PROCESS FOR REMOVAL OF SULFUR FROM MOISTURE-BEARING, SULFUR-CONTAINING HYDROCARBON PROCESS STREAMS

Abstract: A process wherein a particulate sorbent mass of zeolite which has been ion-exchanged with zinc or cad­ mium to provide pore size openings of about 5A [5 × 10⁻¹⁰m], and grater, particularly zinc, is contacted with a moist hydrocarbon process stream which contains sulfur, sulfur compounds, and other contaminants, these being adsorbed onto said particulate sorbent mass, and the process stream thereby denuded of said sulfur, sul­ fur compounds, and other contaminants. Thereafter, the sulfur, sulfur compounds, and other contaminants, are readily desorbed, or removed from said particulate sor­ bent mass by contacting, and purging same with a gas stream, suitably hydrogen, or a hydrogen-containing gas, at elevated temperature.

Description: PROCESS FOR REMOVAL OF SULFUR FROM MOISTURE-BEARING SULFUR-CONTAINING HYDROCARBON STREAMS The present invention relates to a process for the removal of sulfur from moisture-bearing, sulfur-containing hydrocarbon process streams. Sulfur occurs in many industrial processes, and sulfur, or sulfur containing compounds, for varying reasons must often be removed from process streams, e.g., flue gas, waste gas or recycle gas streams. This has been accomplished, e.g., by contacting the sulfur-containing process stream with a sorbent comprising a particulate oxide, hydrated oxide, or hydroxide of alumina, zinc, iron, nickel, cobalt or the like, alone or in admixture with each other or with additional materials, e.g. , alkali or alkaline earth metal oxides or the like. Reference is made, e.g., to U.S. 3,492,083 and British Patent 871,076 (1957) which describes processes of this type. Hot spherical pebbles have also been used to remove sulfur from process streams, as described, e.g., in U.S. 2,551,905. The quality of these sorbents for the removal of sulfur varies considerably, and in many applications it is necessary to scrub essentially all of the sulfur from the process streams. This is done for process reasons, as well as environmental reasons. Sulfur, for example, is a well known catalyst poison which finds its way into a process principally via the feed, and it can gradually accumulate upon and poison a catalyst. Essentially all petroleum feeds contain sulfur. Most of the sulfur, because of this adverse effect, is generally removed from the feed, e.g., by contact with nickel or cobalt oxide guard chambers. Catalytic reforming, or hydroforming, a wellknown and important process employed in the petroleum refining industry for improving the octane quality of naphthas and straight run gasolines, is illustrative of a process where the presence of sulfur can have a detrimental effect. Sulfur unavoidably enters the process, principally as a part of the feed. In a typical reforming process, a series of reactors are provided with fixed beds of sulfided platinum-containing catalysts which are sequentially contacted with a naphtha feed, and hydrogen, and each reactor is provided with a preheater, or interstage heater, because the reactions which take place are endothermic. C5+ hydrocarbons as a product is taken from the last reactor of the series, and a hydrogen-sulfide contaminated hydrogen gas stream is separated therefrom and recycled to the several reactors of the series. In use of the more recently developed multimetallic platinum catalysts wherein an additional metal, or metals hydrogenation-dehydrogenation component is added as a promoter to the platinum, it has become essential to reduce the feed sulfur to only a few parts, per million parts by weight of feed (ppm), because of the sulfur sensitiveness of these catalysts. For example, in the use of platinum-rhenium catalysts it is generally necessary to reduce the sulfur concentration of the feed well below about 10 ppm, and preferably well below about 2 ppm, to avoid excessive loss of catalyst activity and C5 + liquid yield. The sulfur must also be scrubbed from the hydrogen recycle gas stream because this too is a source of catalyst sulfur contamination. The vapor effluent from the last reactor of the series is thus a gas rich in hydrogen, which generally contain hydrogen chloride and chlorine, as well as hydrogen sulfide, moisture and small amounts of normally gaseous and C5-C9 hydrocarbons. It is essential to separate hydrogen from the C5 + liquid product and recycle it to the process; and it is essential to remove the sulfur from the moist recycle hydrogen gas stream. This, as suggested, has been accomplished by the use of guard chambers filled with metal oxides, e.g., zinc oxide, supra. Zinc oxide thus has been used as a sorbent for selectively removing hydrogen sulfide from process streams. Usually, the zinc oxide is contacted with the gas at elevated temperatures to scrub out the sulfur. Such sorbent, however, has not proven successful because the adsorption rate is too low, and it has not been possible to regenerate such sorbent in a reducing atmosphere such as hydrogen due to the high thermodynamic stability of zinc sulfide. Regeneration of this material requires oxida tiok of the sulfur or sulfur-containing compounds, so chat the sulfur is evolved as uslfur oxides, an environmentally unacceptable product. Such regeneration impairs the mechanical strength of the material. Moreover, sulfur oxides are difficult to remove from flue gas effluents, .g., as containing with hydrogen sulfide which is easily cribbed from the stream with a caustic or amine solution. Wolf and co-workers studied the adsorption of 1 .011 sulfide and methyl mercaptan on exchanged syn hect sodium -- A zeolites as a function of the degree .- tion exchange. F. Wolf, W. Hoese & H. Fuertig Martin-Luther Univ. Halle-Wittenberg; Chemiekombinat Hiterfeld VEB) Chem. Tech. (Leipz.) 27 &num;6:362-64 (June Cj), For hydrogen sulfide, the capacities were found to descrease in the order barium < potassium < strontium < cobalt < nickel < zinc < manganese < sodium < magnesium < calcium. For methyl mercaptan the capacities were found comparable. The capacities of sodium X and sodium-potassium sieves for both sulfur compounds were slightly higher than those of the corresponding A sieves. In earlier work some members of tne same group has found chat zinc-A was relatively poor in adsorbing mercaptans. F. Wolf & K. H. ergk (Univ. Hauc, Erdoel Kohle, Erdgas, Petrochem Brennst. -Chem. 27 &num;10:629 (Oct. 1974); and this work was later confirmed by Soviet researchers E. I. Shcherbina, V. A. Yakubovich & L. I. Mikhalrkaya (Beloruss. Technol. Inst., Minsk) Neflekhimya 17 &num;1:151-55 (Jan. - Feb. 1977). German Patent 2,226,531 which issued June 1973 to Gebr Herrmann discloses that Pb zeolites can be used for hydrogen sulfide sorption, and that the lead can be exchanged by other metals, inclusive of zinc. The Patentee, however, states that such exchanged zeolites have not been found of practical use. Robert M. Milton's U.S. Patents 3,078,640 and 3,024,868, which issued on applications filed in the last weeks of the year 1959, are believed to exemplify the state-of-the-art as relates to the separation of sulfurcontaining compounds from gaseous mixtures by the use of molecular sieve adsorbents. In U.S. 3,078,640, which issued February 25, 1963, certain forms of zeolite A are suggested for use in the selective adsorption of hydrogen sulfide from a vapor mixture containing at least one member of the group consisting of hydrogen, carbon dioxide and normal saturated aliphatic hydrocarbons containing less than nine carbon atoms per molecule. The reference suggests that zeolite A can be used in its sodium form, or the sodium ions of the zeolite can be substituted at least in part by other metal ions from Group I and Group II of the Periodic Table. The reference states that the various ion exchanged forms of zeolite A includes the lithium, ammonium, silver, zinc, nickel hydrogen and strontium forms. It is stressed that the divalent metal substituted forms of zeolite A, e.g., zinc, nickel and strontium zeolite A, behave quite differently from the monovalent metal substituted forms of zeolite A, e.g., lithium, and hydrogen zeolite A. It suggests that any cationic form of zeolite A having a pore size of at least 4 Angstroms is suitable for practicing the invention; and conversely that smaller pore size forms are unsatisfactory because they do not admit hydrogen sulfide and mercaptans. Albeit, however, this reference describes the use of molecular sieves having pore sizes greater than 4 as a selective adsorbent for the separation of sulfur-containing compounds from hydr carbons, there is no suggestion of the separation, or adsorption, of sulfur containing compounds from moisture bearing, or water containing streams. The separation of sulfur compounds from moist, or wet streams presents a far more difficult problem inasmuch as water is preferentially adsorbed to the exclusion of sulfur containing compounds, and e.g., water generally replaces essentially all of the hydrogen sulfide from an adsorbent contacted with a stream containing both water and hydrogen sulfide. On the other hand, in U.S. 3,024,868, which EMI4.1 issued March 13, 1962, there is specifically described a process useful for the separation of sulfur containing compounds from moist vaporous streams. In particular, trLe process described is one useful for removing moistui:- sulfur containing compounds, notably hydrogen sulfide, from the recycle hydrogen gas stream of a reformer by contact of the stream with crystalline zeolitic molecular sieves having pore sizes ranging from about 3.6 to 4A. Both the water and sulfur containing compounds are sorbed preferentially, to the exclusion of the saturated paraffinic hydrocarbons. It is expressly stated thet molecular sieves having larger pore sizes, viz. > 4 , strongly preferentially adsorb and concentrate the C4 and higher paraffins. Any substitution of the sodium zeolite A with monovalent or divalent metal ions which enlarges the pore size beyond this limit is thus, according to Milton, to be avoided. This adverse effect, according to Milton, is particularly apparent with divalent cation forms of zeolite, the enlargement being manifested above about 25 percent substitution of divalent ions in the molecular sieve structure. Data presented in the patent show tt zno'içe AA has eight to ten tomes the adsorptive capacity for water and hydrogen sulfide as zeolite 5A and zeolite 13X, with concurrent high exclusion or rejection of the hydrocarbons. In Milton's process a reformer recycle hydrogen gas stream is desulfided by contact with at least two separate beds of the zeolite 4A, the wet reformer hydrogen gas stream being contacted with a first bed in an adsorption stroke at relatively low temperature and pressure, while water and sulfur containing compounds are desorhod from a second bed in a desorption stroke at relatively high temperature and pressure. The flows between the beds are periodically reversed such that the first bed is on an adsorption stroke while the second bed is on a desorption stroke, and vice-versa. Whereas commercial processes based on the use of metal oxides for adsorption of sulfur from process streams have provided varying degrees of success, there is little evidence that the zeolites have attracted any significant commercial interest, if any, for this use A considerable need therefore exists for the development of new and improved processes of this type, especially those which are capable of adsorbing, and separating sulfur'containing compounds from moist hydrocarbon streams; notably hydrogenEsulfide-containing reforming hydrogen recycle gas. It is an object of this present invention to provide a new and improved process, particularly one utilizing a sorbent which is capable of high rates of sulfur adsorption from process streams, and more particularly one which can be regenerated without significant loss of mechanical strength, if any. This object is achieved in accordance with the present invention, embodying a process wherein a particulate sorbent mass of zeolite which has been ion-exchanged with Zinc or cadmium, particularly zinc, sufficient to provide pore size openinings greater than 4 , preferably 5 and greater, most preferably from about SA to about 13A, is contacted with a moisture bearing, hydrocarbon process stream which contains sulfur, sulfur compounds, and other contaminants, these are adsorbed onto said particulate mass of ion-exchaiiged zeolite, and the process stream thereby denuded of said sulfur, sulfur compounds, and other contaminants. Thereafter, the sulfur, sulfur compounds, and other contaminants, are readily desorbed, or removed from said particulate mass of ion-exchanged zeolite by contacting, and purging same with a gas stream, suitably hydrogen, hydrogen-containing gas, or inert gas such as nitrogen or methane at elevated temperature. Various zeolites ion-exchanged with zinc or cadmium metals are useful in accordance with this invention inclusive of intermediate and large pore zeolites. Preferred ion-exchanged zeolites include mordenite, faujasite, erionite, ferrierite, zeolite A, ZSM-5, zeolite X and Y, chabazite, both natural and synthetic having pore size openings greater than 4A, preferably 5A and greater; especially those having pore size opening ranging from about 5 to about 13 . The A type zeolite is preferred, especially one which is ion-exchanged with a zinc salt, sufficient to provide pore size openings of O about 5A, and greater. exchange of at least about 25 percent, and certainly 65 percent of the sodium ions of an type zeolite with zinc, or cadmium, is found to price zeolite 5A. In fact, it is found that the adsorption behavior of most of the zeolites, especially zeolite r, begins to change when greater than about 25 percent of the sodium ions are exchanged with the multivalent cation, zinc or cadmium, the pore size openings increasing their normal sizes, especially zeolite A which increases beyond 4 . Such divalent forms of zeolite A are found far more effective for the selective adsorption of sulfur containing compounds than the small pore species of zeolite A pre iously known for such use, supra. In a preferred operation, a particulate mass of ion-exchanged zeolite, notably zinc exchanged zeolite is iirarged, or packed lito C guard chamber, or series o, quare chambers. Most preferably, the series of zinc exchar--ed polite guard chambers are employed in parallel, this permitting active use of one guard chamber, or set of sue. all aligned guard chambers for contact, and purification s a process stream while th other guard chamber, or set of serially aligned guard chambers, is cut out of series for regeneration. In the treatment of a hydrogen recycle gas stream, as employed in reforming, it is found that the hydrogen sulfide can be readily adsorbed from the stream despite the high moisture content of the gas. This is mildly surprising because it is well known that the selectivity of many sorbents for hydrogen sulfide is adversely affected in the presence of water. As a class, the zeolites, in particular, show a preferential adsorption of water, this resulting in a low capacity of the zeolites for the selective removal of hydrogen sulfide. The zinc, and cadmiumexchange zeolite, notably the zinc exchanged zeolite, shows a high capacity for adsorption of the hydrogen sulfide, several times that of many sulfur sorbent materials. No special preparation of the particulate ion-exchanged zeolite of this invention is required, and it can be employed in a guard chamber as powder, spheres, tablets, pellets extrudes, irregular shaped particles, or the like in virtually any size. The temperature of contact is not critical, and there is no necessity to heat or cool the process stream, notably the recycle gas stream. Suitably, the recycle hydrogen stream is contacted with the particulate zinc exchanged zeolite sorbent at normal gas stream temperatures, i.e., at temperatures ranging from about ambient to EMI8.1 abouti(5000F)1 or more generally at temperatures ranqinq EMI8.2 from about[(100 F) to about [(300 F). It would appear, surprisingly, that the metal atoms of the zeolite structure, notably the zinc atoms of the zinc exchanged zeolite, forms simple adsorption bonds with the sulfur compound, this being sufficient to remove, e.g., hydrogen sulfide from a recycle hydrogen gas stream. Unlike the mechanism involved in the removal of a sulfur compound, e.g., hydrogen sulfide, from a recycle hydrogen gas stream by the use of zinc oxide, there is no chemical reaction wherein zinc sulfide is formed. Apparently, as a consequence thereof the zinc exchanged zeolite is readily regenerated by simply purging, or sweeping the sulfur compound therefrom with a hot, non-reactive, or inert gas after it has become sufficiently saturated with the sulfur compound. In the preferred practice of this invention, the zinc exchanged zeolite is simply contacted, purged, or swept with a hydrogen gas stream at elevated temperature to remove the hydrogen sulfide, and other sulfur compounds, and thereby regenerate the zinc exchanged zeolite. Suitably, the purse is conducted by maintainina the hydrogen qas at EMI8.3 temperatures ranging from about2(300 Fp to ab6utWl2000F), EMI9.1 preferably frOm about [(500 F) to about [(1000 F). Since burning in the presence of oxygen as practiced in the regeneration of many sorbents is unnecessary, the hydrogen sulfide is recovered as hydrogen sulfide rather than as sulfur oxides. Consequently, the hydrogen gas stream itself is readily cleansed of the hydrogen sulfide by washing the gas with a caustic or amine solution. The invention will be more fully understood by reference to the following examples, and comparative data which demonstrate the high selectivities for hydrogen sulfide of the zeolites of this invention in the presence of water. All terms are given in weight units except as otherwise specified. EXAMPLES A series of different commercially known zeolites, as identified hereafter, were exchanged with an aqueous solution of zinc chloride, ZnCl2. This was followed by filtration and washing until the filtrate was free of chloride as determined by testing with an AgNO3 solution. The zeolites were then vacuum dried, and calcined in air EMI9.2 for three hours a±8O00F9. To measure H2S adsorption, the zeolite was packed into a quartz reactor maintained at 93.3 C (200 0F) and a stream of 2000 ppm. H25 in H2 at atmospheric pressure passed through until breakthrough occurred. This was observed by the discoloration of lead acetate paper. For reqeneration, the adsorbents were heated either to EMI9.3 EMI9.4 500 F or tokY9320Fjwhile stripping with H2 gas. The adsorpof HS was then redetermined at a standardized temperature EMI9.5 og[(200 F). Data on several Zn exchanged zeolites are shown in the Table and/or compared with the unexchanged or corresponding natural zeolite. Table Exchanged Zeolites EMI10.1 Wt % S Adsorbed &commat;[(200 F), 1 Atm. From A 2000 ppm H2S in H2 Stream Cycle 2 Cycle 3 Wt. % z Na Adsorbent Zn Exchanged EMI10.2 <tb> <SEP> After <SEP> After <tb> <SEP> 2 <SEP> H2 <SEP> 2GOCC <SEP> H2 <tb> Cycle <SEP> 1 <SEP> iStrip <SEP> Strip <tb> Original&commat;9320F <SEP> &commat;(500OF) <tb> Na Zeolite A (4A Sieve) 0 0 0.22 Z Zeolite A (Zn 5A) 14.5 65 2.57 3.02 2.0 Cd Zeolite A - 50 2.38 1.27 Ni Zeolite Aa - 16 0.76 0.58 Co Zeolite A - 42 0.85 1.40 Cu Zeolite Aa,b - 77 0.47 0.0404 - Hg Zeolite Aa,b - 100 0.40 Zn Exchanged Erionite 5.79 1.12 Natural Chabazite 0 0 0.96 Zn Chabazite 6.33 - 1.51 1.87 Na Mordenite 0 0 1.08 Zn Mordenite 3.67 - 1.25 aPartial destruction of the zeolite A crystal structure occurred during the ion-exchange. bAssuming +2 valence state for Cu and Hg. From these data, it will be initially observed that the original sodium zeolite A (4A sieve) had very limited capacity f(- H2S under these conditions. The Zn 5A form, however, had a capacity nearly ten times as great. Furthermore, a simple hydrogen strip was effective for regeneration of the sorbent. The increase in capacity in going from 2.37 wt. % in Cycle 1 to 3.02 wt. % in Cycle 2 EMI10.3 is attributable to the higher7(932 F)regeneration tempera EMI10.4 ture compared to the) (800 F) original air calcination. The EMI10.5 regeneration at)(500 F) is effective in restoring capacity in Cycle 3 to nearly that observed in Cycle 1. The sodium form of zeolite A has the formula Na12[(AlO2)12(SiO2)12]#XH2O, this material being designated 4A becauese 4 approximates the effective pore size openings of this material in Angstroms. Zeolite 4A will not adsorb propane. When zeolite A is ion-exchanged with potassium so that its chemical composition becomes K12[(AlO2)12(SiO2)12]XH2O, its effective diameter becomes 3t and hence is known as 3A. It adsorbes H2O, NH3, and methanol but not ethane. If zeolite A is exchanged with sufficient of a multivalent cation, e.g., Ca, the effective pore diameter can become 5 , and such material is designated as 5A. This material will adsorb n-paraffins such as n-heptane. It is well known, e.g., by reference to the literature that at least 25% of the Na ions have to be exchanged with calcium to enable its pore diameter to increase in size (See, e.g., U.S. 3,024,968, col. 3, lines 36-44). Profound changes in adsorption behavior also occur when greater than 25% of the sodium ions are exchanged with a multivalent cation, e.g., Ca. In accordance with the present invention the various forms of zeolite are ion-exchanged with zinc or cadmium, preferably zinc; and where the pore openings of the zeolite are of lesser effective diameter than 5A the zeolite is nonetheless suitable if the diameters of the pore size opening can be increased by exchange to provide pore openingsof about 5 , and greater. Of course, zeolite with pore size diameters initially greater then 5 effective pore diameter need only be ion-exchanged with zinc or cadmium, preferably zinc, to render them suitable for use in accordance with the present invention. With continued reference to the Table, it will be observed that zinc exchange with chabazite improves its capacity, and the material can also be regenerated by hydrogen. Although the capacity is generally less than that of Zn4A, chabazite is structurally more stable in acid environments. The other acid resistant zeolites, mordenite and erionite, also show improved capacity for H2S adsorption upon Zn exchange. A feature of this invention lies in the improved selectivity of the ion-exchanged zeolites of this invention for H2S removal from reformer recycle gas. This permits the realization or higher activity, yields and stability for reforming catalysts, notably bimetallic catalysts. Unlike ZnO, the Zn zeolites also serve to remove water and to be easily regenerable with hydrogen stripping. It is apparent that various modifications and changes can be made without departing from the spirit and scope of the invention. For example, the ion-exchanged molecular sieves of this invention can be used in combination with metal alumina spinels, by charging each type of adsorbent to guar chambers and using the guard chambers in series. The ion-exchanged molecular sieves show good sulfur adsorption pro-erties, and superior water adsorption properties. The metal alumina spinels show superior sulfur adsorption properties.

Claims: CLAIMS: 1. A process for the removal of sulfur from a moisture-bearing, sulfur-containing hydrocarbon process stream characterize b-contacting said stream with a particulate mass of zeolite sufficiently ion-exchanged with zinc or cadmium to provide pore size openings of about SA (5 x 10 10m), and greater, to adsorb sulfur thereon, and thereafter contacting said ion-exchanged zeolite after completion of the sulfur sorption cycle with an essentially non-reactive gas or reducing gas at elevated temperature thereby desorbing the sulfur and regenerating the sorbent. 2. The process of Claim 1 characterized in that the ion-exchanged zeolite is sodium zeolite A ion-exchanged with zinc sufficient to replace at least about 25 percent of the sodium of the original zeolite A. 3. The e process of Claim 1 or Claim 2 characterized in that the ion-exchanged zeolite is zinc-exchanged zeolite A or zinc exchanged chabasit e. The process of any one of Claims 1 to 3 characterized in that the gas employed to desorb the sulfur from the ion-exchanged zeolite is comprised of hydrogen. 5. The process of Claim 4 characterized in that the hydrogen is contacted with said zinc-exchanged zeolite sorbent at temperatures ranging from about 204.4-C (400 F) to about 648.9'C (1200-F), preferabl at temperatures ranging from about 426.7-C (800'F) to about 537.8C (100 F). 6. A process of any one of Claims 1 to 5 characterized in that the process is carried out in a series of on-stream reactors and the non-reactive gas or reducing gas is a vaporous effluent rich in hydrogen recycled from the last reactor in the process series.

Inventors: EBERLY, PAUL EARL, JR.
Applicants: EXXON RESEARCH AND ENGINEERING COMPANY
Application year: 1981
Main classification: C10G25
IPC codes: C10G49, C10K1, B01D53, C10G25, C07C7