US20100230296A1 - Production of Hydrogen Gas From Sulfur-Containing Compounds - Google Patents
Production of Hydrogen Gas From Sulfur-Containing Compounds Download PDFInfo
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- US20100230296A1 US20100230296A1 US12/599,857 US59985708A US2010230296A1 US 20100230296 A1 US20100230296 A1 US 20100230296A1 US 59985708 A US59985708 A US 59985708A US 2010230296 A1 US2010230296 A1 US 2010230296A1
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- C—CHEMISTRY; METALLURGY
- C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
- C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
- C25B1/00—Electrolytic production of inorganic compounds or non-metals
- C25B1/01—Products
- C25B1/02—Hydrogen or oxygen
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- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
- C01B17/00—Sulfur; Compounds thereof
- C01B17/48—Sulfur dioxide; Sulfurous acid
- C01B17/50—Preparation of sulfur dioxide
- C01B17/508—Preparation of sulfur dioxide by oxidation of sulfur compounds
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- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
- C01B17/00—Sulfur; Compounds thereof
- C01B17/48—Sulfur dioxide; Sulfurous acid
- C01B17/50—Preparation of sulfur dioxide
- C01B17/54—Preparation of sulfur dioxide by burning elemental sulfur
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- C—CHEMISTRY; METALLURGY
- C01—INORGANIC CHEMISTRY
- C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
- C01B17/00—Sulfur; Compounds thereof
- C01B17/69—Sulfur trioxide; Sulfuric acid
- C01B17/74—Preparation
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- C—CHEMISTRY; METALLURGY
- C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
- C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
- C25B1/00—Electrolytic production of inorganic compounds or non-metals
- C25B1/01—Products
- C25B1/22—Inorganic acids
Definitions
- This invention relates to the preparation of hydrogen gas using electrolytic processing of sulfurous acid.
- Hydrogen (H 2 ) is a valuable feedstock in refineries for an assortment of hydrogenation processes. Hydrogen is also seeing greater value as a fuel source, both in direct combustion and in fuel cells. Public discussions addressing the reduction of carbon dioxide (CO 2 ) emissions often refer to an alternative of a “hydrogen economy.” Thus, methods for the economic generation and recovery of hydrogen while avoiding or reducing the co-production of CO 2 are currently of interest.
- H 2 S hydrogen sulfide
- Many of the processes for generating hydrogen from H 2 S suffer from problems associated with the co-generation of elemental sulfur. While elemental sulfur is a relatively benign solid at ambient conditions, it can be a problem in terms of disposal. Most sulfur is used in the formation of sulfuric acid, an important industrial product. However, local markets may be saturated with sulfur, and long term storage of solid, block sulfur is undesirable. An improved process would generate a co-product that is more easily disposed of than elemental sulfur.
- U.S. Pat. No. 5,843,395 teaches the thermal disassociation of H 2 S containing waste gas at about 1,000° C. to about 1,900° C. to provide hydrogen and sulfur, the hydrogen taken off by membrane separation. Any waste heat is used to pre-heat the waste gas prior to the dissociation step.
- U.S. Pat. No. 4,836,992 teaches the use of an electrolytic cell to make H 2 from H 2 SO 3 , made from mixing SO 2 with NaOH, NaSO 3 or H 2 SO 4 , thus yielding by-products of H 2 SO 4 and NaOH upon the electrolytic conversion. The SO 2 is provided from the burning of waste gases.
- 4,519,881 teaches the use of a three-chamber electrolytic cell to regenerate sodium hydroxide from caustic solutions containing sulfides.
- the process produces hydrogen sulfide by the electrolysis of sodium sulfide and hydrogen ions and also produces hydrogen.
- the process is not compatible with a natural gas stream and does not generate hydrogen gas directly from the sulfurous acid solution.
- the described and claimed invention is a process for producing hydrogen gas comprising (a) combusting sulfur (S) or hydrogen sulfide (H 2 S) with oxygen (O 2 ) to obtain sulfur dioxide (SO 2 ) and water (H 2 O), plus heat; (b) adding water to the product of (a) to obtain a sulfurous acid solution (H 2 SO 3 and H 2 O); (c) applying electrical current to the sulfurous acid solution of (b) to obtain sulfuric acid (H 2 SO 4 ) and hydrogen gas (H 2 ); and, (d) separating the sulfuric acid from the hydrogen gas to obtain separated components of the sulfuric acid and the hydrogen gas, wherein the heat generated in (a) is used to generate at least a portion of the electricity for the electrical current for (c).
- the oxygen in (a) is provided at least in part by the introduction of air, e.g., by providing an air stream into the combustion reaction.
- Oxygen for combustion can be generated from a cryogenic air separation unit (ASU), or from a membrane process, or from a pressure-swing adsorption unit, all of which reduce the nitrogen content of the gas to be processed.
- the SO 2 can be captured in a relatively pure form by using a liquid solvent, such as a diamine, applied to various flue sources containing the SO 2 , for example from combusting acid gas, disulfide oil, or coal, which will all contain CO 2 .
- the sulfur or hydrogen sulfide is provided in (a) by the introduction of combustible compositions, gaseous, liquid or solid, which compositions contain sulfur and/or hydrogen sulfide.
- combustible compositions gaseous, liquid or solid, which compositions contain sulfur and/or hydrogen sulfide.
- examples include “sour natural gas”, acid gas from petroleum and natural gas recovery, sulfur-laden heavy oil and bitumen, and one or more of hard or soft coal and coke products.
- a system for producing hydrogen gas includes: a) an acid gas stream containing hydrogen sulfide; b) an air stream; c) a burner configured to burn the acid gas stream and air stream and produce a product stream having at least sulfur dioxide, water, and heat; d) a boiler unit operatively connected to the product stream of the burner and configured to capture heat from the burner, and generate at least a steam stream and an exhaust gas stream having at least SO 2 ; e) an SO 2 separation unit operatively connected to the exhaust gas stream of the boiler unit and configured to remove SO 2 from the exhaust gas stream and generate an SO 2 exit stream; and f) an electrolytic cell operatively connected to the SO 2 exit stream and configured to produce hydrogen gas (H 2 ).
- FIG. 1 presents a block diagram of one embodiment of the invention process for converting hydrogen sulfide and/or elemental sulfur into hydrogen and sulfuric acid.
- the invention described and claimed below comprises a combination of hydrogen sulfide (H 2 S), or elemental sulfur (S), combustion, electricity generation from recycled heat, and electrolytic processing of sulfurous acid (H 2 SO 3 ) to generate hydrogen and sulfuric acid with little CO 2 (or SO 2 ) being emitted.
- H 2 S hydrogen sulfide
- S elemental sulfur
- combustion electricity generation from recycled heat
- SO 2 SO 3 sulfurous acid
- the required SO 2 can be generated from a number of one-pass processes.
- elemental sulfur can be captured from a Claus sulfur recovery process, wherein SO 2 is combined with H 2 S in a molar ratio of 1:2 to generate approximately 3 moles of elemental sulfur and 2 moles of water.
- tail gas treating unit where the remaining gases are captured for further treatment, i.e., combusted in accordance with the invention.
- the tail gas could be combusted to convert all sulfur-containing compounds to SO 2 , while capturing the SO 2 in a special solvent, as described in WO-A-2006/016979.
- Another example is the combustion of sulfur-containing coal, or bitumen that generates SO 2 .
- selective capture of SO 2 by a diamine or other solvent can generate a fairly pure SO 2 stream for processing.
- Disulfide oils, mercaptans, etc. which can be separated from liquid hydrocarbons using caustic processes, may also be considered as combustible feed for this process.
- the ready availability of sulfur and/or hydrogen sulfide, plus oxygen, enables an efficient process for producing both sulfuric acid and hydrogen.
- the hydrogen gas can be cycled for use in hydrogenation processes or transported and/or packaged for sale and used for developing fuel processes using hydrogen.
- the sulfuric acid by-product is a commodity product that can be recycled or sold for further use, e.g., chemical process use, or it can be readily disposed of in saline aquifers generally available where sulfur-containing natural gas is recovered. Since the sulfuric acid is a liquid, it is amenable to downhole disposal, whereas solid elemental sulfur must be kept in stockpiles on the surface, or buried at some effort and expense.
- relatively pure H 2 S is combusted in oxygen according to:
- the heat generated by these reactions can be used to produce steam, which then can be used to generate electricity for step (c) in the process.
- the SO 2 -containing stream is then quenched with water to generate a sulfurous acid solution:
- the sulfurous acid solution is then routed to an electrolytic cell.
- Some of the electricity generated via recovery of heat from reaction (5) powers the electrolytic cell, where hydrogen is liberated, and sulfuric acid is generated according to the following:
- Heat is recovered in the waste heat boiler at 600° F. (315.6° C.), well above the dewpoint of the SO 3 /H 2 SO 4 present. Ninety-five percent heat recovery and 30% efficient conversion to electricity are assumed. Adequate heat is recovered to regenerate the scrubbing solvent, plus generate enough electricity for the electrolysis. Surplus heat can be used for additional steam or electricity.
- acid gas 1 containing hydrogen sulfide at 250.0 kgmols/hr, carbon dioxide at 705.0 kgmols/hr, water in the form of moisture in an amount of 45.0 kgmol/hr, air 2 containing oxygen in amount of 426.8 kgmols/hr, nitrogen in an amount at 1740.2 kgmols/hr, and water in the form of moisture in an amount of 33.0 kgmols/hr is introduced into a burner, or combustion chamber 20 .
- stream 3 comprises the nitrogen and carbon dioxide in the same amounts as in the feed gas (unreacted), with sulfur dioxide at 245 kgmols/hr, with 5.0 kgmols/hr sulfur trioxide, 328.0 kgmols/hr water, and 49.3 kgmols/hr oxygen.
- This hot, gaseous stream 3 is passed to a boiler unit 21 (i.e., heat exchanger) where 863.3 kgmol/hr water, comprising at least in part condensed steam from the electrical generator 24 , is introduced via stream 13 to provide water for the boiler.
- a separate water stream (not shown) can be used to source the boiler.
- water is condensed from the combusted stream 3 to provide the water reagent for reaction (6).
- Steam containing 3116.2 kgmols/hr water vapor is withdrawn in stream 10 , and a gaseous, SO 2 -containing stream 4 , containing additionally the CO 2 , O 2 , N 2 , water vapor, and SO 3 of stream 3 exits the boiler unit 21 .
- Stream 4 will generally be maintained at temperatures above the SO 3 dewpoint, to avoid condensation of corrosive sulfuric acid, H 2 SO 4 .
- the operating temperature may be as high as 600° F.
- Stream 4 is then quenched by contact with liquid water in a device such as a DynaWave scrubber from MECS, Inc., to reduce the temperature to 100-150 F.
- Reactive SO 3 and H 2 SO 4 dissolve in the aqueous quench stream.
- a small amount of this stream is purged from the system as a weak solution of H 2 SO 4 in purge stream 15 .
- the balance of the stream is cooled, and recycled to the scrubbing device.
- the cooled, H 2 SO 4 -free gas stream is then provided for separation where SO 2 is preferentially removed by absorbing it into an SO 2 -selective solvent in a gas-liquid contacting device 22 a .
- the exit stream 6 cooled to 100-150° F., comprises 240.6 kgmols/hr SO 2 and flows from the regeneration unit 22 b at 17-25 psia to the electrolytic cell 23 at near-atmospheric pressure. A portion of the steam (1,992.2 kgmols/hr) from the boiler unit 21 in exit stream 10 is diverted in stream 12 to the regeneration unit 22 b to provide heat.
- stream 11 to the electricity generator comprises 862.3 kgmols/hr steam.
- Excess steam in an amount of 261.8 kgmols/hr water is removed from stream 12 via stream 16 prior to provision to the regeneration unit 22 b .
- a separate stream 15 takes off 5.0 kgmols/hr H 2 SO 4 , 3.4 kgmols/hr SO 2 (as H 2 SO 3 ), and 25.0 kgmols/hr water from the scrubbing unit 22 a .
- Unreacted and by-product gases are vented from the separation unit and removed in stream 5 , this stream thus comprising all of the CO 2 , residual O 2 , and N 2 , plus 1.0 kgmol/hr SO 2 , and 328.0 kgmols/hr water vapor.
- Separate stream 14 returns 1,992.2 kgmols/hr water from the regenerator unit 22 b as condensate to the boiler unit 21 .
- the spent steam from the electrical generator is condensed in the generator 24 or in a separate condensing unit 25 , and returned via stream 13 to the boiler unit 21 as the boiler feed water.
Abstract
The described invention is a process for producing hydrogen gas comprising (a) combusting sulfur (S) or hydrogen sulfide (H2S) with oxygen (O2) to obtain sulfur dioxide (SO2) and water (H2O), plus heat; (b) adding water to the product of (a) to obtain a sulfurous acid solution (H2SO3 and H2O); (c) applying electrical current to the sulfurous acid solution of (b) to obtain sulfuric acid (H2SO4) and hydrogen gas (H2); and, (d) using gas-liquid separation to separate the sulfuric acid from the hydrogen gas to obtain separated components of the sulfuric acid and the hydrogen gas; and, wherein the heat generated in (a) is used to generate at least a portion of the electricity for the electrical current of (c).
Description
- This application claims the benefit of U.S. Provisional Application No. 60/961,639, filed 23 Jul. 2007.
- This invention relates to the preparation of hydrogen gas using electrolytic processing of sulfurous acid.
- Hydrogen (H2) is a valuable feedstock in refineries for an assortment of hydrogenation processes. Hydrogen is also seeing greater value as a fuel source, both in direct combustion and in fuel cells. Public discussions addressing the reduction of carbon dioxide (CO2) emissions often refer to an alternative of a “hydrogen economy.” Thus, methods for the economic generation and recovery of hydrogen while avoiding or reducing the co-production of CO2 are currently of interest.
- In theory, the most “clean” method of producing hydrogen is the dissociation of water into the sought hydrogen with a by-product of oxygen (O2). However, the direct thermal dissociation of water is cost prohibitive in view of the high temperatures and energy required for this highly endothermic reaction. Direct electrolysis of water is similarly energy intensive. Thus, the major current route to large-scale hydrogen generation is through steam reforming of hydrocarbonaceous fuels. Here, the hydrocarbons are partially oxidized to carbon monoxide (CO) and hydrogen gas (H2), creating what is known as “syngas”. Steam reforming of methane yields the greatest amount of H2 per mole of methane:
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CH4+H2O---->CO+3H2 ΔH°298=210 kJ/mole (1) - Note that (1) is still strongly endothermic, and thus requires heat. The CO is used to generate more hydrogen through the water-shift reaction:
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H2O+CO---->CO2+H2 ΔH°298=−42 kJ/mole (2) - Theoretically, it is possible to generate 4 moles of H2 per mole of CO2 emitted. In practice, hydrocarbonaceous fuels are combusted to generate heat for reaction (1), so the actual H2:CO2 ratio is less than 4:1. It is desirable to increase the H2:CO2 ratio to reduce the relative amount of CO2 and other greenhouse gases emitted. It would be even better to eliminate the co-production of carbon containing gases, including CO2, all together.
- To this end, a number of different routes for abstracting hydrogen directly from hydrogen sulfide (H2S) have been proposed, since the theoretical dissociation energy for H2S is much lower than that for water. See, for example, “Hydrogen for H2S: Technologies and Economics,” Luinstra, E. A., Alberta Energy-Alberta Hydrogen Research Program, Calgary, May 26, 1995. Many of the processes for generating hydrogen from H2S suffer from problems associated with the co-generation of elemental sulfur. While elemental sulfur is a relatively benign solid at ambient conditions, it can be a problem in terms of disposal. Most sulfur is used in the formation of sulfuric acid, an important industrial product. However, local markets may be saturated with sulfur, and long term storage of solid, block sulfur is undesirable. An improved process would generate a co-product that is more easily disposed of than elemental sulfur.
- An early method of producing hydrogen by the electrolytic processing of sulfurous acid is described in U.S. Pat. No. 3,888,750. Here the source of the sulfurous acid is based on a high temperature process for the recycle of sulfuric acid where the by-product of the electrolytic conversion of the sulfurous acid is the sulfuric acid that is subsequently converted into sulfur dioxide and oxygen by thermal decomposition. The sulfur dioxide is separated from the oxygen by vapor-liquid separation. The oxygen is taken off for other uses or vented to the atmosphere and the sulfur dioxide is recycled to the electrolytic cell. The thermal decomposition step requires a high energy input.
- U.S. Pat. No. 5,843,395 teaches the thermal disassociation of H2S containing waste gas at about 1,000° C. to about 1,900° C. to provide hydrogen and sulfur, the hydrogen taken off by membrane separation. Any waste heat is used to pre-heat the waste gas prior to the dissociation step. U.S. Pat. No. 4,836,992 teaches the use of an electrolytic cell to make H2 from H2SO3, made from mixing SO2 with NaOH, NaSO3 or H2SO4, thus yielding by-products of H2SO4 and NaOH upon the electrolytic conversion. The SO2 is provided from the burning of waste gases. U.S. Pat. No. 4,519,881 teaches the use of a three-chamber electrolytic cell to regenerate sodium hydroxide from caustic solutions containing sulfides. The process produces hydrogen sulfide by the electrolysis of sodium sulfide and hydrogen ions and also produces hydrogen. However, the process is not compatible with a natural gas stream and does not generate hydrogen gas directly from the sulfurous acid solution.
- Accordingly, there is still a need for an effective process for the production of hydrogen from readily available sources while reducing or eliminating any co-production of carbon dioxide or other by-products that are difficult to dispose of in a environmentally effective manner.
- The described and claimed invention is a process for producing hydrogen gas comprising (a) combusting sulfur (S) or hydrogen sulfide (H2S) with oxygen (O2) to obtain sulfur dioxide (SO2) and water (H2O), plus heat; (b) adding water to the product of (a) to obtain a sulfurous acid solution (H2SO3 and H2O); (c) applying electrical current to the sulfurous acid solution of (b) to obtain sulfuric acid (H2SO4) and hydrogen gas (H2); and, (d) separating the sulfuric acid from the hydrogen gas to obtain separated components of the sulfuric acid and the hydrogen gas, wherein the heat generated in (a) is used to generate at least a portion of the electricity for the electrical current for (c).
- In another preferred embodiment, the oxygen in (a) is provided at least in part by the introduction of air, e.g., by providing an air stream into the combustion reaction. Oxygen for combustion can be generated from a cryogenic air separation unit (ASU), or from a membrane process, or from a pressure-swing adsorption unit, all of which reduce the nitrogen content of the gas to be processed. Alternatively, the SO2 can be captured in a relatively pure form by using a liquid solvent, such as a diamine, applied to various flue sources containing the SO2, for example from combusting acid gas, disulfide oil, or coal, which will all contain CO2. In a further preferred embodiment, the sulfur or hydrogen sulfide is provided in (a) by the introduction of combustible compositions, gaseous, liquid or solid, which compositions contain sulfur and/or hydrogen sulfide. Examples include “sour natural gas”, acid gas from petroleum and natural gas recovery, sulfur-laden heavy oil and bitumen, and one or more of hard or soft coal and coke products.
- In an alternative embodiment, a system for producing hydrogen gas is provided. The system includes: a) an acid gas stream containing hydrogen sulfide; b) an air stream; c) a burner configured to burn the acid gas stream and air stream and produce a product stream having at least sulfur dioxide, water, and heat; d) a boiler unit operatively connected to the product stream of the burner and configured to capture heat from the burner, and generate at least a steam stream and an exhaust gas stream having at least SO2; e) an SO2 separation unit operatively connected to the exhaust gas stream of the boiler unit and configured to remove SO2 from the exhaust gas stream and generate an SO2 exit stream; and f) an electrolytic cell operatively connected to the SO2 exit stream and configured to produce hydrogen gas (H2).
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FIG. 1 presents a block diagram of one embodiment of the invention process for converting hydrogen sulfide and/or elemental sulfur into hydrogen and sulfuric acid. - The invention described and claimed below comprises a combination of hydrogen sulfide (H2S), or elemental sulfur (S), combustion, electricity generation from recycled heat, and electrolytic processing of sulfurous acid (H2SO3) to generate hydrogen and sulfuric acid with little CO2 (or SO2) being emitted. There is a plentiful supply of sulfur and H2S in many parts of the world, so SO2 does not have to be recycled from H2SO4 with large expenditure of energy, as it is in related technologies. The required SO2 can be generated from a number of one-pass processes. For example, elemental sulfur can be captured from a Claus sulfur recovery process, wherein SO2 is combined with H2S in a molar ratio of 1:2 to generate approximately 3 moles of elemental sulfur and 2 moles of water. Since the Claus reaction does not typically go to completion, remaining H2S and SO2 must be handled in a “tail gas treating unit” where the remaining gases are captured for further treatment, i.e., combusted in accordance with the invention. Alternatively, the tail gas could be combusted to convert all sulfur-containing compounds to SO2, while capturing the SO2 in a special solvent, as described in WO-A-2006/016979. Another example is the combustion of sulfur-containing coal, or bitumen that generates SO2. Again, selective capture of SO2 by a diamine or other solvent can generate a fairly pure SO2 stream for processing. Disulfide oils, mercaptans, etc., which can be separated from liquid hydrocarbons using caustic processes, may also be considered as combustible feed for this process.
- The ready availability of sulfur and/or hydrogen sulfide, plus oxygen, enables an efficient process for producing both sulfuric acid and hydrogen. The hydrogen gas can be cycled for use in hydrogenation processes or transported and/or packaged for sale and used for developing fuel processes using hydrogen. The sulfuric acid by-product is a commodity product that can be recycled or sold for further use, e.g., chemical process use, or it can be readily disposed of in saline aquifers generally available where sulfur-containing natural gas is recovered. Since the sulfuric acid is a liquid, it is amenable to downhole disposal, whereas solid elemental sulfur must be kept in stockpiles on the surface, or buried at some effort and expense.
- In one possible embodiment, relatively pure H2S is combusted in oxygen according to:
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H2S+ 3/2O2---->SO2+H2O+123.3 kcal/mol, (5) - or elemental sulfur is combusted according to:
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S+O2---->SO2+70.96 kcal/mol. (5a) - According to the invention, the heat generated by these reactions can be used to produce steam, which then can be used to generate electricity for step (c) in the process. The SO2-containing stream is then quenched with water to generate a sulfurous acid solution:
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SO2+H2O---->H2SO3 (6) - The sulfurous acid solution is then routed to an electrolytic cell. Some of the electricity generated via recovery of heat from reaction (5) powers the electrolytic cell, where hydrogen is liberated, and sulfuric acid is generated according to the following:
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H2SO3+H2O+electricity---->H2SO4+H2 (7) - So, the overall result is that water, oxygen, and H2S are consumed, and hydrogen, H2SO4 and excess electricity are generated according to:
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H2S+H2O+ 3/2O2---->H2SO4+H2 (8) - Thus when elemental sulfur (or H2S) is used as a fuel, and pure oxygen as the oxidant, only SO2 (and only a little SO3) is produced, with no need for further purification. However, since H2S is usually contaminated with CO2 or hydrocarbon, there may in fact be some CO2 in the resulting SO2 product.
- The advantage of electrolyzing sulfurous acid instead of pure water is that only 0.17 V is required at 25° C., compared to 1.23 V required for pure water. In principle, only about one-seventh of the power is thus required to generate a given quantity of hydrogen compared to the electrolysis of water.
- An example heat and material balance for the process of
FIG. 1 follows. This illustrative example starts with 1000 kg-mol/hr of acid gas containing 25% H2S, equating to 189 long tons/day (192×103 kg/day) of elemental sulfur. The case assumes that 2% of the H2S combusted is immediately converted to SO3, and must be purged out ahead of the separation unit. - Heat is recovered in the waste heat boiler at 600° F. (315.6° C.), well above the dewpoint of the SO3/H2SO4 present. Ninety-five percent heat recovery and 30% efficient conversion to electricity are assumed. Adequate heat is recovered to regenerate the scrubbing solvent, plus generate enough electricity for the electrolysis. Surplus heat can be used for additional steam or electricity.
- In
FIG. 1 acid gas 1 containing hydrogen sulfide at 250.0 kgmols/hr, carbon dioxide at 705.0 kgmols/hr, water in the form of moisture in an amount of 45.0 kgmol/hr,air 2 containing oxygen in amount of 426.8 kgmols/hr, nitrogen in an amount at 1740.2 kgmols/hr, and water in the form of moisture in an amount of 33.0 kgmols/hr is introduced into a burner, orcombustion chamber 20. After combustion,stream 3 comprises the nitrogen and carbon dioxide in the same amounts as in the feed gas (unreacted), with sulfur dioxide at 245 kgmols/hr, with 5.0 kgmols/hr sulfur trioxide, 328.0 kgmols/hr water, and 49.3 kgmols/hr oxygen. - This hot,
gaseous stream 3 is passed to a boiler unit 21 (i.e., heat exchanger) where 863.3 kgmol/hr water, comprising at least in part condensed steam from theelectrical generator 24, is introduced viastream 13 to provide water for the boiler. Alternatively, a separate water stream (not shown) can be used to source the boiler. In yet another embodiment, water is condensed from the combustedstream 3 to provide the water reagent for reaction (6). Steam containing 3116.2 kgmols/hr water vapor is withdrawn instream 10, and a gaseous, SO2-containingstream 4, containing additionally the CO2, O2, N2, water vapor, and SO3 ofstream 3 exits theboiler unit 21.Stream 4 will generally be maintained at temperatures above the SO3 dewpoint, to avoid condensation of corrosive sulfuric acid, H2SO4. The operating temperature may be as high as 600° F. -
Stream 4 is then quenched by contact with liquid water in a device such as a DynaWave scrubber from MECS, Inc., to reduce the temperature to 100-150 F. Reactive SO3 and H2SO4 dissolve in the aqueous quench stream. A small amount of this stream is purged from the system as a weak solution of H2SO4 inpurge stream 15. The balance of the stream is cooled, and recycled to the scrubbing device. The cooled, H2SO4-free gas stream is then provided for separation where SO2 is preferentially removed by absorbing it into an SO2-selective solvent in a gas-liquid contacting device 22 a. For example, Cansolv Technologies, Inc. markets a diamine solvent that is selective for SO2 over CO2 and other combustion gases. Gases not absorbed into the solution (including trace SO2) are vented throughstream 5. The rich solution is then regenerated in a separate vessel, generally requiring steam (12) to heat the solvent to 250-300° F. Theexit stream 6, cooled to 100-150° F., comprises 240.6 kgmols/hr SO2 and flows from theregeneration unit 22 b at 17-25 psia to theelectrolytic cell 23 at near-atmospheric pressure. A portion of the steam (1,992.2 kgmols/hr) from theboiler unit 21 inexit stream 10 is diverted instream 12 to theregeneration unit 22 b to provide heat. Thus stream 11 to the electricity generator comprises 862.3 kgmols/hr steam. Excess steam in an amount of 261.8 kgmols/hr water is removed fromstream 12 viastream 16 prior to provision to theregeneration unit 22 b. Aseparate stream 15 takes off 5.0 kgmols/hr H2SO4, 3.4 kgmols/hr SO2 (as H2SO3), and 25.0 kgmols/hr water from the scrubbingunit 22 a. Unreacted and by-product gases are vented from the separation unit and removed instream 5, this stream thus comprising all of the CO2, residual O2, and N2, plus 1.0 kgmol/hr SO2, and 328.0 kgmols/hr water vapor.Separate stream 14 returns 1,992.2 kgmols/hr water from theregenerator unit 22 b as condensate to theboiler unit 21. - Electricity is applied to the sulfurous acid solution (H2SO3) in the
electrolytic cell 23 from theelectrical generator 24 that is driven in major part by thesteam stream 11. Additional water (264.7 kgmols/hr) is added to theelectrolytic cell 23 instream 7. Thus with the SO2 instream 6, the electrolysis reaction (7) above, produces 240.6 kgmols/hr H2 which is removed instream 9 and 240.6 kgmol/hr H2SO4 which is removed instream 8. - The spent steam from the electrical generator is condensed in the
generator 24 or in aseparate condensing unit 25, and returned viastream 13 to theboiler unit 21 as the boiler feed water. - The total flow rates, temperatures and pressures in the combined streams above are contained in the following Table 1 by stream number.
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TABLE 1 Stream Total flow Temperature Pressure number (kgmol/hr) (° F./° C.) (psia/kPa) 1 1000 100/38 16.7/115.3 2 2200 100/38 16.7/115.3 3 3072.5 2091/1144 16.2/111.8 4 3072.5 625/329 15.7/108.4 5 2828.5 120/49 14.7101.5 6 240.6 140/60 19.7/136.0 7 264.7 100/38 20.7/142.9 8 264.7 120/49 15.7/108.4 9 240.6 120/49 15.7/108.4 10 3116.2 600/316 615/4246 11 862.3 600/316 615/4246 12 1992.2 600/316 615/4246 13 862.3 140/60 615/4246 14 1992.2 140/60 615/4246 15 33.4 100/38 16.7/115.3 16 261.8 600/316 615/4246 - The foregoing application is directed to particular embodiments of the present invention for the purpose of illustrating it. It will be apparent, however, to one skilled in the art, that many modifications and variations to the embodiments described herein are possible. All such modifications and variations are intended to be within the scope of the present invention, as defined in the appended claims.
Claims (18)
1. A process for producing hydrogen gas comprising:
a. combusting sulfur (S) or hydrogen sulfide (H2S) with oxygen to obtain sulfur dioxide (SO2) and water (H2O), plus heat;
b. adding water to the product of (a) to obtain a sulfurous acid solution (H2SO3 and H2O);
c. applying electrical current to the sulfurous acid solution of (b) to obtain sulfuric acid (H2SO4) and hydrogen gas (H2);
d. using gas-liquid separation to separate the sulfuric acid from the hydrogen gas
to obtain separated components of the sulfuric acid and the hydrogen gas; and,
wherein the heat generated in (a) is used to generate at least a portion of the electricity for the electrical current of (c).
2. The process of claim 1 where said oxygen is provided by introduction of air.
3. The process of claim 1 wherein said hydrogen sulfide in (a) is provided as a raw acid gas from the production of petrochemical products, said gas comprising hydrogen sulfide and carbon dioxide (CO2), and optionally, gaseous hydrocarbons.
4. The process of claim 3 wherein before said water in (b) is added, the product sulfur dioxide is separated from the other gaseous combustion products and unreacted gases.
5. The process of claim 1 wherein said sulfur in (a) is comprised in a combustible, carbon-containing compound, or mixture of compounds.
6. The process of claim 5 wherein said combustible, carbon-containing compound or compounds is selected from one or more of hard coal, soft coal, or coke products.
7. The process of claim 5 wherein said combustible, carbon-containing compound or compounds is a sulfur-laden heavy oil or bitumen.
8. The process of claim 1 , wherein the electrical current is applied using a voltage below 0.50 volts.
9. The process of claim 1 , further comprising removing the sulfuric acid from the process.
10. The process of claim 1 , wherein step (b) is operated at a temperature of about 125° F. (about 52° C.).
11. A system for producing hydrogen gas comprising:
a. an acid gas stream containing hydrogen sulfide;
b. an air stream;
c. a burner configured to burn the acid gas stream and air stream and produce a product stream having at least sulfur dioxide, water, and heat;
d. a boiler unit operatively connected to the product stream of the burner and configured to capture heat from the burner, and generate at least a steam stream and an exhaust gas stream having at least SO2;
e. an SO2 separation unit operatively connected to the exhaust gas stream of the boiler unit and configured to remove SO2 from the exhaust gas stream and generate an SO2 exit stream; and
f. an electrolytic cell operatively connected to the SO2 exit stream and configured to produce hydrogen gas (H2).
12. The system of claim 11 , further comprising: an electrical generator driven by at least a portion of the steam stream and configured to provide electricity to the electrolytic cell.
13. The system of claim 11 , wherein the SO2 separation unit is a solvent based SO2 separation unit.
14. The system of claim 11 , further comprising a water inlet stream configured to provide water to the electrolytic cell.
15. The system of claim 11 , further comprising a regeneration unit operatively connected to the SO2 separation unit and configured to produce at least one water stream, wherein at least a portion of the steam stream is supplied to the regeneration unit and at least a portion of the water stream is supplied to the boiler unit.
16. The system of claim 11 , further comprising:
a. a sulfuric acid purge stream configured to take off at least sulfuric acid from the SO2 separation unit; and
b. a sulfuric acid exit stream configured to remove sulfuric acid from the electrolytic cell.
17. The system of claim 11 , wherein the SO2 separation unit is configured to operate at a temperature of about 100° F. (about 38° C.).
18. The system of claim 15 , wherein the regeneration unit is configured to operate at a temperature of about 300° F. (about 149° C.).
Priority Applications (1)
Application Number | Priority Date | Filing Date | Title |
---|---|---|---|
US12/599,857 US20100230296A1 (en) | 2007-07-23 | 2008-06-17 | Production of Hydrogen Gas From Sulfur-Containing Compounds |
Applications Claiming Priority (3)
Application Number | Priority Date | Filing Date | Title |
---|---|---|---|
US96163907P | 2007-07-23 | 2007-07-23 | |
US12/599,857 US20100230296A1 (en) | 2007-07-23 | 2008-06-17 | Production of Hydrogen Gas From Sulfur-Containing Compounds |
PCT/US2008/007524 WO2009014584A1 (en) | 2007-07-23 | 2008-06-17 | Production of hydrogen gas from sulfur-containing compounds |
Publications (1)
Publication Number | Publication Date |
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US20100230296A1 true US20100230296A1 (en) | 2010-09-16 |
Family
ID=38910941
Family Applications (1)
Application Number | Title | Priority Date | Filing Date |
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US12/599,857 Abandoned US20100230296A1 (en) | 2007-07-23 | 2008-06-17 | Production of Hydrogen Gas From Sulfur-Containing Compounds |
Country Status (5)
Country | Link |
---|---|
US (1) | US20100230296A1 (en) |
EP (1) | EP2167423A4 (en) |
AU (1) | AU2008279815A1 (en) |
CA (1) | CA2689461A1 (en) |
WO (1) | WO2009014584A1 (en) |
Cited By (6)
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US20140080071A1 (en) * | 2012-09-20 | 2014-03-20 | Alstom Technology Ltd | Method and device for cleaning an industrial waste gas comprising co2 |
US8899011B2 (en) | 2011-04-28 | 2014-12-02 | Knauf Gips Kg | Method and device for generating electricity and gypsum from waste gases containing hydrogen sulfide |
US20180119293A1 (en) * | 2016-10-30 | 2018-05-03 | Tolulope Israel Mayomi | Salt cycle for hydrogen production |
US10066834B2 (en) | 2013-01-30 | 2018-09-04 | Bogdan Wojak | Sulphur-assisted carbon capture and storage (CCS) processes and systems |
CN113277639A (en) * | 2021-03-31 | 2021-08-20 | 李晟贤 | Test gas sewage treatment method |
WO2023187781A1 (en) * | 2022-03-31 | 2023-10-05 | Hys Energy Ltd | Hydrogen production by electrochemical decomposition of saline water using sulfur dioxide or bisulfite as an anode depolarizer |
Families Citing this family (2)
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WO2013098329A1 (en) * | 2011-12-27 | 2013-07-04 | Shell Internationale Research Maatschappij B.V. | Method for producing sulphuric acid |
CN109539280B (en) * | 2019-01-09 | 2024-02-09 | 大连昊通节能环保工程技术有限公司 | Ammonia desulfurization waste liquid heat accumulating type incineration SO preparation 2 Process gas technology and system |
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Cited By (7)
Publication number | Priority date | Publication date | Assignee | Title |
---|---|---|---|---|
US8899011B2 (en) | 2011-04-28 | 2014-12-02 | Knauf Gips Kg | Method and device for generating electricity and gypsum from waste gases containing hydrogen sulfide |
US20140080071A1 (en) * | 2012-09-20 | 2014-03-20 | Alstom Technology Ltd | Method and device for cleaning an industrial waste gas comprising co2 |
US9644840B2 (en) * | 2012-09-20 | 2017-05-09 | General Electric Technology Gmbh | Method and device for cleaning an industrial waste gas comprising CO2 |
US10066834B2 (en) | 2013-01-30 | 2018-09-04 | Bogdan Wojak | Sulphur-assisted carbon capture and storage (CCS) processes and systems |
US20180119293A1 (en) * | 2016-10-30 | 2018-05-03 | Tolulope Israel Mayomi | Salt cycle for hydrogen production |
CN113277639A (en) * | 2021-03-31 | 2021-08-20 | 李晟贤 | Test gas sewage treatment method |
WO2023187781A1 (en) * | 2022-03-31 | 2023-10-05 | Hys Energy Ltd | Hydrogen production by electrochemical decomposition of saline water using sulfur dioxide or bisulfite as an anode depolarizer |
Also Published As
Publication number | Publication date |
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WO2009014584A1 (en) | 2009-01-29 |
EP2167423A1 (en) | 2010-03-31 |
AU2008279815A1 (en) | 2009-01-29 |
CA2689461A1 (en) | 2009-01-29 |
EP2167423A4 (en) | 2011-11-09 |
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