Classifications

• • C—CHEMISTRY; METALLURGY
  • C10—PETROLEUM, GAS OR COKE INDUSTRIES; TECHNICAL GASES CONTAINING CARBON MONOXIDE; FUELS; LUBRICANTS; PEAT
  • C10K—PURIFYING OR MODIFYING THE CHEMICAL COMPOSITION OF COMBUSTIBLE GASES CONTAINING CARBON MONOXIDE
  • C10K3/00—Modifying the chemical composition of combustible gases containing carbon monoxide to produce an improved fuel, e.g. one of different calorific value, which may be free from carbon monoxide
  • C10K3/02—Modifying the chemical composition of combustible gases containing carbon monoxide to produce an improved fuel, e.g. one of different calorific value, which may be free from carbon monoxide by catalytic treatment
  • C10K3/026—Increasing the carbon monoxide content, e.g. reverse water-gas shift [RWGS]
• • C—CHEMISTRY; METALLURGY
  • C01—INORGANIC CHEMISTRY
  • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
  • C01B3/00—Hydrogen; Gaseous mixtures containing hydrogen; Separation of hydrogen from mixtures containing it; Purification of hydrogen; Reversible storage of hydrogen
  • C01B3/02—Production of hydrogen; Production of gaseous mixtures containing hydrogen
  • C01B3/32—Production of hydrogen; Production of gaseous mixtures containing hydrogen by reaction of gaseous or liquid organic compounds with gasifying agents, e.g. water, carbon dioxide or air
  • C01B3/34—Production of hydrogen; Production of gaseous mixtures containing hydrogen by reaction of gaseous or liquid organic compounds with gasifying agents, e.g. water, carbon dioxide or air by reaction of hydrocarbons with gasifying agents
• • C—CHEMISTRY; METALLURGY
  • C01—INORGANIC CHEMISTRY
  • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
  • C01B3/00—Hydrogen; Gaseous mixtures containing hydrogen; Separation of hydrogen from mixtures containing it; Purification of hydrogen; Reversible storage of hydrogen
  • C01B3/02—Production of hydrogen; Production of gaseous mixtures containing hydrogen
  • C01B3/04—Production of hydrogen; Production of gaseous mixtures containing hydrogen by decomposition of inorganic compounds
• • C—CHEMISTRY; METALLURGY
  • C01—INORGANIC CHEMISTRY
  • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
  • C01B3/00—Hydrogen; Gaseous mixtures containing hydrogen; Separation of hydrogen from mixtures containing it; Purification of hydrogen; Reversible storage of hydrogen
  • C01B3/02—Production of hydrogen; Production of gaseous mixtures containing hydrogen
  • C01B3/06—Production of hydrogen; Production of gaseous mixtures containing hydrogen by reaction of inorganic compounds containing electro-positively bound hydrogen with inorganic reducing agents
  • C01B3/12—Production of hydrogen; Production of gaseous mixtures containing hydrogen by reaction of inorganic compounds containing electro-positively bound hydrogen with inorganic reducing agents by reaction of water vapour with carbon monoxide
• • C—CHEMISTRY; METALLURGY
  • C01—INORGANIC CHEMISTRY
  • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
  • C01B32/00—Carbon; Compounds thereof
  • C01B32/40—Carbon monoxide
• • C—CHEMISTRY; METALLURGY
  • C10—PETROLEUM, GAS OR COKE INDUSTRIES; TECHNICAL GASES CONTAINING CARBON MONOXIDE; FUELS; LUBRICANTS; PEAT
  • C10G—CRACKING HYDROCARBON OILS; PRODUCTION OF LIQUID HYDROCARBON MIXTURES, e.g. BY DESTRUCTIVE HYDROGENATION, OLIGOMERISATION, POLYMERISATION; RECOVERY OF HYDROCARBON OILS FROM OIL-SHALE, OIL-SAND, OR GASES; REFINING MIXTURES MAINLY CONSISTING OF HYDROCARBONS; REFORMING OF NAPHTHA; MINERAL WAXES
  • C10G2/00—Production of liquid hydrocarbon mixtures of undefined composition from oxides of carbon
  • C10G2/30—Production of liquid hydrocarbon mixtures of undefined composition from oxides of carbon from carbon monoxide with hydrogen
  • C10G2/32—Production of liquid hydrocarbon mixtures of undefined composition from oxides of carbon from carbon monoxide with hydrogen with the use of catalysts
• • C—CHEMISTRY; METALLURGY
  • C01—INORGANIC CHEMISTRY
  • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
  • C01B2203/00—Integrated processes for the production of hydrogen or synthesis gas
  • C01B2203/02—Processes for making hydrogen or synthesis gas
  • C01B2203/0205—Processes for making hydrogen or synthesis gas containing a reforming step
  • C01B2203/0211—Processes for making hydrogen or synthesis gas containing a reforming step containing a non-catalytic reforming step
  • C01B2203/0216—Processes for making hydrogen or synthesis gas containing a reforming step containing a non-catalytic reforming step containing a non-catalytic steam reforming step
• • C—CHEMISTRY; METALLURGY
  • C01—INORGANIC CHEMISTRY
  • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
  • C01B2203/00—Integrated processes for the production of hydrogen or synthesis gas
  • C01B2203/06—Integration with other chemical processes
  • C01B2203/062—Hydrocarbon production, e.g. Fischer-Tropsch process
• • C—CHEMISTRY; METALLURGY
  • C01—INORGANIC CHEMISTRY
  • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
  • C01B2203/00—Integrated processes for the production of hydrogen or synthesis gas
  • C01B2203/08—Methods of heating or cooling
  • C01B2203/0805—Methods of heating the process for making hydrogen or synthesis gas
  • C01B2203/0811—Methods of heating the process for making hydrogen or synthesis gas by combustion of fuel
  • C01B2203/0822—Methods of heating the process for making hydrogen or synthesis gas by combustion of fuel the fuel containing hydrogen
• • C—CHEMISTRY; METALLURGY
  • C01—INORGANIC CHEMISTRY
  • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
  • C01B2203/00—Integrated processes for the production of hydrogen or synthesis gas
  • C01B2203/12—Feeding the process for making hydrogen or synthesis gas
  • C01B2203/1205—Composition of the feed
  • C01B2203/1211—Organic compounds or organic mixtures used in the process for making hydrogen or synthesis gas
  • C01B2203/1235—Hydrocarbons
• • C—CHEMISTRY; METALLURGY
  • C01—INORGANIC CHEMISTRY
  • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
  • C01B2203/00—Integrated processes for the production of hydrogen or synthesis gas
  • C01B2203/12—Feeding the process for making hydrogen or synthesis gas
  • C01B2203/1205—Composition of the feed
  • C01B2203/1211—Organic compounds or organic mixtures used in the process for making hydrogen or synthesis gas
  • C01B2203/1235—Hydrocarbons
  • C01B2203/1241—Natural gas or methane
• • C—CHEMISTRY; METALLURGY
  • C01—INORGANIC CHEMISTRY
  • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
  • C01B2203/00—Integrated processes for the production of hydrogen or synthesis gas
  • C01B2203/80—Aspect of integrated processes for the production of hydrogen or synthesis gas not covered by groups C01B2203/02 - C01B2203/1695
  • C01B2203/86—Carbon dioxide sequestration

Definitions

• the present application relates to a method and system for producing a synthesis or reducing gas comprising carbon monoxide (CO) and hydrogen (H 2 ) from various sources of carbon and hydrogen (H 2 ). More particularly, the method of producing the synthesis or reducing gas uses at least a first source of carbon which is CO 2 and at least a second source of carbon comprising a hydrocarbon.
• Carbon monoxide and hydrogen gas mixtures - commonly referred to as syngas or reducing gas - are used in the manufacture of a wide spectrum of commodities such as synthetic liquid hydrocarbons and alcohols. Additionally, they can be used for the production of reducing gases in the metallurgical industry (e.g. direct reduction of iron oxides). To produce such gases, including carbon monoxide (CO), a carbon source is required to fuel the process.
• the carbon source can come from fossil resources such as natural gas or coal. Using a carbon source and water vapor, a mixture of carbon monoxide and hydrogen can be produced. Well-known approaches to doing this include natural gas reforming techniques and coal steam gasification.
• GHG Greenhouse Gas
• CO2 is found in ambient air, but also in atmospheric emissions from industrial processes that emit CO2 (e.g. cement works, aluminum works, steelworks, etc.).
• CO2 Carbon Capture Utilization
• the CO2 thus captured can be used as a carbon source for the production of synthesis gas for the production of a wide spectrum of products with improved carbon neutrality, ie, whose production and use cycle involves little net GHG emissions, when CO2 comes from biogenic sources or ambient air. It is thus possible to produce synthetic fuels with increased carbon neutrality, which can be used in existing infrastructure. It is also possible to produce synthesis gases that can be used for the formulation of reducing gases for the metallurgical industry (eg, for the direct reduction of metal oxides).
• the water vapor generated by the oxy-flame following the reaction (B) and also by the RWGS reaction (A), during the production of the synthesis gas, can be considered as a "loss" of hydrogen and have an impact on operating costs.
• a method that can take advantage of this generated water vapor, by using it to produce a synthesis gas, would be desirable.
• the present technology relates to a method of producing synthesis gas comprising carbon monoxide (CO) and hydrogen (H 2 ), the method comprising: feeding an oxidizing flow comprising oxygen (O 2 ) and a first reducing flow comprising hydrogen (H 2 ) in at least a first zone of at least one reactor, where the oxidizing flow and/or the first reducing flow further comprises a first source of carbon which is CO 2 ; generation of an oxy-flame in the first zone by reaction between the oxygen of the oxidizing flow and the hydrogen of the first reducing flow, and production of a first gas comprising at least carbon monoxide (CO) and steam of water (H 2 O) by bringing the oxidizing flow and the first reducing flow into contact with the oxy-flame; feeding into the reactor a second reducing flow comprising a second carbon source comprising at least one hydrocarbon; generation in a second reaction zone of the reactor of a second gas comprising the synthesis gas, from the first gas coming from the first reaction zone and the
• the production of the first gas comprising at least carbon monoxide (CO) and water vapor (H 2 O), in the first zone is carried out at a temperature of at least 1000°C and at most 2400°C.
• the generation of the synthesis gas, in the second zone is carried out at a temperature lower than a temperature in the first zone.
• the oxidizing flow is supplied in a lower and central part of the first zone and the first reducing flow is supplied in the lower part of the first zone on the periphery of the oxidizing flow.
• part of the second gas is recycled in the first reducing flow.
• the generation of the synthesis gas, in the second zone is carried out at a temperature lower than a temperature in the first zone.
• the second gas generated in the second zone comprises the synthesis gas and residual CO2 and the system further comprises means for recycling part of the second gas in the first zone.
• only the oxidizing flow comprises CO2.
• the hydrogen present in the first reducing flow comprises hydrogen resulting from a water electrolysis reaction in an electrolyser which is powered by electricity produced from a renewable source (e.g. , produced from solar energy, wind energy, hydraulic energy, biomass or geothermal energy) or nuclear energy, and hydrogen resulting from a steam reforming reaction of natural gas or methane in a process for which the CO2 generated is at least partly captured and sequestered.
• a renewable source e.g. , produced from solar energy, wind energy, hydraulic energy, biomass or geothermal energy
• nuclear energy e.g., produced from solar energy, wind energy, hydraulic energy, biomass or geothermal energy
• the hydrogen present in the first reducing flow further comprises hydrogen resulting from a methane pyrolysis reaction.
• the second reducing flow further comprises hydrogen (H 2 ).
• the hydrogen present in the second reducing flow results from a steam reforming reaction of natural gas or methane in a process for which the CO 2 generated is at least partly captured and sequestered.
• the oxygen (O 2 ) present in the oxidizing flow results from a water electrolysis reaction.
• Figure 7 represents a schematic vertical sectional view of a reactor which can be used to carry out the present method and which is used for the examples. The figure shows the general arrangement of the tubes for this reactor.
• synthesis gas reducing gas
• syngas a gas mixture comprising at least carbon monoxide (CO) and hydrogen (H2).
• the synthesis gas, reducing gas or syngas may include CO2.
• flow is used to describe the different gas flows which are involved in the production of the synthesis gas, in the different zones, inside the reactor.
• the oxy-flame can generate ionic species and free radicals that can promote the conversion of the carbon source to CO.
• the production of carbon monoxide and water vapor in the first reaction zone 12 can be carried out in the absence of a catalyst such as solid catalysts used conventionally.
• the combustion of hydrogen (H 2 ) in the presence of oxygen (O 2 ) which produces the oxy-flame can be initiated using an ignition device.
• the oxy-flame can make it possible to reach a temperature, in the first reaction zone, of at least 600°C.
• the temperature reached in the first zone 12 is at least 1000°C and at most 2400°C.
• the reactor can be provided with thermal insulation around the reactive zones to minimize heat loss and thus maintain the temperature in the reactor at a high enough level to support the reactions.
• the production of the first gas comprising at least carbon monoxide (CO) and water vapor (H 2 O) in the first zone 12 can be carried out at a temperature between approximately 1000°C and approximately 2300°C, or between approximately 1000°C and approximately 2200°C, or between approximately 1000°C and approximately 2100°C, or between approximately 1000°C and approximately 2000°C, or between approximately 1000°C and approximately 1900°C.
• the first reducing flow 18 may comprise a mixture of green hydrogen and blue hydrogen, or a mixture of green hydrogen and turquoise hydrogen, a mixture of blue hydrogen and turquoise hydrogen, a mixture of green hydrogen, blue hydrogen and turquoise hydrogen.
• hydrogen, oxygen and CO2 are supplied into the first zone 12 in an H2/O2 molar ratio of at least 2, and an H2/CO2 molar ratio of at least 1.8 .
• hydrogen, oxygen and CO2 can be supplied into the first zone in an H2/O2 molar ratio of between 2 and 10, and an H2/CO2 molar ratio of between 1.8 and 9.
• hydrogen and oxygen can be supplied into the first zone 12 with an H2/O2 molar ratio of approximately 2, approximately 3, approximately 4, approximately 5, approximately 6, d 'about 7, about 8, about 9, or about 10, or any value between these values.
• the O2/CO2 molar ratio is approximately 0.5, or approximately 1, or approximately 2, or approximately 3, or approximately 4, or approximately 6, or no matter what value is between these values.
• the H2/O2, H2/O2 and O2/CO2 molar ratios can be adjusted according to the quantity of other gases sent into the reactor if necessary, and according to the ratio of CO and H 2 desired in the final synthesis gas.
• the second reducing flow 24 comprises at least one hydrocarbon as a second carbon source, and the generation of the synthesis gas, in the second reaction zone 14, is carried out in part by steam reforming of the hydrocarbon(s) with the water vapor included in the first gas and/or water vapor possibly present in the reducing flow 24 as mentioned above.
• This carbon source can be a fossil or renewable hydrocarbon, preferably methane or fossil or renewable natural gas (RNG).
• RNG fossil or renewable natural gas
• the second source of carbon is methane which comes from biogas.
• the reaction (E), and the reaction (F) in the presence of residual CO2 occur in the second zone 14.
• hydrogen can also be supplied to the second zone 14 to produce the synthesis gas.
• additional hydrogen is supplied into zone 14 by the reducing flow 24, on the one hand it is possible to balance the composition of the synthesis gas in order to respect equations (C) and (D) as mentioned previously and, on the other hand, on the other hand, reduce water vapor and residual CO 2 in this area.
• the second reducing flow 24 may contain, in addition to the inputs described above, water vapor and a small quantity of impurities.
• the reducing flow 24 fed into the second zone 14 may comprise methane (CH 4 ) and optionally water vapor (H 2 O) with a molar ratio of water vapor (H 2 O) compared to CH 4 which can be between 0 and 2.
• the reducing flow 24 fed into the second zone 14 may also comprise organic compounds derived from biomass, that is to say comprising biogenic carbon.
• organic compounds comprising biogenic carbon can have the formula CJHpOy with a varying from 1 to 5, p varying from 2 to 10 and y varying from 1 to 4.
• the reaction in the second zone 14 of the reactor is carried out at a temperature which is lower than the temperature in the first zone 12.
• the generation of the synthesis gas, in the second zone 12 can be carried out at a temperature of at least 700°C and at most 1500°C.
• the temperature in the second reaction zone may be between about 700°C and about 1000°C.
• the temperature in the second reaction zone can also be between approximately 700°C and approximately 1400°C, between approximately 700°C and approximately 1300°C, between approximately 700°C and approximately 1200°C, between approximately 700°C and approximately 1200°C.
• the desired temperature can be reached in the second reaction zone 14 by using a wall that is less insulated than, for example, the wall of the reactor in the first zone. It is also possible, in certain cases, to use a cooling system to have the desired temperature in the second zone of the reactor.
• the production of synthesis gas in the second zone 14 of the reactor can be carried out in the absence of catalyst such as solid catalysts (e.g., metal catalysts) as used conventionally.
• catalyst such as solid catalysts (e.g., metal catalysts) as used conventionally.
• FIG. 1 to 3 A schematic representation of a reactor which can be used for the implementation of the present method, is shown in Figures 1 to 3.
• the design of the reactor can vary and/or a system comprising several reactors can be used.
• Other examples of designs are shown in Figures 4 to 7 which will be discussed below.
• the design of the reactor or system is not limited to the representations of Figures 1 to 7, and this design can be adjusted as long as it allows the reactions involved for the production of the synthesis gas to be carried out, according to the parameters described. above.
• a cylindrical reactor can be used which includes two reaction zones, as described above. According to certain embodiments, each of the two zones can itself be cylindrical.
• the reactor 10 may comprise a first means for supplying the oxidizing flow 16 in a lower and central part of the first zone 12 and a second means for supplying the first reducing flow 18 in the lower part of the first zone on the periphery of the oxidizing flow.
• the reactor may comprise a first central tube through which the oxidizing flow 16 is supplied into the first zone 12 and an annular space extending perpendicularly between an external wall of the central tube and an internal wall of the first zone 12 to supply the first reducing flow 18.
• the reactor may comprise a third means for supplying the second reducing flow 24 in the second zone 14.
• this third means may consist of an opening formed by an annular space extending between an external wall of the first zone 12 and an internal wall of the second zone 14.
• the annular space through which the second reducing flow 24 is supplied into the reactor can extend between the external wall of the first zone 12 and the internal wall of the second zone 14 in an upper region of the first zone and a lower region of the second zone.
• the inputs of each of the streams 16, 18 and 24 can be at the same level as shown in Figure 7 for example.
• the reactor can also include an outlet 28 in an upper part of the second zone 14 to recover the gas formed in the second zone which includes the synthesis gas.
• the production of the synthesis gas can be carried out using a reactor comprising a plurality of first zones 12 and a second common zone 14 ( Figures 5 and 6). More particularly, in this embodiment, each first zone 12 of the reactor is supplied by the oxidizing flow and the first reducing flow to produce the first gas in each first zone, and the second common zone 14 is supplied by the second reducing flow 24 and receives the first gas produced in each first zone to generate the second gas in the second common zone.
• the first zones 12 operate in parallel and each has an oxy-flame.
• the second reducing flow 24 can be fed into the second common zone 14 by at least one input which can be located in a peripheral zone of the second zone.
• several inputs can be provided to supply the second reducing flow 24 in the second zone. For example, entrances can be provided at several locations in a peripheral zone of the second zone and near the lower part of its internal wall.
• the synthesis gas which is obtained at the outlet of the reactor is generally cooled and then used in a subsequent chemical synthesis.
• the method described in this document can make it possible to produce synthesis gases based on CO and H 2 which are balanced, ie, with appropriate proportions of CO and H 2 , to then allow the production of a variety of products by conventional chemical syntheses.
• It is also possible to adjust the proportion of CO and H 2 in the synthesis gas by controlling the temperature and possibly the pressure in each reaction zone of the reactor.
• the syngas produced by the present method can be used to produce a large number of commodity chemicals and fuels.
• these products we find in particular methanol and hydrocarbons such as those found in motor gasoline, diesel, kerosene, to name a few examples.
• the synthesis gas produced by the present method is used as a reducing agent for the metallurgical industry, among others, for the direct reduction of metal oxides, particularly iron oxides.
• the method of producing synthesis gas described above and the reactor that can be used to carry out this method therefore have several advantages.
• the reagents are easily accessible and can be derived from renewable sources and the method is simple to implement. It is not necessary to resort to the use of solid catalysts.
• a low carbon footprint eg, green, blue, turquoise and/or pink hydrogen.
• the method also makes it possible to take advantage of the water vapor generated during the reduction of CO2, by using it to produce the synthesis gas. This avoids having to condense a large quantity of water as is done in other known methods and avoids an indirect loss of hydrogen via water vapor.
• the method has a beneficial environmental effect by recycling CO2 while allowing the efficient conversion of other carbon sources such as fossil hydrocarbons, such as methane for example.
• the method allows for an overall conversion to CO of the carbon entering the reactor, which is significant while being flexible through the relative and in situ conversions of CO2 and hydrocarbon(s).
• the end of the central tube defines the passage of the oxidizing flow 16 of the first zone of the reactor, while the annular space between the external diameter of the central tube and the internal diameter of the middle tube is found to define the passage of the reducing flow 18 of the first reaction zone. Finally, the annular space between the inner diameter of the outer tube and the outer diameter of the middle tube is found to define the passage of the second reducing flow of the second reaction zone 24.
• the external alumina tube which defines the wall of the reaction chamber, is itself surrounded - over the entire length of the reactor - by an insulating envelope based on calcium silicate (thermal conductivity of 0.3 W/ mK, density of 1.36 g/cm 3 ) of cylindrical shape having an external diameter of 132 mm and an internal diameter of 20 mm (not shown in Figure 7).
• the purpose of the insulating envelope is to ensure a certain thermal insulation of the reactor so as to minimize heat losses.
• oxygen is mixed with CO2 and this mixture constitutes the oxidizing flow 16 of the first reaction zone.
• the hydrogen supplied constitutes the reducing flow 18 of the first zone.
• methane is supplied to constitute the reducing flow 24 of the second zone while for the second example, it is a mixture of methane and water vapor which constitutes the reducing flow 24 of the second zone.
• the methane-water vapor mixture is produced by a device for hot saturation of the methane flow in the presence of a controlled flow of water.
• the table provides the analysis of the gas exiting the reactor as determined by mass spectrometry. From the volume composition of the gas, the ratio S equal to (H 2 -CO2)/(CO+CO2) is calculated on the basis of the respective volume fraction of each of the gases H 2 , CO2 and CO of the dry gas obtained . The conversion rate of methane and that of CO2 are calculated from the atomic balances and from the composition of the gas (dry basis) as obtained by gas analysis by mass spectrometry. In the table, we also present the conversion rate into CO, of the total carbon entering in the reactor, i.e. the carbon contained in the CO2 supplied plus the carbon contained in the CH 4 supplied.
• the table also presents the temperature as measured using a thermocouple located 25 mm from outlet 28 of the reactor.
• the measured temperature value is used to calculate the average residence time of the reactants (i.e. all of the gases supplied) in the reactor, based on the reaction volume as described above and considering that the reactor operates at atmospheric pressure.
• Examples 1, 2 and 3 as presented in Table 1 demonstrate the flexibility of the method and the system according to the present description. This flexibility essentially results from the geometric distinction of the reactive zones in the reactor.
• the configuration used in these examples offers the advantage of obtaining a fairly wide and flexible range of relative and in situ conversions of CH 4 and CO2 while ensuring an overall and significant conversion of the incoming carbon. in the reactor (at least 70%).
• the results of Examples 1 and 2 show that the supply of water vapor is not critical for achieving high methane conversion. Indeed, adding water to the second zone only slightly increases the conversion of methane (from 79% to 83%) (by reaction (E)) but promotes a reduction in the conversion of CO2 probably into favoring the opposite of reaction (A).
• Example 3 show that a high and equivalent conversion of CH 4 and CO2 is achievable by the addition of a certain quantity of excess hydrogen in the first zone (9 vs. 6 sL/min). Indeed, this excess hydrogen seems to help convert CO2 more efficiently in the first zone by reaction (A)).
• the conversion of CH 4 is not significantly affected by the increase in the conversion of CO2 due to the fact that this CH 4 is supplied separately in the second zone.

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Citations (6)

• 2022
  • 2022-04-07 CA CA3154398A patent/CA3154398A1/fr active Pending
• 2023
  • 2023-04-06 CA CA3246738A patent/CA3246738A1/fr active Pending
  • 2023-04-06 US US18/848,649 patent/US20250066190A1/en active Pending
  • 2023-04-06 CN CN202380032793.2A patent/CN118973950A/zh active Pending
  • 2023-04-06 WO PCT/CA2023/050479 patent/WO2023193115A1/fr not_active Ceased
  • 2023-04-06 EP EP23784049.1A patent/EP4504649A1/fr active Pending
  • 2023-04-06 JP JP2024559014A patent/JP2025511387A/ja active Pending
• 2024
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