Patent Publication Number: US-4482641-A

Title: Metal-containing active carbon and method for making same

Description:
BACKGROUND OF THE INVENTION 
     1. Field of the Invention 
     This invention relates generally to active carbon having a metal component and more particularly concerns a substantially uniform dispersion of a metal component in a porous carbon matrix having a high surface area and a method for making same. 
     2. Description of the Prior Art 
     It is known that the presence of metals in active carbon can greatly enhance the efficiency and selectivity of the active carbon when it is employed in catalytic, sorption, or filtering applications. Wennerberg et al., U.S. Pat. No. 4,082,694 disclose a high surface area active carbon material which has a cage-like structure exhibiting a microporosity which contributes to over 60 percent of its surface and which has an effective BET surface area of greater than about 2,300 square meters per gram and a bulk density greater than about 0.25 gram per cubic centimeter. Wennerberg et al., disclose a process for making such high surface area active carbon by first heating an agitated combination of solid potassium hydroxide containing between 2 and 25 weight percent water and a carbonaceous material comprising coal coke, petroleum coke or a mixture thereof below about 483° C., then heating the resulting dehydrated product at a temperature between 705° C. and 983° C. to thereby form active carbon, and finally cooling the resulting activated product and removing essentially all of the inorganic material therefrom by water washing to form the high surface area active carbon end product. Wennerberg et al., U.S. Pat. Nos. 3,642,657 and 3,817,874 and Wennerberg, U.S. Pat. No. 3,726,808 disclose related methods for making high surface area active carbon products. 
     Attempts to incorporate metal compounds into activated carbon by conventional physical impregnation techniques have been problematical. One disadvantage with physical impregnation of activated carbon with metal compounds is that the small pores at the surface of the active carbon particles are inaccessible to liquid penetration and prevent penetration of the liquid, metal-containing impregnating solutions, thereby rendering impossible uniform and thorough impregnation of the carbon particles with metal. Furthermore, physical impregnation of the active carbon causes partial blocking of the pores of the carbon particles resulting in an appreciable reduction of the active surface area thereof. In addition, it is not possible to control to any large extent the total quantity of the metal applied to the active carbon particles by impregnation and its distribution on and in the carbon particles, with the end result that there is a substantial risk that the metal will crystallize and agglomerate in an undesirable manner on the carbon particles. 
     Several techniques have been proposed to overcome the problems associated with impregnating active carbon with metal compounds. For example, Dimitry, U.S. Pat. No. 3,886,093 discloses activated carbons having uniformly distributed active metal sites and a method for making such activated carbons. The method of Dimitry involves mixing an aqueous solution of a lignin salt with an aqueous solution of a transition metal salt to precipitate the transition metal and lignin as a metal lignate. The transition metal must be capable of forming a chemical bond with the lignin and in so doing precipitating the lignin from solution as a metal lignate. Dimitry discloses that the time required to complete the precipitation is less than one hour and that usually 30 minutes is sufficient for this purpose. According to Dimitry, suitably the wet metal lignate precipitate can then be dried in a spray drier. The precipitate is then carbonized at a temperature between 371° C. and 983° C. and finally activated at a temperature between 760° C. and 1065° C. Dimitry states that, although drying the metal lignate precipitate is not critial to form an activated carbon product, drying is necessary to form a high surface area end product. However, Dimitry gives neither a general disclosure nor a specific example of what it means by a &#34;high surface&#34; area for its end product. Dimitry states that the active metal sites are uniformly distributed throughout the activated carbon end product and presents an electron micrograph of an activated carbon end product magnified 5,700 times. However, from this relatively low magnification micrograph, the distribution of the active metal sites in the activated carbon end product is not readily apparent. 
     Furthermore, Siren, U.S. Pat. No. 4,242,226  states that the metal content in the active carbon which can be achieved by pyrolysis and activation of a metal lignate precipitate is much too low for the majority of fields of use and that it is difficult using such technique to predetermine the properties of the resulting metal-containing active carbon end product owing to the substantially undefined structure of the lignin. Siren disclosed an alternative technique in which a cation of calcium, magnesium, barium, aluminum, copper or a transition metal and an anionic group chemically bound to a polyhexose derivative are caused to react in solution, and the resulting product is precipitated either spontaneously or by adding a suitable precipitating agent. Siren discloses that, after separating the precipitate from solution, the precipitate can, if desired, be dried, for example, by spray drying. Thereafter the separated reaction product is pyrolyzed and activated using conventional techniques to form the activated carbon. In the method of Siren, suitably the polyhexose derivative employed comprises an acid polyhexose derivative and preferably the anionic groups of the polyhexose derivative comprise carboxylic acid groups, sulfonic acid groups or phosphoric acid groups. Preferably the polyhexose derivatives contain from 1 to 3 metal cations per hexose unit. 
     However, techniques such as those of Dimitry and Siren which require the occurrence of a chemical reaction between the metal cation and the carbonaceous anion in solution and the precipitation in solution of the resulting reaction product impose severe limitations on the metal-containing active carbon end products which can be obtained. For example, only those metals or metal compounds can be incorporated into the active carbon structures which are available in forms which can react chemically with the carbonaceous anion in solution and which thereby produce reaction products with either precipitate spontaneously or can be precipitated by the addition of a precipating agent to the solution. Furthermore, limitations are imposed on the amount of metal or metal compounds that can be incorporated into the active carbon matrix by the stoichiometry of the reaction between the metal cation with the carbonaceous anion in solution. In addition, limitations on the uniformity of the distribution of the metal or metal compounds in the active carbon end product are imposed by factors which are intrinsic to any process involving conventional precipitation of a salt from solution. Such factors include co-precipitation and post-precipitation as well as irregularities in the nature of the crystal formed and in the rate of crystal growth in solution as a result of the concentration of the salt being precipitated, the excess concentration of either the cationic or anionic portion of such salt, the solution temperature, the time period over which precipitation occurs, the presence, concentration and relative solubilities of other materials in solution, and the changes in any of these factors during the course of the precipitation process. 
     OBJECTS OF THE INVENTION 
     It is therefore a general object of the present invention to provide an improved metal-containing active carbon and a method for making same to meet the aforementioned requirements and to solve the aforementioned problems. 
     More particularly it is an object of the present invention to provide an improved metal-containing active carbon having a substantially uniform dispersion of a metal or metal-containing material throughout the carbon matrix and a method for making same. 
     A related object of the present invention is to provide an improved metal-containing active carbon without significant metal crystal size development. 
     Another object of the present invention is to provide an improved metal-containing active carbon having high porosity and surface area. 
     An additional object of the present invention is to provide an improved catalytically active metal-containing active carbon. 
     Other objects and advantages of the invention will become apparent upon reading the following detailed description and appended claims, and upon reference to the accompanying drawings. 
     SUMMARY OF THE INVENTION 
     These objects are achieved by an improved method of this invention for making a substantially uniform dispersion of a metal or metal-containing material in a porous carbon matrix, which comprises: forming a uniform co-crystallite of a precursor of the metal or metal-containing material and of a carbon precursor, wherein the metal in the precursor of the metal or of the metal-containing material is a transition metal or a metal from Groups IIIA, IVA or VA of the Periodic Table of the Elements; forming a uniform powdered mixture of the co-crystallite and organic solids comprising an alkali metal hydroxide; pyrolizing the powdered mixture in an inert atmosphere at a temperature in the range of from about 400° C. to about 980° C. to form the carbon matrix having the metal or metal-containing material substantially uniformly dispersed therein; and separating unreacted inorganic material and inorganic reaction products other than the dispersed metal or metal-containing material from the porous carbon matrix. The present invention is also the product formed according to this method. 
     The present invention is also an active carbon composition comprising a substantially uniform dispersion of a metal or metal-containing material in a porous carbon matrix, wherein the weight ratio of the metal or metal-containing material to active carbon matrix is from about 1:10,000 to about 1:1, based on the weight of the metal or metal-containing material, respectively, and having a cage-like structure and a BET surface area of at least 800 square meters per gram and a bulk density of at least 0.1 gram per cubic centimeter. 
    
    
     BRIEF DESCRIPTIONS OF THE DRAWINGS 
     For a more complete understanding of this invention, reference should now be made to the embodiment illustrated in greater detail in the accompanying figures and described below by way of examples of the invention. In the figures: 
     FIG. 1 is a phase contrast, electron microscope photomicrograph at a relatively low total magnification (×250,000) of an active carbon formed by the method of this invention in which the rate of temperature increase in the pyrolysis step was 66.5° C. per minute; 
     FIG. 2 is a phase contrast, electron microscope photomicrograph at a relatively high total magnification (×2,900,000) of an active carbon formed by the method of this invention in which the rate of temperature increase in the pyrolysis step was 66.5° C. per minute; 
     FIG. 3 is a phase contrast, electron microscope photomicrograph under a total magnification of ×250,000 of an active carbon formed by the method of this invention in which the rate of temperature increase in the pyrolysis step was 66.5° C. per minute and thereafter subjected to thermal treatment to recrystallize the dispersed metal-containing material; 
     FIG. 4 is a phase contrast, electron microscope photomicrograph under a total magnification of ×250,000 of an active carbon formed by the method of this invention in which the rate of temperature increase in the pyrolysis step was 11° C. per minute; and 
     FIG. 5 is a phase contrast, electron microscope photomicrograph under a total magnification of ×250,000 of a prior art active carbon having platinum deposited thereon. 
     It should be understood, of course, that the invention is not necessarily limited to the particular embodiments illustrated herein. 
    
    
     DETAILED DESCRIPTION OF THE DRAWINGS INCLUDING PREFERRED EMBODIMENTS 
     Suitable carbon precursors for use in the method of this invention include aromatic carboxylic acids, phenols, aromatic amines and salts of any such materials. In addition, when the inclusion of sulfur in the final porous carbon matrix is acceptable, aromatic sulfonic acids and aromatic thiols and salts of such materials can also be employed as the carbon precursor. Preferably, metal salts of the aforesaid aromatic carboxylic acids, aromatic sulfonic acids, phenols and aromatic thiols are employed as the carbon precursors in the present invention. 
     The aforesaid aromatic acid may be any compound having an acid radical directly or indirectly attached to the benzene ring. The acid radical may be COOH, SO 3  H, SO 2  NH 2 , PO 3  H, etc. Other functional groups may be present without deleterious effect. Aromatic carboxylic acids are preferred and may be simple monocarboxylic acids, such as benzoic acid, or polycarboxylic acids, such as terephthalic, isophthalic, trimesic, and trimellitic, or polynuclear carboxylic acids, such as naphthoic acid, or polynuclear polycarboxylic acids, such as coke acids. It is also contemplated that the aromatic carboxylic acids may be derived from any suitable carbonaceous material which is subsequently oxidized to form the carboxylic acid. The feed material may be treated, when necessary or desired, to remove contaminants or undesirable elements. For example, petroleum coke has a metal content, but oxidation of petroleum coke with nitric acid serves the dual function of forming coke acid and removing metals. While petroleum coke acid having any degree of oxidation is suitable in the method of this invention, the preferred petroleum coke acid is one having an elemental oxygen content of between about 20 to 30 weight percent. 
     Suitable precursors of the metal or metal-containing material for use in the formation of the co-crystallite in the method of this invention include salts or complexes of a transition metal or of a metal from Groups IIIA, IVA or VA of the Periodic Table of the Elements on page 846 of Webster&#39;s New Collegiate Dictionary, 1979. 
     Any technique can be employed to form the co-crystallite in the method of this invention which affords uniform co-crystallization--that is, simultaneous crystallization--of the carbon precursor and the precursor of the metal or metal-containing material and the formation of a substantially uniform co-crystallite thereof. Homogeneity of the co-crystallite mixture is essential to the ultimate formation of a uniform dispersion of the metal or metal-containing material in high surface area active carbon. A strongly preferred technique to form the uniform co-crystallite of the carbon precursor and precursor of the metal or metal-containing material in the method of this invention involves the formation of a stable solution of both such precursors in a suitable solvent and spray drying such solution to dryness. In such technique, solvent removal must be carried out rapidly enough to maximize rapid, simultaneous and homogeneous co-crystallization of both precursors from solution. Spray drying provides the desired rapid evaporation to insure rapid, simultaneous and uniform co-crystallization and formation of a homogeneous co-crystallite of both precursors. 
     In a spray drying system which is suitable for use in carrying out the spray drying step in a preferred embodiment of the method of this invention, a solution of the carbon precursor and of the precursor of the metal or metal-containing material is introduced into a drying chamber through a nozzle. A hot inert gas such as nitrogen is introduced into the drying chamber through a line which surrounds the nozzle and serves to assist in atomizing the solution entering the drying chamber through the nozzle, to accelerate and raise the temperature of the atomized solution droplets and thereby to promote substantially instantaneous evaporation of solvent therefrom to afford a homogeneous co-crystallite powder. Air is introduced into the drying chamber to sweep the co-crystallite powder and nitrogen downward in the drying chamber where the bulk of the co-crystallite powder falls to the bottom of the drying chamber, where it collects and from which it is later removed for use in the subsequent steps of the method of this invention. Gas passes from the drying chamber and then to a cyclone system where co-crystallite powder entrained in the gas stream is separated from the gas and passes downward through a line for collection. 
     In the spray drying technique, it is of course essential that stable solutions of the carbon precursor and precursor of the metal or metal-containing material be employed. Although it is preferred that a single solution containing dissolved carbon precursor and precursor of the metal or metal-containing material be employed, it is also suitable to employ separate solutions, with one containing the dissolved carbon precursor and the other containing the dissolved precursor of the metal or metal-containing material. When two such solutions are employed, the two solutions are mixed upstream of the aforementioned nozzle and aspirated together into the aforementioned drying chamber. Although any convenient solvent can be employed, water is the preferred solvent. 
     In the spray drying technique, forms of each of the carbon precursor and of the precursor of the metal or metal-containing material which are both soluble in the solvent used or each soluble in one or the other of the solvents used must be employed. Variables which can be controlled to effect the necessary solubility of both precursors in the same solvent or of each precursor in a different solvent include the pH of the solvents, the concentration of the precursors in the solvents, and the forms in which the precursors are introduced into the solvents--for example, the identity of the salt or complex of the precursor of the metal or metal-containing material. Water soluble forms of the carbon precursor include potassium, sodium, rubidium and ammonium salts of aromatic carboxylic and sulfonic acids, phenols and aromatic thiols in an alkaline aqueous solution and aromatic amine hydrochlorides in an acidic aqueous solution. 
     Table 1 contains a list of merely a few illustrative examples of water-soluble metal salts and complexes which serve as precursors of metals and metal-containing materials in the method of this invention. 
     
                       TABLE 1                                                     
______________________________________                                    
                     Metal or Metal-                                      
Precursor            Containing Material                                  
______________________________________                                    
K.sub.2 Cr.sub.2 O.sub.7                                                  
                     Cr.sub.2 O.sub.3                                     
NaAlO.sub.2          Al.sub.2 O.sub.3                                     
Na.sub.2 SiO.sub.3   SiO.sub.2                                            
KMnO.sub.4           MnO.sub.2                                            
Na.sub.2 WO.sub.4 ; (NH.sub.4).sub.2 WO.sub.4                             
                     W.sub.2 O.sub.3                                      
K.sub.2 MoO.sub.4 ; (NH.sub.4).sub.2 MoO.sub.4                            
                     MoO.sub.2                                            
Co(NH.sub.3).sub.4 Cl.sub.2, Cobalt                                       
                     CoO, Co                                              
phenolate complex                                                         
Cu(NH.sub.3).sub.4 Cl.sub.2                                               
                     CuO, Cu                                              
Ni(NH.sub.3).sub.4 Cl.sub.2                                               
                     NiO, Ni                                              
Ag(NH.sub.3).sub.2 Cl                                                     
                     Ag.sub.2 O, Ag                                       
Ferric phenolate complex                                                  
                     Fe.sub.2 O.sub.3, Fe                                 
RhCl.sub.3 complexes with glycine                                         
                     RhO.sub.2, Rh                                        
or EDTA                                                                   
PdCl.sub.2 complexes with glycine,                                        
                     PdO, Pd                                              
EDTA or hydroxyquinoline                                                  
H.sub.2 PtCl.sub.6 complexes with glycine,                                
                     PtO, Pt                                              
EDTA or NH.sub.3                                                          
______________________________________                                    
 
    
     After the co-crystallite is formed, the co-crystallite powder is intimately mixed with the inorganic solids comprising an alkali metal hydroxide. Preferably at least 25 weight percent of the inorganic solids is the alkali metal hydroxide. Although not intending to limit the scope of the present invention by any theoretical explanation, the role of the alkali metal hydroxide in the formation of the active carbon of the present invention is believed to occur by reaction with the carbon precursor during pyrolysis to thereby propagate the formation of active carbon. The particle size of the inorganic solids need only be sufficiently small to insure that the inorganic solids disperse well enough in the co-crystallite powder that an intimate mixture is formed. The weight ratio of alkali metal hydroxide-to-co-crystallite in the resulting mixture is from about 1:1 to about 5:1, preferably from about 2:1 to about 4:1 and more preferably from about 2.5:1 to about 3.5:1. 
     Although a hydroxide of any metal of Group IA of the Periodic Table can be mixed with the co-crystallite in the method of this invention, potassium hydroxide is strongly preferred. In addition to its ready availability and relative low cost, potassium hydroxide is advantageous because unless potassium hydroxide is employed, it is extremely difficult to obtain a metal-containing active carbon end product having a surface area of at least 1,000 square meters per gram, without additional treatment being required. Furthermore, as will be discussed hereinbelow, potassium hydroxide is preferred because it is highly soluble in water and its carboxylate salts are highly soluble in water. 
     Preferably the alkali-metal hydroxide is hydrated. The water of hydration serves to assist in lowering the fusion temperature of the alkali metal hydroxide and in producing a uniform melt of the co-crystallite and alkali metal hydroxide in the pyrolysis step before pyrolysis occurs, to thereby facilitate mixing of the alkali metal hydroxide and co-crystallite before reaction occurs. Preferably the alkali metal hydroxide contains from 2 to 25 weight percent of water of hydration. 
     The inorganic solids can comprise, in addition to the alkali metal hydroxide, an alkali metal salt such as an alkali metal halide, carbonate, sulfate, phosphate, nitrate or oxide. Preferably potassium is the alkali metal in the alkali metal halide, carbonate, sulfate, phosphate, nitrate or oxide. In one embodiment of the method of this invention, some or all of the alkali metal salt is mixed with the carbon precursor and precursor of the metal or metal-containing material prior to or during formation of the co-crystallite, for example, in the spray drying step. 
     In the method of this invention, the intimate mixture of co-crystallite powder and inorganic solids is then pyrolyzed under an inert atmosphere such as nitrogen gas. The pyrolysis temperature is selected to be high enough to decompose the carbon precursor and less than the graphitization temperature of carbon, that is, from about 400° C. to about 980° C., preferably from about 700 ° C. to about 900° C. The rate of temperature increase to which the mixture of co-crystallite and inorganic solids is subjected in the pyrolysis chamber is preferably at least 35° C. per minute and more preferably at least 300° C. per minute. Such rates of temperature increases of at least several hundred degrees centigrade per minute are readily attainable with microwave heating. Higher rates at which the temperature of the mixture is raised from ambient temperature to the final pyrolysis temperature effectively neutralizes the tendency toward the formation of separate phases as a result of differences in the temperatures and rates at which the carbon precursor and precursor of the metal or metal-containing material pyrolyze. Such phase separation is manifested by relatively larger crystal growth for the metal or metal-containing material dispersed in the active carbon end product and thus is detectable by a relative increase in the crystallite size and by relative decreases in the uniformity of dispersion of the metal or metal-containing material and of the accessible surface area of the dispersed metal or metal-containing material. 
     Following the pyrolysis step, while still under a blanket of inert gas, the pyrolysis chamber and its contents are cooled and the powdered pyrolysis product is suspended in a suitable liquid, preferably water, in the blanketed pyrolysis chamber and then transferred as a slurry to a receiver. The solvency of the slurry liquid must be controlled to insure that the dispersed metal or metal oxide does not dissolve in the slurry liquid. For example, when substantially neutral water is employed as the slurry liquid, the resulting slurry of the powdered pyrolysis product is alkaline and has a pH of about 12. Under these conditions, if the metal dispersed in the active carbon is in the form of an amphoteric metal oxide, the metal oxide would dissolve in the water and would thereby be removed from the active carbon. For example, dispersed Al 2  O 3 , SiO 2 , WO 3 , MoO 3 , V 2  O 3  and SnO 2  would dissolve as KAlO 2 , K 2  SiO 3 , K 2  WO 4 , K 2  MoO 4 , KVO 3  and K 2  SnO 2 , respectively. Since it is necessary to prevent solubilization of the dispersed metal oxide in such cases, the pH of the water would have to be reduced to about 7.0-8.0 with a suitable acid solution such as acetic acid, or vapor such as carbon dioxide or acetic acid vapor, before being used to rinse and slurry the powdered pyrolysis product. 
     The slurry is then filtered to separate the powdered pyrolysis product from the slurry liquid. Thereafter the powdered product is purified by repeated washings with a suitable solvent, preferably water, to remove the alkali metal therefrom and yet to leave undissolved the dispersed metal or metal-containing material in solid form in the active carbon matrix. When water is used as the wash solvent and when the dispersed metal is in the form of an amphoteric metal oxide, the pH of the water should be from 7 to 8 to insure dissolution of the alkali metal in the water but to prevent dissolution of the dispersed metal oxide. Since potassium salts are more soluble than the corresponding salts of the other alkali metals, it is highly preferred that potassium is the alkali metal in the alkali metal hydroxide and in any alkali metal salt mixed with the co-crystallite prior to the pyrolysis step to facilitate removal thereof from the active carbon end product. 
     Thereafter the powdered product is dried using any conventional and suitable drying technique. 
     The active carbon of the instant invention has a cage-like structure which contributes preferably to over sixty percent of its surface and, more preferably, to over 80 percent of its surface and, most preferably, to over 90 percent of the carbon surface, as measured by phase contrast, high resolution electron microscopy. This cage-like structure is characterized in that the individual cages are of a size to exhibit properties of microporosity, that is, essentially complete filling of the individual cages by the adsorbate at low effective concentration to give a large micropore volume. The cages in the cage-like structure are substantially homogeneous in size as can be seen by the relatively low magnification image photomicrograph (×250,000) taken by phase contrast, high resolution electron microscopy on a Hitachi model HU-12 electron microscope supplied by Hitachi and shown in FIG. 1. Using a JEOL model 100C electron microscope at high magnification (×2,900,000), the individual cages are clearly evident and appear to be formed using single sheets of graphitic-type lamellae, as shown in FIG. 2. This cage-like structure is responsible for the multi-layer adsorption demonstrated by the carbons of this invention and the extremely large effective surface areas as measured by the BET method. 
     The active carbon product preferably has an effective BET surface area greater than about 800 square meters per gram, more preferably, greater than about 1,600 square meters per gram, and, most preferably, greater than about 2,000 square meters per gram. The active carbon preferably has a bulk density which is preferably greater than about 0.1 gram per cubic centimeter and, more preferably, greater than about 0.2 gram per cubic centimeter. 
     Any transition metal or metal of Groups IIIA, IVA or VA of the Periodic Table of the Elements or any combination thereof or a material containing any such metal or combination can be dispersed in the active carbon matrix in the composition of the present invention. Preferably the dispersed metal and the metal in the dispersed metal-containing material is platinum, palladium, rhodium, molybdenum, chromium, aluminum, silicon, tungsten, iron, cobalt, nickel, silver or copper. Preferably the dispersed metal-containing material is a metal oxide. The weight ratio of the dispersed metal or metal-containing material-to-the active carbon matrix in the composition of this invention is preferably from 1:10,000 to 1:1, based on the weight of the metal or metal-containing material, respectively. 
     The dispersed crystallites of metal or metal-containing material in the active carbon matrix of the composition of this invention appear in FIGS. 1 and 2 as black spots on the walls of the cage-like structures shown therein. The darkening of the photomicrographs in FIGS. 1 and 2 in areas further removed from the edges of the carbon matrix indicate increasing thicknesses of the matrix, not increasing size of the dispersed metal or metal-containing material. Although the crystallite size of the dispersed metal or metal-containing material depends on the metal, the form in which it is dispersed, and the rate of increase of temperature to which the mixture of co-crystallite powder and inorganic solid were subjected during the pyrolysis step of the method of this invention, the average crystallite size of the dispersed metal or metal-containing material is generally in the range of from about 5 Å to about 30 Å of the dispersed metal or molecules of the dispersed metal-containing material. For example, when a precursor of platinum is employed in the method of this invention, and when the rate of temperature increase in the pyrolysis step is at least 35° C. per minute, the platinum is dispersed in the end product predominantly as platinum metal having an average crystallite size equivalent to from 5 Å to 15 Å of platinum metal. 
     The composition of the present invention possesses substantially improved resistance to thermally or chemically induced sintering or recrystallization of the dispersed metal or metal-containing material to form a dispersed material of relatively larger crystallite size and relatively lower effective surface area. Upon exposure to high temperatures, for example, 900°-1150° C. for 12 hours, or to certain chemical treatments, for example, with 106 percent phosphoric acid for 65 hours at 200° C., the crystals of dispersed metal or metal-containing material recrystallize to form larger crystals. FIG. 3 contains a micrograph illustrating the dispersed crystals after prolonged exposure to 1,021° C. of the same active carbon end product of this invention shown in FIGS. 1 and 2. Comparison of FIGS. 1 and 3, both at the same magnification, illustrates that some of the dispersed crystals have increased in size as a result of the thermal treatment. The larger crystals in FIG. 3 are formed from smaller crystals of the type illustrated in FIG. 1 by aggregation of the smaller crystals. 
     The rate of temperature increase in the pyrolysis step leading to the formation of the active carbon shown in FIG. 4 was 11° C. per minute. Comparison of FIGS. 1 and 4 illustrates that the crystals shown in FIG. 1 are smaller than those in FIG. 4 and that the use of a relatively higher rate of temperature increase in the pyrolysis step in the method of this invention affords a product having dispersed therein a metal or metal-containing material of relatively smaller average crystallite size. 
     FIG. 5 contains an electron micrograph at a magnification of ×250,000 of an active carbon matrix containing 5 weight percent platinum which had been deposited thereon by impregnation, supplied by Engelhardt Industries of Springfield, N.J. The micrograph in FIG. 5 illustrates as dark spots the crystallite size of the impregnated platinum, which is substantially larger than the crystallite size of the dispersed platinum in the composition of this invention. 
     The micrographs in FIGS. 3-5 were obtained using the same electron microscope used to obtain the micrograph in FIG. 1. 
     The dried end product of the method of this invention generally has a particle size in the range of from about 25 to about 28 microns and in that size range is suitable for use in many applications. However, in certain applications such as a catalyst for use in a packed or fluidized bed, it may be desirable or necessary to employ larger particles. 
     A suitable, low cost granular activated carbon having a high surface area and a suitable particulate form with sufficient crush strength and abrasion resistance comprises a clay binder which is capable of forming a high viscosity gel when dispersed in water, for example, the montmorillonite clays. When using activated carbon, the montmorillonites enable the carbon to retain a high percentage of its effective surface area. In fact, the loss of effective surface area due to the presence of the clay binder is only about equal to the relative percentage of clay binder present. Hence, for a granular activated carbon containing 15 weight percent montmorillonite, the effective surface area would be only about 15 percent less than the effective surface area of the powdered activated carbon used as the starting material. The aforesaid granular activated carbon containing clay binder may be prepared in any size or shape desired. A characteristic of the granular activated carbon containing montmorillonite clay binder is that it retains throughout the fabricated form the average pore size of the powdered carbon starting material. Such granular activated carbons are also characterized by a good high temperature strength and crush strength. The weight ratio of activated carbon to clay binder in such granular activated carbon is from about 90:10 to about 70:30, on a dry basis. 
     A suitable process for preparing the aforesaid granular activated carbon comprises the steps of: (a) blending the activated carbon with a powdered montmorillonite clay binder in the presence of sufficient water to achieve a composition having from about 30 to about 40 weight percent solids and a carbon:binder weight ratio of from about 90:10 to about 70:30; (b) compounding the composition to achieve dispersion of the clay binder in the aqueous phase and penetration of the resulting aqueous-binder phase into the interstitial spaces between the activated carbon particles; (c) extruding the composition through an orifice to form an extrudate; (d) drying the extrudate at a maximum temperature of about 191° C. in a manner so as to minimize the shock effects of rapid water evaporation from the porous carbon and secondary carbon surface oxidation by water vapor; and (e) curing the extrudate at a temperature sufficient to effect a physical-chemical change in the extrudate which is manifested by increased hardness and stability. 
     Suitable curing temperatures are from about 774° C. to about 1038° C., preferably in the range from about 899° C. to about 927° C. 
     Drying is preferably accomplished by a gradual increase in temperature to minimize the effects of water evaporation on the strength of the carbon structure. A time-temperature profile which has been found effective comprises air drying the extrudate material at increasing temperatures wherein the temperature is increased at a rate of about 2.8° C. permitted until a drying temperature of 94° C. is reached. Thereafter the temperature is increased at a rate of 5.5° C. permitted until a maximum drying temperature of 191° C. is reached. Total drying time is from about 45 minutes to about 1 hour. The resulting water content is about 2 weight percent. 
     In the alternative, the active carbon of this invention can be granulated with alumina using the procedure exemplified in Example 9 hereinbelow. 
     It may also be desirable in certain instances to reduce the particle size of the metal-containing active carbon of this invention below the aforesaid range of 25-28 microns. In such cases, the active carbon end product of the method of this invention can be milled by any convenient method to small particle sizes. A major advantage of the uniform distribution of metal or metal-containing material in the method of this invention is that reduction of the particle size by milling or attrition does not affect the distribution of the dispersed metal component within the active carbon or on its exterior surface and hence of the availability or accessibility of the dispersed metal component. 
     The composition of this invention is useful for all the uses to which prior art active carbon compositions have been put, for example, as sorbents in such applications as water treatment and gas and vapor adsorption. In addition, the composition of the present invention is useful as a support for catalysts, or as a catalyst itself, for example, to catalyze hydrogen transfer reactions involving hydrocarbons. 
     While the invention is described in connection with the specific examples below, it is to be understood that these are for illustrative purposes only. Many alternatives, modifications and variations will be apparent to those skilled in the art in the light of the below examples and such alternatives, modifications and variations fall within the scope and spirit of the appended claims. 
     EXAMPLE 1 
     6.53 grams of chloroplatinic acid (H 2  PtCl 6 .6H 2  O) were introduced into 1100 grams of water, and 6 grams of ethylenediamine tetraacetic acid (EDTA) were introduced to 100 grams of water. Sufficient amounts of a dilute solution of ammonium hydroxide were addes to the aqueous solution of EDTA as necessary to raise the pH of the solution to 8 and to thereby form a stable solution of the ammonium salt of EDTA. When the solutions of chloroplatinic acid and of the EDTA salt were combined, a stable solution of the complex of the chloroplatinate anion with the ammonium salt of EDTA was formed. 
     166 grams of terephthalic acid were introduced to 2200 grams of water and dissolved therein as ammonium terephthalate by the addition of sufficient amounts of a concentrated solution of ammonium hydroxide to raise the pH of the resulting solution to 8.0-8.5. The solutions of the complex of the chloroplatinate salt with the EDTA salt and of the terephthalate salt were then combined to form a stable homogeneous solution at 21°-29° C. The combined solution was then spray dried using the procedure described above with respect to FIG. 1 to yield finely divided co-crystallite powder of potassium terephthalate and potassium chloroplatinate. 
     20 grams of the co-crystallite powder were then dry blended with 54.06 grams of 90 percent potassium hydroxide powder and 59.89 grams of potassium carbonate powder in a Waring blender to produce 134 grams of a uniform powdered mixture. This entire powdered mixture was transferred to a rotating quartz calcining tube equipped for continuous argon purge, placed in a tubular furnace, and preheated to 650° C. The temperature of the powdered mixture rose at a rate of 66.7° C. per minute to 650° C. The quartz tube remained in the furnace during its heat up and during the one hour period at 650° C., during which time the powdered mixture pyrolized to form a powdered pyrolysis product and after which tine the tube was withdrawn from the furnace and allowed to cool to ambient temperature. The quartz tube and its contents were maintained under a blanket of argon throughout the period before introduction of the powdered mixture into the quartz tube, during the pyrolysis and during cool down of the quartz tube and its contents to ambient temperature. While still under an argon blanket, the cooled pyrolysis product was rinsed with water from the cooled quartz tube. After separation from the water, the pyrolysis product was repeatedly washed with water to remove the potassium salts therefrom, until a resulting wash water had a pH of 7. A final wash with a solution of 1 weight percent of acetic acid in water was performed to remove the last traces of potassium salts from the pyrolysis product. The resulting washed pyrolysis product was dried in a vacuum oven at 105° C. under a nitrogen blanket. 
     The resulting dried pyrolysis product weighed 6.0 grams, had a BET surface area of 2744 square meters per gram and contained 3.66 percent of platinum by weight, based on the weight of the pyrolysis product. Electron micrographs of the dried pyrolysis product are shown in FIGS. 1 and 2. The platinum was predominantly in the form of elemental platinum. The platinum had a surface area of 11.0 square meters per gram as determined by CO chemisorption, and 99.03 percent of the platinum had an average crystallite size less than 35 Å, as determined by X-ray diffraction. 
     Thermal sintering of the powdered pyrolysis product at 1021°-1150° C. for a period of 12 hours resulted in recrystallization of a portion of the dispersed platinum as manifested by crystal growth of 26 weight percent of the dispersed platinum to an average crystallite size of about 105 Å. An electron micrograph of the sintered pyrolysis product is shown in FIG. 3. In addition, contacting of the powdered pyrolysis product with 106 percent phosphoric acid for 65 hours at 200° C. resulted in recrystallization of the dispersed platinum as manifested by crystal growth of 30 weight percent of the dispersed platinum to an average crystallite size of 60 Å. 
     EXAMPLE 2 
     The procedure of Example 1 was repeated, with the difference of inserting the powdered mixture of co-crystallite, potassium hydroxide and potassium carbonate into the purged quartz tube at ambient temperature and then inserting the tube into the furnace. The temperature of the tube&#39;s contents rose at a rate of 11.1° C. per minute, instead of 66.7° C. per minute, from ambient temperature to 650° C. 
     The resulting dried pyrolysis product weighed 6.0 grams, had a BET surface area of 2164 square meters per gram and contained 3.97 percent of platinum by weight, based upon the weight of the pyrolysis product. An electron micrograph of the dried pyrolysis product is shown in FIG. 4. The platinum was predominantly in the form of elemental platinum. The platinum had a surface area of 9.0 square meters per gram as determined by CO chemisorption, and 83.87 percent of the platinum had an average crystallite size less than 35 Å, as determined by X-ray diffraction. 
     Thermal sintering of the powdered pyrolysis product at 1021°-1150° C. for a period of 12 hours resulted in recrystallization of the dispersed platinum as manifested by crystal growth of 100 percent of the dispersed platinum to an average crystallite size of 135 Å. In addition, treatment of the powdered pyrolysis product with 106 percent phosphoric acid for 65 hours at 200° C. resulted in recrystallization of the dispersed platinum as manifested by crystal growth of 98 percent of the dispersed platinum to an average crystallite size of 60 Å. 
     EXAMPLE 3 
     The procedure of Example 1 was repeated with the following exceptions. Instead of concentrated ammonium hydroxide, 120 grams of potassium hydroxide were added to the terephthalic acid solution to solubilize the terephthalic acid as potassium terephthalate. Instead of the solution containing chloroplatinic acid, a stable solution of a complex of the palladium cation with the potassium salt of EDTA was formed by introducing 0.832 gram of palladium chloride (in the form of H 2  PdCl 4 ) into 150 grams of water containing the potassium salt of EDTA formed by neutralizing 20 grams of EDTA to a pH of 8.0 with an aqueous solution of potassium hydoxide. Instead of introducing the powdered mixture of co-crystallite, potassium hydroxide and potassium carbonate into the purged quartz tube at 650° C., the tube was at ambient temperature as in Example 2, and the temperature of the tube&#39;s contents rose at a rate of 11.1° C. per minute from ambient temperature to 650° C. 
     The resulting dried pyrolysis product weighed 3.4 grams, had a BET surface area of 3433 square meters per gram, and contained 1.00 percent of palladium by weight, based on the weight of the pyrolysis product. The palladium was predominantly in the form of elemental palladium. The dispersed palladium had a surface area of 0.65 square meters per gram, as determined by CO chemisorption, and 82 percent (0.82 weight percent based on the weight of the pyrolysis product) of the palladium had an average crystallite size less than 35 Å. Thermal sintering of the pyrolysis product at 1021° C. for a period of 12 hours resulted in recrystallization of the palladium as manifested by crystal growth of 100 percent of the dispersed palladium to an average crystallite size of 118 Å. 
     EXAMPLE 4 
     The procedure of Example 1 was repeated with the following exceptions. An aqueous solution of potassium terephthalate formed as in Example 3 was used in place of the ammonium terephthalate solution formed as in Example 1. Instead of the solution of the complex of the chloroplatinate anion employed in Example 1, a stable aqueous solution of Ni(NH 3 ) 4  (acetate) 2  was formed by neutralizing 11.09 grams of Ni(acetate) 2 .4H 2  O was neutralized with ammonium hydroxide in 150 milliliters of water. The resulting dried pyrolysis product weighed 6.0 grams, had a BET surface area of 2085 square meters per gram, and contained 1.21 percent of nickel by weight, based on the weight of the pyrolysis product. The nickel was predominantly in the form of elemental nickel. 76 weight percent of the dispersed nickel had a crystallite size less than 35 Å. 
     EXAMPLE 5 
     The procedure of Example 4 was repeated, with the difference of inserting the powdered mixture of co-crystallite, potassium hydroxide and potassium carbonate into the purged quartz tube at ambient temperature and then inserting the tube into the furnace. The temperature of the tube&#39;s contents rose at a rate of 11° C. per minute instead of 66.7° C. per minute. The resulting dried pyrolysis product weighed 6.0 grams, had a BET surface area of 2445 square meters per gram, and contained 1.3 percent of nickel by weight, based on the weight of the pyrolysis product. The nickel was predominantly in the form of elemental nickel. 22 percent of the dispersed nickel had a crystallite size of less than 35 Å. 
     EXAMPLE 6 
     0.65 gram of chloroplatinic acid (H 2  PtCl 6 .6H 2  O) was dissolved in 250 grams of water and 0.627 gram of rhodium chloride (RhCl 3 .3H 2  O) was dissolved in 250 grams of water, and the two solutions were combined. To this solution was then added a solution of 3 grams of glycine in 100 grams of water neutralized to a pH of 8 with potassium hydroxide, to form stable complexes of glycine with the chloroplatinate anion and the rhodium cation. 166 grams of terephthalic acid were introduced into 2200 grams of water and dissolved therein as potassium terephthalate by the addition thereto of 75 grams of 90 percent potassium hydroxide and then the adjustment of the pH to 8. The solution of the glycine complexes and of potassium terephthalate was then combined to form a stable homogeneous solution at 21°-29° C. The combined solution was then spray dried to yield 222 grams of finely-divided co-crystallite powder of potassium terephthalate, rhodium chloride and potassium chloroplatinate. 
     20 grams of the co-crystallite powder were then dry blended with 54.06 grams of 90 percent potassium hydroxide powder and 59.89 grams of potassium carbonate powder in a Waring blender to produce 134 grams of a uniform powdered mixture. This entire powdered mixture was transferred to a rotating quartz calcining tube equipped for continuous argon purge and at ambient temperature. The quartz tube containing the powdered mixture was then placed into a tubular furnace which had been preheated to 650° C. The temperature of the contents of the tube rose at a rate of 11.1° C. per minute to 650° C. The quartz tube remained in the furnace at 650° C. for one hour, during which time the powdered mixture pyrolyzed to form a powdered pyrolysis product and after which time the tube was withdrawn from the furnace and allowed to cool to ambient temperature. The quartz tube and its contents were maintained under a blanket of argon throughout the period before introduction of the powdered mixture into the quartz tube, during the pyrolysis and during cool down of the quartz tube to ambient temperature. While still in the quartz tube under an argon blanket, the cooled pyrolysis product was suspended in water and transferred as a slurry from the tube to a beaker. After separation from the water, the pyrolysis product was repeatedly washed with water to remove potassium salts therefrom, as indicated by a pH of 7 for the resulting wash water. The resulting washed pyrolysis product was dried in a vacuum oven at 105° C. under a nitrogen blanket. The resulting dried pyrolysis product weighed 3.1 grams, had a BET surface area of 2579 square meters per gram and contained 3.5 percent of each of platinum and rhodium by weight, based on the weight of the pyrolysis product. The results of X-ray diffraction indicated that the platinum and rhodium were present predominantly as the elemental metals and in the form of a platinum-rhodium alloy containing 59 atomic percent of rhodium and 41 atomic percent of platinum. The alloy had a surface area of 1.13 square meters per gram, as determined by CO chemisorption, and 0.77 percent of the alloy had an average crystallite size of 95 Å, as determined by X-ray diffraction, the remainder having an average crystallite size below 35 Å, the limit of detectability for the instrument used. 
     EXAMPLE 7 
     The procedure of Example 1 was repeated with the following exceptions. Instead of the solution containing the soluble complex of chloroplatinate and the sodium salt of EDTA, a solution containing a soluble complex of silver ammonia chloride (Ag(NH 3 ) 2  Cl) was formed by dissolving 3.93 grams of silver nitrate in 100 grams of water, adding potassium chloride to precipitate silver chloride, and then adding sufficient ammonium hydroxide to completely solubilize the silver chloride precipitate. Spray drying yielded 141 grams of finely divided co-crystallite of silver chloride and potassium terephthalate. The resulting dried pyrolysis product weighed 5.33 grams, had a BET surface area of 2316 square meters per gram, and contained 4.32 percent of silver by weight, based on the weight of the pyrolysis product. The silver was in the form of predominantly elemental silver. The dispersed silver had an average crystallite size of 145 Å, the remainder having an average crystallite size below 35 Å. 
     EXAMPLE 8 
     The procedure of Example 1 was employed with the following exceptions. 24.75 grams of terephthalic acid were added to a solution of 18.89 grams of potassium hydroxide in 200 grams of distilled water, slowly and with heating and stirring to form potassium terephthalate, and then 41.17 grams of potassium carbonate were dissolved in the solution. 6.16 grams of potassium dichromate were dissolved in 100 grams of water, and this solution was added to the solution of potassium terephthalate to form the solution for spray drying. 50 grams of the resulting co-crystallite powder from the spray drying step was then dry blended with 31.7 grams of 90 percent potassium hydroxide powder in the Waring blender. The resulting dry pyrolysis product weighed 5.7 grams, had a BET surface area of 1680 square meters per gram, and contained 30 percent of chromia (Cr 2  O 3 ) by weight, based on the weight of the pyrolysis product. Two percent of the chromia had an average crystallite size of 80 Å, with the remainder having an average crystallite size below 35 Å. 
     EXAMPLE 9 
     32 grams of the product of Example 1 were blended with 309 grams of an acid stabilized aqueous alumina hydrosol containing 32 grams of alumina. The mixture was gelled (solidified) by the addition of a solution containing 7.7 milliliters of water and 7.7 milliliters of a 50 percent aqueous solution of ammonium hydroxide. The resulting mixture was then dried overnight in a forced air oven at 165° C. The dried solid was calcined at 483° C. for 48 hours. The resulting granulated product contained 1.84 weight percent of platinum, 48.16 weight percent of active carbon and 50 weight percent of alumina. 
     EXAMPLE 10 
     The procedure of Example 9 was repeated using instead a blend of 7 grams of the product of Example 6 and 67.9 grams of the aqueous alumina hydrosol. The resulting granulated product contained 1.75 weight percent of platinum, 1.75 weight percent of rhodium, 46.5 weight percent of active carbon and 50 weight percent of alumina. 
     EXAMPLE 11 
     The procedure of Example 9 was repeated using instead a blend of 24 grams of the product of Example 1 and 233 grams of the aqueous alumina hydrosol. The resulting granulated product contained 1.83 weight percent of platinum, 47.25 weight percent of active carbon and 50.00 weight percent of alumina. 
     EXAMPLE 12 
     The procedure of Example 9 was repeated using instead a blend of 24 grams of the product of Example 8 and 233 grams of the alumina hydrosol. The resulting granulated product contained 15 weight percent of chromia, 35 weight percent of active carbon and 50 weight percent of alumina. 
     EXAMPLE 13 
     The procedure of Example 9 was repeated using instead a blend of 9.12 grams of the product of Example 4 and 88.54 grams of the alumina hydrosol. The resulting granulated product contained 0.60 weight percent of nickel, 49.4 weight percent of active carbon and 50 weight percent of alumina. 
     EXAMPLE 14 
     One part by weight of the product of Example 1 was mixed with 3 parts by weight of 90 percent potassium hydroxide to form a uniform powdered mixture, and the pyrolysis, water separation, wash and drying steps of Example 1 were repeated using this uniform powdered mixture as the starting material, to form a second pyrolysis product. This second pyrolysis causes an effective increase in the concentration of platinum in the active carbon matrix to 10 weight percent, by removal of some of the carbon matrix by oxidation of the pyrolysis product of Example 1. 
     The procedure of Example 9 was repeated using instead a blend of 20 grams of this second pyrolysis product and 194 grams of the aqueous alumina hydrosol. The resulting granulated product contained 5 weight percent of platinum, 45 weight percent of active carbon and 50 weight percent of alumina. 
     EXAMPLES 15-25 
     The utility of the composition of the present invention as hydrocarbon conversion catalysts is illustrated in Examples 15-25. In particular, Examples 15-20 illustrate the use of compositions of this invention as catalysts for the hydrogenation of hydrocarbons, and Examples 21-25 illustrate the use of compositions of this invention as catalysts for the dehydrogenation of hydrocarbons. More specifically, Example 21 illustrates the dehydrocyclization of n-heptane to toluene. 
     In each of Examples 15-25, a tubular reactor having a cross sectional area of 1.27 square centimeters and containing a bed of one of the catalytic compositions formed in Examples 9-14 was employed. The catalyst and bed height employed in each of Examples 15-25 are indicated in Tables 2 and 3. A gaseous hydrocarbon feed was passed downward through the catalyst bed with hydrogen in Examples 15-21, and with argon in Examples 22-25. The hydrocarbon feed was propylene in Examples 15-19, benzene in Example 20, n-heptane in Example 21, and propane in Examples 22-25. The hydrocarbon feed rate was 1.31 standard liters per hour in Examples 15-19, 1.6 milliliters per hour in Example 20, 13 milliliters per hour in Example 21, 1.31 standard liters per hour in Examples 22-23 and 1.59 standard liters per hour in Examples 24-25. The hydrogen feed rates ranged between 3.6 and 3.76  standard liters per hour in Examples 15-19 and were 10 standard liters per hour in Examples 20 and 21. The argon feed rates in Examples 22-25 ranged between 2.5 and 265 standard liters per hour. The catalyst bed temperatures in Examples 15-25 are indicated in Tables 2 and 3. The pressures in the reactor were 3.51 kilograms per square centimeter in Examples 15-19, 4.92 kilograms per square centimeter in Example 20, 21.09 kilograms per square centimeter in Example 21, and 1.05 kilograms per square centimeter in Examples 22-25. The degree of conversion of the hydrocarbon feeds for Examples 15-25 are given in Tables 2 and 3. For Examples 15-19, the conversion is expressed as the percent of propylene converted to propane. For Example 20, the conversion is expressed as the percent of benzene converted to cyclohexane. For Example 21, the conversion is expressed as the percent of n-heptane converted to toluene. For Examples 22-25, the conversion is expressed as the percent of propane converted to propylene. 
     
                       TABLE 2                                                     
______________________________________                                    
                             Catalyst                                     
                             Bed                                          
        Catalyst  Catalyst   Tempera-                                     
                                     Percent                              
        from      Bed        ture    Conver-                              
Example Example   Height (Cm.)                                            
                             (°C.)                                 
                                     sion                                 
______________________________________                                    
15       9        25         75      100                                  
16      10        13         65      100                                  
17      11        13         63      100                                  
18      12        13         69      100                                  
19      13        17         65       19                                  
                             82       45                                  
                             85       74                                  
                             94       83                                  
20      14        13         32      100                                  
                             35      100                                  
______________________________________                                    
 
    
     
                       TABLE 3                                                     
______________________________________                                    
                             Catalyst                                     
                             Bed                                          
        Catalyst Catalyst    Tempera-                                     
                                    Percent                               
        from     Bed         ture   Conver-                               
Example Example  Height (Cm.)                                             
                             (°C.)                                 
                                    sion                                  
______________________________________                                    
21       9       12          456    93.6                                  
                             482    98.3                                  
                             499    98.8                                  
                             515    100                                   
                             499    99.4                                  
                             499    99.2                                  
22       9       25          427    5.8                                   
                             456    5.7                                   
                             482    11.2                                  
                             510    13.8                                  
23      10       13          427    3.5                                   
                             456    3.5                                   
                             482    5.1                                   
24      12       17          427    0                                     
                             456    0.8                                   
                             482    3.0                                   
                             510    5.4                                   
                             538    9.5                                   
                             565    13.2                                  
25      13       17          427    1.1                                   
                             456    2.8                                   
                             482    4.7                                   
                             510    6.9                                   
                             538    12.2                                  
______________________________________                                    
 
    
     Analysis of the products from Examples 22-25 revealed no evidence that the cracking of propane occurred. Thus, the results of Examples 15-25 demonstrate the high activity and selectivity of the compositions of this invention as catalysts for hydrogen transfer reactions involving hydrocarbons. 
     From the above description, it is apparent that the objects of the present invention have been achieved. While only certain embodiments have been set forth, alternative embodiments and various modifications will be apparent from the above description to those skilled in the art. These and other alternatives are considered equivalents and within the spirit and scope of the present invention.