Steam reforming

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Steam reforming or steam methane reforming is a chemical synthesis for producing syngas (hydrogen and carbon monoxide) from hydrocarbons such as natural gas. This is achieved in a reformer which reacts steam at high temperature and pressure with methane in the presence of a nickel catalyst. The steam methane reformer is widely used in industry to make hydrogen.

Industrial reforming[edit]

Steam reforming of natural gas is the most common method of producing commercial bulk hydrogen at about 95% of the world production[1][2] of 500 billion m3 in 1998.[3] Hydrogen is used in the industrial synthesis of ammonia and other chemicals.[4] At high temperatures (700 – 1100 °C) and in the presence of a metal-based catalyst (nickel), steam reacts with methane to yield carbon monoxide and hydrogen.

CH4 + H2OCO + 3 H2

Catalysts with high surface-area-to-volume ratio are preferred because of diffusion limitations due to high operating temperature. Examples of catalyst shapes used are spoked wheels, gear wheels, and rings with holes. Additionally, these shapes have a low pressure drop which is advantageous for this application.[5]

Additional hydrogen can be obtained by reacting the CO with water via the water-gas shift reaction.

CO + H2O ⇌ CO2 + H2

The first reaction is strongly endothermic (consumes heat, ΔHr= 206 kJ/mol), the second reaction is mildly exothermic (produces heat, ΔHr= -41 kJ/mol).

The United States produces nine million tons of hydrogen per year, mostly with steam reforming of natural gas. The worldwide ammonia production, using hydrogen derived from steam reforming, was 144 million tonnes in 2014.[6]

This steam reforming process is quite different from and not to be confused with catalytic reforming of naphtha, an oil refinery process that also produces significant amounts of hydrogen along with high octane gasoline.

Steam reforming of natural gas is approximately 65–75% efficient.[7]

Production of H2 and CO from hydrocarbon gases (e.g. natural gas) is performed by two well-known "primary" and "secondary" reformers. Steam methane reforming (SMR) and autothermal reformer (ATR) are two industrial examples of the primary and secondary reformers, respectively. Each of which uses only special characteristics. On the other hand, the process of combined reforming utilizes both of primary and secondary tools for production of synthesis gas, as it is commonly practiced in ammonia manufacturing. For the case of methanol, ATR is fed with nearly pure oxygen (99.5%) rather than air since the presence of excessive N2 in the syngas would overburden compression and retard the methanol production. The ATR reformer consists of a partial oxidation (POX) chamber (usually non-catalytic medium) and a fixed bed catalytic section. The catalytic fixed bed not only adjusts the H2/CO ratio, but also destroys any probable soot and precursor (e.g. ethylene and acetylene) that may be formed in the POX chamber. Natural gas (NG) is partially oxidized in the combustion chamber by oxygen or air (as an oxidant). Steam to carbon (S/C) ratio that is usually 0.6 in the oxygen-based case has been commercialized by Haldor-Topose Company.[8]

Autothermal reforming[edit]

Autothermal reforming (ATR) uses oxygen and carbon dioxide or steam in a reaction with methane to form syngas. The reaction takes place in a single chamber where the methane is partially oxidized. The reaction is exothermic due to the oxidation. When the ATR uses carbon dioxide the H2:CO ratio produced is 1:1; when the ATR uses steam the H2:CO ratio produced is 2.5:1

The reactions can be described in the following equations, using CO2:

2CH4 + O2 + CO2 → 3H2 + 3CO + H2O

And using steam:

4CH4 + O2 + 2H2O → 10H2 + 4CO

The outlet temperature of the syngas is between 950-1100 C and outlet pressure can be as high as 100 bar.[9]

The main difference between SMR and ATR is that SMR only uses oxygen via air for combustion as a heat source to create steam, while ATR directly combusts oxygen. The advantage of ATR is that the H2:CO can be varied, this is particularly useful for producing certain second generation biofuels, such as DME which requires a 1:1 H2:CO ratio.

Partial oxidation[edit]

Partial oxidation (POX) is a type of chemical reaction. It occurs when a substoichiometric fuel-air mixture is partially combusted in a reformer, creating a hydrogen-rich syngas which can then be put to further use.

Partial oxidation is an exothermic process (it gives off heat). The process is, typically, much faster than steam reforming and requires a smaller reactor vessel. As can be seen in chemical reactions of partial oxidation, this process initially produces less hydrogen per unit of the input fuel than is obtained by steam reforming of the same fuel.[10] Nevertheless, tendency to soot formation and relatively low hydrogen production yield are among the major drawbacks of this method.[11]

Advantages and disadvantages[edit]

The capital cost of steam reforming plants is prohibitive for small to medium size applications because the technology does not scale down well. Conventional steam reforming plants operate at pressures between 200 and 600 psi (14 - 40 bar) with outlet temperatures in the range of 815 to 925 °C. However, analyses have shown that even though it is more costly to construct, a well-designed SMR can produce hydrogen more cost-effectively than an ATR.[12]

Reforming for combustion engines[edit]

Flared gas and vented VOCs are known problems in the offshore industry and in the on-shore oil and gas industry, since both emit unnecessary greenhouse gases into the atmosphere.[13] Reforming for combustion engines utilizes steam reforming technology for converting waste gases into a source of energy.[14]

Reforming for combustion engines is based on steam reforming, where non-methane hydrocarbons (NMHCs) of low quality gases are converted to synthesis gas (H2 + CO) and finally to methane (CH4), carbon dioxide (CO2) and hydrogen (H2) - thereby improving the fuel gas quality (methane number).[15]

In contrast to conventional steam reforming, the process is operated at lower temperatures and with lower steam supply, allowing a high content of methane (CH4) in the produced fuel gas. The main reactions are:

Steam reforming:

CnHm + n H2O ⇌ (n + ​m2) H2 + n CO


CO + 3 H2 ⇌ CH4 + H2O

Water-gas shift:

CO + H2O ⇌ H2 + CO2

Reforming for fuel cells[edit]

There is also interest in the development of much smaller units based on similar technology to produce hydrogen as a feedstock for fuel cells.[16] Small-scale steam reforming units to supply fuel cells are currently the subject of research and development, typically involving the reforming of methanol, but other fuels are also being considered such as propane, gasoline, autogas, diesel fuel, and ethanol.[17][18]

Advantages of reforming for supplying fuel cells[edit]

Steam reforming of gaseous hydrocarbons is seen as a potential way to provide fuel for fuel cells. The basic idea for vehicle on-board reforming is that for example a methanol tank and a steam reforming unit would replace the bulky pressurized hydrogen tanks that would otherwise be necessary. This might mitigate the distribution problems associated with hydrogen vehicles;[19] however the major market players discarded the approach of on-board reforming as impractical.[citation needed] (At high temperatures see above).

Disadvantages of reforming for supplying fuel cells[edit]

The reformer–fuel-cell system is still being researched but in the near term, systems would continue to run on existing fuels, such as natural gas or gasoline or diesel. However, there is an active debate about whether using these fuels to make hydrogen is beneficial while global warming is an issue. Fossil fuel reforming does not eliminate carbon dioxide release into the atmosphere but reduces the carbon dioxide emissions and nearly eliminates carbon monoxide emissions as compared to the burning of conventional fuels due to increased efficiency and fuel cell characteristics.[20] However, by turning the release of carbon dioxide into a point source rather than distributed release, carbon capture and storage becomes a possibility, which would prevent the carbon dioxide's release to the atmosphere, while adding to the cost of the process.

The cost of hydrogen production by reforming fossil fuels depends on the scale at which it is done, the capital cost of the reformer and the efficiency of the unit, so that whilst it may cost only a few dollars per kilogram of hydrogen at industrial scale, it could be more expensive at the smaller scale needed for fuel cells.[21]

Current challenges with reformers supplying fuel cells[edit]

However, there are several challenges associated with this technology:

  • The reforming reaction takes place at high temperatures, making it slow to start up and requiring costly high temperature materials.
  • Sulfur compounds in the fuel will poison certain catalysts, making it difficult to run this type of system from ordinary gasoline. Some new technologies have overcome this challenge with sulfur-tolerant catalysts.
  • Coking would be another cause of catalyst deactivation during steam reforming. High reaction temperatures, low steam-to-carbon ratio (S/C), and the complex nature of sulfur-containing commercial hydrocarbon fuels make coking especially favorable. Olefins, typically ethylene, and aromatics are well known carbon-precursors, hence their formation must be reduced during the SR. Additionally, catalysts with lower acidity were reported to be less prone to coking by suppressing dehydrogenation reactions. H2S, the main product in the reforming of organic sulfur, can bind to all transition metal catalysts to form metal–sulfur bonds and subsequently reduce catalyst activity by inhibiting the chemisorption of reforming reactants. Meanwhile, the adsorbed sulfur species increases the catalyst acidity, and hence indirectly promotes coking. Precious metal catalysts such as Rh and Pt have lower tendencies to form bulk sulfides than other metal catalysts such as Ni. Rh and Pt are less prone to sulfur poisoning by only chemisorbing sulfur rather than forming metal sulfides.[22]
  • Low temperature polymer fuel cell membranes can be poisoned by the carbon monoxide (CO) produced by the reactor, making it necessary to include complex CO-removal systems. Solid oxide fuel cells (SOFC) and molten carbonate fuel cells (MCFC) do not have this problem, but operate at higher temperatures, slowing start-up time, and requiring costly materials and bulky insulation.
  • The thermodynamic efficiency of the process is between 70% and 85% (LHV basis) depending on the purity of the hydrogen product.

See also[edit]


  1. ^ Ogden, J.M. (1999). "Prospects for building a hydrogen energy infrastructure". Annual Review of Energy and the Environment. 24: 227–279. doi:10.1146/
  2. ^ "Hydrogen Production: Natural Gas Reforming". Department of Energy. Retrieved 6 April 2017.
  3. ^ Rostrup-Nielsen. "Large-scale Hydrogen Production" (PDF). Haldor Topsøe. p. 3. The total hydrogen market was in 1998 390·10^9 Nm3/y + 110·10^9 Nm3/y co-production.
  4. ^ Crabtree, George W.; Dresselhaus, Mildred S.; Buchanan, Michelle V. (2004). The Hydrogen Economy (PDF) (Technical report).
  5. ^ Reimert, Rainer; Marschner, Friedemann; Renner, Hans-Joachim; Boll, Walter; Supp, Emil; Brejc, Miron; Liebner, Waldemar; Schaub, Georg (2011). "Gas Production, 2. Processes". Ullmann's Encyclopedia of Industrial Chemistry. doi:10.1002/14356007.o12_o01. ISBN 978-3-527-30673-2.
  6. ^ Nitrogen (Fixed)—Ammonia (PDF) (Report). United States Geological Survey. January 2016.
  7. ^ "Hydrogen Production – Steam Methane Reforming (SMR)" (PDF), Hydrogen Fact Sheet, archived from the original (PDF) on 4 February 2006, retrieved 28 August 2014
  8. ^ Ebrahimi, Hadi; Behroozsarand, Alireza; Zamaniyan, Akbar (2010). "Arrangement of primary and secondary reformers for synthesis gas production". Chemical Engineering Research and Design. 88 (10): 1342–1350. doi:10.1016/j.cherd.2010.02.021.
  9. ^ Topsoe ATR
  10. ^
  11. ^ Nourbakhsh, Hessamodin; Rahbar Shahrouzi, Javad; Zamaniyan, Akbar; Ebrahimi, Hadi; Jafari Nasr, Mohammad Reza (2018). "A thermodynamic analysis of biogas partial oxidation to synthesis gas with emphasis on soot formation". International Journal of Hydrogen Energy. 43 (33): 15703–15719. doi:10.1016/j.ijhydene.2018.06.134.
  12. ^ AIA: Software Analyzes Cost of Hydrogen Production - Archives - ASSEMBLY
  13. ^ "Atmospheric Emissions". Archived from the original on 2013-09-26.
  14. ^ "Wärtsilä Launches GasReformer Product For Turning Oil Production Gas Into Energy". Marine Insight. 18 March 2013. Archived from the original on 2015-05-11.
  15. ^ "Method of operating a gas engine plant and fuel feeding system of a gas engine".
  16. ^ "Fossil fuel processor". 2000-10-04.
  17. ^ Wyszynski, Miroslaw L.; Megaritis, Thanos; Lehrle, Roy S. (2001). Hydrogen from Exhaust Gas Fuel Reforming: Greener, Leaner and Smoother Engines (PDF) (Technical report). Future Power Systems Group, The University of Birmingham.
  18. ^ "Commonly used fuel reforming today". 2000-10-04.
  19. ^ Advantage of fossil fuel reforming
  20. ^ Fossil fuel reforming not eliminating any carbon dioxides
  21. ^ Doty, F. David (2004). "A Realistic Look at Hydrogen Price Projections". CiteSeerX Cite journal requires |journal= (help)[self-published source?]
  22. ^ Zheng, Qinghe; Janke, Christiane; Farrauto, Robert (2014). "Steam reforming of sulfur-containing dodecane on a Rh–Pt catalyst: Influence of process parameters on catalyst stability and coke structure". Applied Catalysis B: Environmental. 160-161: 525–533. doi:10.1016/j.apcatb.2014.05.044.