The reaction mixture in reactor 12 was stirred overnight to allow a complete reaction at room tempera- ture. The reacted Fe 2 0 3 /MgO composite was then removed from the reactor 12, filtered using regular filter paper, washed with THF to remove any residuals of iron III (acetylacetonate) 3 , and dried in air for 10 minutes. IR spectra of the resultant dried product showed bands for the acetylacetonate species, indicating the existence of some acetylacetonate ligands bound to the surfaces of the MgO. This product was heated again under vacuum (10 ~3 Torr.) at 500 °C to remove these ligands. C. Chlorocarbon Decomposition Using MgO and the Fe 2 0 ? /MgO Composite Two different studies were carried out to investigate and compare the efficiency of activated MgO and Fe 2 0 3 /MgO samples in decomposing CC1 4 . Previous investigations using CaO for CC1 4 destruction indicated that the best decomposition occurs at 400°C. Therefore, in the following two systems, the reaction temperature was 400°C. In the first IR and XRD (X-Ray Diffraction) study, the apparatus of Fig. 2 was employed. This appara¬ tus 32 included two Schlenk tubes 34, 36 respectively containing the MgO or Fe 2 0 3 /MgO composite and dry CC1 4 , a calibrated 0.1 ml vial 38 and a vacuum source 40. A conduit and valve assembly 42 interconnected the source 40 with the tubes 34, 36 and vial 38 as shown. Also, tube 34 and vial 38 were equipped with external liquid nitrogen immersion containers 44, 46 for selective cooling of the contents of the tube 34 and vial 38. In test procedures, the MgO or Fe 2 0 3 /MgO was heated by means not shown in Fig. 2 under vacuum (10 "3 Torr.) for complete activation (3 hours for a 0.2 g sample) , with the CC1 4 vessel remaining closed via the appropriate valve. Next, 0.1 ml CC1 4 was collected in the calibrated vial 38 using external cooling via liquid nitrogen container 46, and by opening the valve adjacent the tube 36. After the CC1 4 was collected in vial 38, and tube 34 had sufficiently cooled, the external liquid nitrogen container 44 was employed to further cool the contents of tube 34, and the valve adjacent tube 34 was opened. This resulted in transfer of the CC1 4 from vial 38 to tube 34 (the above steps were repeated when more than 0.1 ml of CC1 4 was needed) . In practice, different molar ratios of MgO or Fe 2 0 3 /MgO to CC1 4 were reacted for subse¬ quent testing. The tube 34 containing the MgO or Fe 2 0 3 /MgO and the added CC1 4 was closed and heated at 400°C for 9 hours. Next, the CC1 4 tube 36 was replaced by an IR gas cell with KBr windows, followed by evacuation (10 ~3 Torr.) of the system with the valve associated with tube 34 still closed. The tube 34 was then opened by opening the adjacent valve, in order to transfer the gases produced from the reaction to the IR cell. After each such experi¬ ment, an IR spectrum was recorded for the gaseous product, and an XRD spectrum was recorded for the solid products. IR spectra of the gaseous products showed bands for C0 2 , C 2 C1 4 , C0C1 2 , CC1 4 , and weak bands for HC1 and CO gases (Figs. 3-6) . As indicated from the band intensi¬ ties, the composition of these products changes as the sample/CCl 4 ratio changes. At low sample CC1 4 molar ratio 3:1) , all of these gases are produced. As the ratio increases, the sample becomes in excess and decomposes all of the CC1 4 and the intermediate products, COCl 2 and HC1. Comparing the spectra of the MgO and Fe 2 0 3 /MgO reaction products, the following results are manifest. 1. The disappearance of COCl 2 (phosgene) in the case of Fe 2 0 3 /MgO was faster than in the case of MgO (Fig. 4) as the ratio was increased, which means that Fe 2 0 3 /MgO produces less phosgene at all ratios. 2. The production of C 2 C1 4 was generally higher in the reaction of Fe 2 0 3 /MgO. 3. The most striking feature was that the remaining (undecomposed) CC1 4 was less in reaction of Fe 2 0 3 /MgO as shown by the less intense bands of CC1 4 in the case of Fe 2 0 3 /MgO at all ratios, especially at ratios of 6 : 1 and 10 :1. These confirm that Fe 2 0 3 composites are more efficient for destruction of CC1 4 , in terms of decomposing more CC1 4 , and producing less COCl 2 gas. The X-Ray diffraction spectra of the solid products showed patterns for MgCl 2 , hydrated MgCl 2 and MgO. The hydration of some MgCl 2 was due to the exposure of the samples to air during the XRD experiments. Comparing the spectra of the reaction products of the Fe 2 0 3 /MgO composite systems with the reaction products of the MgO systems, it was determined that : 1. At low molar ratios (3:1 and 6:1) , MgO is a major component in the reaction products of the MgO systems, while it disappears almost completely in the reaction products of the Fe 2 0 3 /MgO systems. 2. Fe 2 0 3 /MgO systems produce more MgCl 2 than do the MgO systems, as shown by the stronger patterns of MgCl 2 in the spectra of the Fe 2 0 3 /MgO systems. 3. Thus, more CC1 4 reacted with the Fe 2 0 3 /MgO composites, as compared with the same amount of MgO, thereby confirming the greater efficiency of the Fe 2 0 3 /MgO composites. In a second GC (gas chromatography) study, the gases produced from the rapid reaction between a series of 1 μL injections (2 min. apart) of CC1 4 through 0.1 g of MgO or Fe 2 0 3 /MgO composite at 400°C. For this test, a 0.1 g sample of MgO or Fe 2 0 3 /MgO composite was packed in a U- shaped stainless steel reactor using glass wool and glass beads on other side or the sample to hold it in place. The reactor was connected to the column of a GC instrument (TCD GC Series 580, GOW-MAC Instrument Co. ) , and heated to 400°C over 1 hour. The instrument was calibrated at a column and injector temperature of 100°C. He was used as a carrier gas at a flow rate of 0.5 cm/s. CC1 4 was injected in 1 μL portions over the heated sample and the results were recorded after each injection for the gases coming out of the reaction tube. The main gaseous products detected were C0 2 , C 2 C1 4 and unreacted CC1 4 , as identified by a mass spectrometer connected to the GC instrument . Gas chromatography was used to study the gaseous products of a short duration reaction between 0.1 g of MgO or Fe 2 0 3 /MgO and a series of 1 μL portions of CC1 4 injected over the sample at 400°C allowing 2 minutes between injections. The main gaseous products detected were C0 2 , C 2 C1 4 , and the unreacted CC1 4 as identified by a mass spectrometer connected with a GC instrument in a separate system. Generally, C0 2 gas was the major product along with traces of C 2 C1 4 in the first few CC1 4 injections. After a certain number of injections, CC1 4 became in excess and started to appear with the reaction products. The concentration of CC1 4 increased slowly with injections of more CC1 4 until the sample was saturated and unable to decompose more CC1 4 , as shown in Figs. 7-8. As more CC1 4 was injected, the C0 2 and C 2 C1 4 production decreased but they continued to form after the saturation of the sample, which indicated that some decomposition continued to take place under these conditions. The results of two typical experiments using MgO and Fe 2 0 3 /MgO samples were illus- trated in Figs. 7 and 8, where the percent composition of the gaseous products is plotted with respect to the amount of CC1 4 injected. The percentage of each gas was measured by the percentage of its peak height after each injection. The number of injections in which CC1 4 did not appear with the products gives the amount of CC1 4 complete¬ ly decomposed by a 0.1 g sample. The efficiency of Fe 2 0 3 /MgO composites in decomposing CC1 4 was compared with that of MgO by carrying out the reaction with CC1 4 on the same amount of both samples (0.1 g) under the same condi- tions. In all of the experiments carried out, the differ¬ ence in the behavior of both samples toward CC1 4 was great . In the MgO reaction (Fig. 7) , CC1 4 was completely decom¬ posed in the first 3 injections and the sample was satu¬ rated with 15 μL of CC1 4 . In contrast, the Fe 2 0 3 /MgO sample was saturated with 75 μL of CC1 4 and 49 μL were completely decomposed. Depending on these results the sample/CCl 4 molar ratio for complete CC1 4 decomposition was 80:1 and 5:1 for MgO and Fe 2 0 3 /MgO respectively. In other words, to decompose 1 mole of CC1 4 , we need 80 moles of MgO or 5 moles of Fe 2 0 3 /MgO. Another difference was that C 2 C1 4 was not produced from the first 10 injections in the Fe 2 0 3 /MgO system and C0 2 was the only product, while it was produced from the first injection in the MgO reaction. This confirms that the Fe 2 0 3 /MgO composites are very much more efficient in terms of decomposing CC1 4 and producing more C0 2 , as compared with MgO. D. Effect of Iron Content The GC apparatus was also used to determine the effect of varying the iron content in the Fe 2 0 3 /MgO compos- ites insofar as CC1 4 destruction is concerned. It was determined that the amount of iron deposited on the MgO surface increased the efficiency of the composites. Table 1 sets forth the amount of CC1 4 completely decomposed by Fe 2 0 3 /MgO composites having differing amounts of iron, where the GC experiments were carried out as set forth above. Table 1 %Fe (by weight) uL of CC1. Completely Decomposed 0 3 1.7 21 2.1 38 2.2 49 E. Effect of Other Reactants The preferred Fe 2 0 3 /MgO composites were compared with other related samples by GC testing as described above. The other samples were: MgO mixed with iron III (acetylacetonate) 3 using different amounts of iron; MgO mixed with c.-Fe 2 0 3 using different amounts of iron; straight c.-Fe 2 0 3 ; and straight iron III (acetylacetonate) 3 . Table 2 below sets forth the amounts of CC1 4 (in μL) completely decomposed by 0.1 g of different samples at 400°C. Table 2 Sample % Fe 0% 1 . 7 2 . 1 2 . 2 2 . 5 5 . 0 q, % % "o % Fe 2 0 3 /MgO 3 21 38 49 - - MgO/Fe ( aca- 3 - - 24 - 23 c ) 3 MgO/α-Fe 2 0 3 1 3 - - - 5 - α- Fe 2 0 3 11 Fe ( acac ) 3 13 X A physical mixture of separate MgO and α-Fe 2 0 3 particles F. The Effect of Time Between Injections The time between CC1 4 1 μL injections in the GC test described above was found to have a significant influence on the efficiency of the Fe 2 0 3 /MgO composite samples in reacting with CC1 4 . The results of this series of experiments, carried out using different time periods between CC1 4 injections, but with all other conditions constant, is set forth in Table 3. Table 3 μL of CC1 4 Completely Decomposed Time (minutes) Sample A* Sample B* 2 24 30 5 40 - 10 - 60 *A and B are typical Fe 2 0 3 /MgO samples The significant increase in the reactivity of Fe 2 0 3 /MgO toward CC1 4 by increasing the time between CC1 4 injections indicates that longer times help the sample to regenerate it surface structure and potential. This means that Cl/O exchange process goes toward completion if longer time is allowed. Based on these tests, the de¬ scribed spillover catalysis mechanism is proposed. When short time intervals between CC1 4 injections were used, two things might happen to inhibit the Cl/O exchange: first, the Fe-Cl/Fe-0 exchange may not occur for all of the surface Fe-Cl bonds. Second, the exchange process would be expected to start with oxygen ions in the outer layers of MgO particles, which will be blocked with Cl ions after a short time, covering the bulk oxygen ions. When longer time intervals were used, these problems were somewhat alleviated: first, enough time was allowed for a complete Fe-Cl/Fe-0 exchange on the surface; second, the Cl ions accumulating in the outer layers migrate over time, uncovering more 0 "2 ions for the exchange process. Example 2 In this example, a CaO/Fe 2 0 3 composite was prepared and tested for its ability to destructively adsorb chlorocarbons. The apparatus employed was identi¬ cal to that shown in Fig. 1. Commercially available Ca(OH) 2 was first thermally activated to CaO under the dynamic vacuum and heating conditions recited in Example 1 to yield CaO having a surface area of about 100-120 m 2 /g. The CaO was then stirred for several hours in a tetra- hydrofuran solution of iron III (acetylacetonate) 3 under argon at the conditions of Example 1. The THF was then removed under vacuum, leaving an orange solid. This solid was heat treated again to 500°C to drive off the acetyl¬ acetonate ligands . A gray/black powder resulted due to the carbon present. The composite was then stored and handled in a dry box to prevent reaction with moisture. X-ray diffraction studies of the sample detected from the atmosphere showed only the presence of CaO. The CaO/Fe 2 0 3 composite was tested for destruct¬ ive adsorption of CC1 4 and found to be very efficient for this purpose.

Claims: Claims : 1. A finely divided composite material com¬ prising particles of a first metal oxide selected from the group consisting of MgO, CaO, Al 2 0 3 , Sn0 2 , Ti0 2 and mixtures thereof, said particles being at least partially coated with a quantity of a second metal oxide selected from the group consisting of Fe 2 0 3 , Cu 2 0, NiO, CoO and mixtures thereof. 2. The composite material of claim 1, said particles having an average size of up to about 20 nm. 3. The composite material of claim 2, said average being from about 4-10 nm. 4. The composite material of claim 1, said composite having an average surface area of at least about 100 m 2 /g. 5. The composite material of claim 4, said average surface area being from about 300-500 m 2 /g. 6. The composite material of claim 1, said first metal oxide comprising from about 90-99% by weight of the total composite material. 7. The composite material of claim 6, said first metal oxide comprising from about 95-99% by weight of the total composite material . 8. The composite material of claim 1, said second metal oxide comprising from about 1-10% by weight of the total composite material. 9. The composite material of claim 8, said second metal oxide comprising from about 1-5% by weight of the total composite material. 10. The composite material of claim 1, said first metal oxide being MgO, and said second metal oxide being Fe 2 0 3 . 11. The composite material of claim 1, said second metal oxide being applied as a thin layer having a thickness of up to about 1 nm. 12. A method of destroying unwanted fluids in a fluid stream, comprising the step of contacting said fluid stream with a quantity of a finely divided composite material comprising particles of a first metal oxide selected from the group consisting of MgO, CaO, Al 2 0 3 , Sn0 2 , Ti0 2 and mixtures thereof, said particles being at least partially coated with a quantity of a second metal oxide selected from the group consisting of Fe 2 0 3 , Cu 2 0, NiO, CoO and mixtures thereof. 13. The method of claim 12, said unwanted fluid being selected from the group consisting of chlorocarbons, chlorofluorocarbons, toxic heteroatom compounds and mixtures thereof. 14. The method of claim 12, the concentration of said unwanted gases being from about 0.30 g to 1.3 g for each gram of said composite material. 15. The method of claim 12, including the step of heating said composite material prior to said contact¬ ing step. 16. The method of claim 15, wherein said composite material is heated to a temperature of at least about 100°C. 17. The method of claim 12, said contacting step comprising the step of passing said fluid • stream through a filtering device, said filtering device includ¬ ing said composite material therein. 18. The method of claim 12, said particles having an average size of up to about 20 nm. 19. The method of claim 18, said average being from about 4-10 nm. 20. The method of claim 12, said composite having an average surface area of at least about 100 m 2 /g. 21. The method of claim 20, said average surface area being from about 300-500 m 2 /g. 22. The method of claim 12, said first metal oxide comprising from about 90-99% by weight of the total composite material . 23. The method of claim 22, said first metal oxide comprising from about 95-99% by weight of the total composite material. 24. The method of claim 12, said second metal oxide comprising from about 1-10% by weight of the total composite material. 25. The method of claim 24, said second metal oxide comprising from about 1-5% by weight of the total composite material . 26. The method of claim 12, said first metal oxide being MgO, and said second metal oxide being Fe 2 0 3 .

Inventors: KHALEEL ABBAS, KLABUNDE KENNETH J, KHALEEL, ABBAS, KLABUNDE, KENNETH, J.
Applicants: KHALEEL ABBAS, KLABUNDE KENNETH J, UNIV KANSAS STATE, KANSAS STATE UNIVERSITY RESEARCH FOUNDATION, KHALEEL, ABBAS, KLABUNDE, KENNETH, J.
Application year: 1995
Main classification: C01B7
IPC codes: A62D3, B01D53, B01J20, B01J23, B01J37, C01B7, C01B13, C01F5, C01F7, C01F11