{ "id": "epkzvvhkgr", "slug": "water-gas-shift-reaction", "title": "Water-gas shift reaction", "updated": "2026-10-21", "topic_path": [ { "id": "physical", "label": "Physical world and mathematics", "api_url": "https://www.edgepedia.org/api/v1/topics/physical" }, { "id": "physical.chemistry", "label": "Chemistry", "api_url": "https://www.edgepedia.org/api/v1/topics/physical.chemistry" }, { "id": "physical.chemistry.methods", "label": "Chemical principles and methods", "api_url": "https://www.edgepedia.org/api/v1/topics/physical.chemistry.methods" }, { "id": "physical.chemistry.methods.chemical-reaction-science", "label": "Reaction rates, mechanisms, and engineering", "api_url": "https://www.edgepedia.org/api/v1/topics/physical.chemistry.methods.chemical-reaction-science" }, { "id": "physical.chemistry.methods.reaction-mechanisms-and-named-reactions", "label": "Reaction mechanisms and named reactions", "api_url": "https://www.edgepedia.org/api/v1/topics/physical.chemistry.methods.reaction-mechanisms-and-named-reactions" } ], "geo": [ { "id": "geo.nongeo.t1800.physical.chemistry.methods", "label": "Non-geographic · 1800 to 1945: Chemical principles and methods", "api_url": "https://www.edgepedia.org/api/v1/geo/geo.nongeo.t1800.physical.chemistry.methods", "path": [ { "id": "geo.nongeo", "label": "Non-geographic", "api_url": "https://www.edgepedia.org/api/v1/geo/geo.nongeo" }, { "id": "geo.nongeo.t1800", "label": "Non-geographic · 1800 to 1945", "api_url": "https://www.edgepedia.org/api/v1/geo/geo.nongeo.t1800" }, { "id": "geo.nongeo.t1800.physical", "label": "Physical world and mathematics", "api_url": "https://www.edgepedia.org/api/v1/geo/geo.nongeo.t1800.physical" }, { "id": "geo.nongeo.t1800.physical.chemistry", "label": "Chemistry", "api_url": "https://www.edgepedia.org/api/v1/geo/geo.nongeo.t1800.physical.chemistry" }, { "id": "geo.nongeo.t1800.physical.chemistry.methods", "label": "Chemical principles and methods", "api_url": "https://www.edgepedia.org/api/v1/geo/geo.nongeo.t1800.physical.chemistry.methods" } ] } ], "excerpt": "The water-gas shift reaction (WGS) is an industrial catalytic reaction converting carbon monoxide and steam into carbon dioxide and hydrogen, first applied industrially in 1915 for ammonia synthesis.", "snippet": "The water-gas shift reaction (WGS) is an industrial catalytic reaction converting carbon monoxide and steam into carbon dioxide and hydrogen, first applied industrially in 1915 for ammonia synthesis.", "node": "physical.chemistry.methods.reaction-mechanisms-and-named-reactions", "markdown": "# Water-gas shift reaction\n\nThe water-gas shift reaction (WGS) is an industrial catalytic reaction that converts carbon monoxide and steam into carbon dioxide and hydrogen, written CO + H₂O ⇌ CO₂ + H₂, and it is important for industrial purification of H₂ streams.[1](https://journal.hep.com.cn/fcse/EN/10.1007/s11705-025-2547-0) • [2](https://www.fung-group.org/assets/pdf/polo2019elucidation.pdf) The reaction is moderately exothermic and reversible, with a standard reaction enthalpy of −41.1 kJ·mol⁻¹ (some compilations give −40.6 kJ/mol).[1](https://journal.hep.com.cn/fcse/EN/10.1007/s11705-025-2547-0) • [3](https://www.sciencedirect.com/science/article/abs/pii/S1226086X16304907) • [4](https://www.sciencedirect.com/science/article/abs/pii/S0021951707002667) Because the number of gas molecules does not change, pressure has only a second-order effect on equilibrium.[3](https://www.sciencedirect.com/science/article/abs/pii/S1226086X16304907) Approximately 76% of global hydrogen (and 95% of US hydrogen) is produced by steam methane reforming of natural gas, with coal gasification accounting for about 22% globally and electrolysis about 2%; WGS is used to convert the CO in these streams.[5](https://pmc.ncbi.nlm.nih.gov/articles/PMC9679995/)\n\n| Key fact | Detail |\n|---|---|\n| Reaction | CO + H₂O ⇌ CO₂ + H₂, ΔH°₂₉₈ = −41.1 kJ·mol⁻¹[1](https://journal.hep.com.cn/fcse/EN/10.1007/s11705-025-2547-0) |\n| Industrial arrangement | Two adiabatic stages: HTS at 350–450 °C over Fe–Cr, then LTS at 190–250 °C over Cu–Zn–Al[2](https://www.fung-group.org/assets/pdf/polo2019elucidation.pdf) |\n| Residual CO | 3–5% after HTS, about 0.3% after LTS[1](https://journal.hep.com.cn/fcse/EN/10.1007/s11705-025-2547-0) • [4](https://www.sciencedirect.com/science/article/abs/pii/S0021951707002667) |\n| Operating pressure | Typically 1.0–6.0 MPa[6](https://www.nature.com/articles/s41467-018-07937-w) |\n| Steam/CO ratio | Optimal 3–4 for high-temperature shift; ≥3 also minimizes the negative effect of feed CO₂[7](https://pubs.aip.org/aip/acp/article/3215/1/070006/3322074/High-temperature-water-gas-shift-Thermodynamic-and) • [8](https://onlinelibrary.wiley.com/doi/10.1002/er.5861) |\n| Main catalyst families | Fe–Cr (magnetite active phase), Cu–Zn–Al, noble metals on reducible oxides, sulfided Co–Mo for sour gas[5](https://pmc.ncbi.nlm.nih.gov/articles/PMC9679995/) • [9](https://www.mdpi.com/2073-4344/9/9/772) |\n| Thermodynamic limit | The standard reaction Gibbs free energy becomes positive around 1100 K, so equilibrium conversion falls as temperature rises[1](https://journal.hep.com.cn/fcse/EN/10.1007/s11705-025-2547-0) |\n\n## How it works\n\nThe exothermic equilibrium favors conversion at low temperature: equilibrium conversion decreases as reaction temperature rises, and the standard reaction [Gibbs free energy](https://www.edgepedia.org/gibbs-free-energy) becomes positive around 1100 K (the actual reaction Gibbs energy also depends on composition and is zero at equilibrium).[1](https://journal.hep.com.cn/fcse/EN/10.1007/s11705-025-2547-0) • [7](https://pubs.aip.org/aip/acp/article/3215/1/070006/3322074/High-temperature-water-gas-shift-Thermodynamic-and) Raising the molar steam-to-CO ratio increases equilibrium CO conversion, especially above 423 K, which is why plants run steam in excess.[1](https://journal.hep.com.cn/fcse/EN/10.1007/s11705-025-2547-0)\n\nTwo mechanistic families describe the reaction. In the regenerative (redox) mechanism, CO is oxidized by surface oxygen to CO₂ and the reduced site is reoxidized by water to release H₂; on the industrial magnetite catalyst this proceeds through the Fe³⁺/Fe²⁺ couple, with Fe²⁺ oxidized to Fe³⁺ by H₂O and reduced back by CO.[5](https://pmc.ncbi.nlm.nih.gov/articles/PMC9679995/) The redox route is generally regarded as kinetically relevant above 350 °C over the industrial Fe–Cr catalyst.[10](https://chem.libretexts.org/Courses/Centre_College/CHE_332%3A_Inorganic_Chemistry/11%3A_Organometallic_Reactions_and_Catalysis/11.04%3A_Heterogeneous_Catalysts/11.4.02%3A_Water-Gas_Shift_Reaction) In the associative mechanism, adsorbed CO and water form intermediates such as formate (HCOO), carboxyl (COOH), or bicarbonate before H₂ and CO₂ desorb.[1](https://journal.hep.com.cn/fcse/EN/10.1007/s11705-025-2547-0) • [10](https://chem.libretexts.org/Courses/Centre_College/CHE_332%3A_Inorganic_Chemistry/11%3A_Organometallic_Reactions_and_Catalysis/11.04%3A_Heterogeneous_Catalysts/11.4.02%3A_Water-Gas_Shift_Reaction) For the iron-chromium system, both a regenerative mechanism through adsorbed oxygen atoms and mechanisms through a C–H–O intermediate such as the formate ion were proposed in the classic 1980 review literature.[11](https://www.osti.gov/servlets/purl/6384399)\n\nModern experiments and calculations assign the route catalyst by catalyst. On an industrial-type CuCrFeOₓ catalyst, density functional theory found the redox route energetically favored: the slow step, CO* oxidation by Fe₃O₄ lattice oxygen, has a barrier of 0.39 eV versus 0.73 eV for HO–CO* coupling in the associative route; isotope-scrambling (SSITKA) experiments showed extensive ¹⁸O/¹⁶O exchange characteristic of a redox mechanism, with surface formate present only transiently.[2](https://www.fung-group.org/assets/pdf/polo2019elucidation.pdf) CO adsorbs most strongly at the Cu–Fe interface (−1.60 eV), making the Cu–Fe₃O₄ interface the active site.[2](https://www.fung-group.org/assets/pdf/polo2019elucidation.pdf) On noble-metal catalysts the route depends on the support: Pt/CeO₂ follows the associative formate route, Pt/ZrO₂ the formate route with redox regeneration, and Pt/TiO₂ both routes at 300 °C.[4](https://www.sciencedirect.com/science/article/abs/pii/S0021951707002667) Theoretical work on Cu(111) showed COOH plays the central role while formates are stable bystanders formed by CO₂ hydrogenation.[1](https://journal.hep.com.cn/fcse/EN/10.1007/s11705-025-2547-0)\n\n## How it is done\n\nIndustrial plants operate at 1.0–6.0 MPa and use a two-step reactor train.[6](https://www.nature.com/articles/s41467-018-07937-w) The feed first passes through a high-temperature shift (HTS) bed at 350–450 °C over an iron-oxide-based catalyst, where reaction rate is high and the bulk of the CO is converted; outlet CO is 3–5%.[2](https://www.fung-group.org/assets/pdf/polo2019elucidation.pdf) • [1](https://journal.hep.com.cn/fcse/EN/10.1007/s11705-025-2547-0) A second, low-temperature shift (LTS) bed at 190–250 °C over a copper-zinc-oxide-based catalyst exploits the favorable low-temperature equilibrium to push residual CO down to about 0.3% (0.1–0.3% in copper-based formulations).[2](https://www.fung-group.org/assets/pdf/polo2019elucidation.pdf) • [1](https://journal.hep.com.cn/fcse/EN/10.1007/s11705-025-2547-0) • [3](https://www.sciencedirect.com/science/article/abs/pii/S1226086X16304907) • [4](https://www.sciencedirect.com/science/article/abs/pii/S0021951707002667)\n\nThe HTS catalyst is hematite-based, typically 74.2% Fe₂O₃ and 10.0% Cr₂O₃ in a classic composition, and is activated by partial reduction to magnetite (Fe₃O₄), the active phase.[3](https://www.sciencedirect.com/science/article/abs/pii/S1226086X16304907) • [5](https://pmc.ncbi.nlm.nih.gov/articles/PMC9679995/) Chromium oxide is a textural promoter that increases the Fe₃O₄ surface area and reduces sintering, while copper is a chemical promoter that lowers activation barriers and raises turnover frequencies.[2](https://www.fung-group.org/assets/pdf/polo2019elucidation.pdf) Chromium also limits Fe²⁺ formation and improves thermal stability.[5](https://pmc.ncbi.nlm.nih.gov/articles/PMC9679995/) For bio-syngas, the highest CO conversion and H₂ yield occur at 400 °C with a steam/CO ratio of 3 or higher.[8](https://onlinelibrary.wiley.com/doi/10.1002/er.5861)\n\n## Origin\n\nThe reaction was used to enrich hydrogen for fuel-cell applications.[1](https://journal.hep.com.cn/fcse/EN/10.1007/s11705-025-2547-0) The industrial catalytic process (U.S. Patent 1115776 A),[2](https://www.fung-group.org/assets/pdf/polo2019elucidation.pdf) • [12](https://pubs.rsc.org/en/content/articlehtml/2025/ta/d5ta02030a) and the reaction was first applied on an industrial scale in 1915 in the Haber-Bosch ammonia synthesis process in Germany, where it removed CO from the hydrogen stream.[1](https://journal.hep.com.cn/fcse/EN/10.1007/s11705-025-2547-0) • [2](https://www.fung-group.org/assets/pdf/polo2019elucidation.pdf) A much later milestone was the world's first industrialization of lean steam/gas sour shift (SWGS) in China in 2003, with plants running over 10 years and average catalyst lifetimes of 3–4 years.[9](https://www.mdpi.com/2073-4344/9/9/772)\n\n## Variants\n\n**Sour shift.** Sulfur-tolerant Mo–Co/alkali/Al₂O₃ catalysts operate steadily at steam/gas ratios as low as 0.2–0.3 on sulfur-containing syngas; adding K₂O to MgAl₂O₄-spinel-modified supported CoMoOₓ raises CO conversion and suppresses methane formation.[9](https://www.mdpi.com/2073-4344/9/9/772)\n\n**Single-stage fuel-cell catalysts.** Pt-based bifunctional catalysts, with platinum activating CO and a hydrophilic reducible oxide support activating water, enable single-stage WGS for fuel-cell applications.[4](https://www.sciencedirect.com/science/article/abs/pii/S0021951707002667) Related materials reach high activity at low temperature: atomic Pt substituted into Mn₃O₄ gives almost full CO conversion at 260 °C with zero methane formation, and mesoporous ceria supports show full CO conversion at 175 °C.[13](https://link.springer.com/article/10.1007/s42247-020-00116-y)\n\n**Sorption- and membrane-enhanced reactors.** Sorption-enhanced WGS over Cu-CeO₂/HTlc at 125–295 °C gave a 70% volume enrichment in hydrogen by in-situ CO₂ removal.[13](https://link.springer.com/article/10.1007/s42247-020-00116-y) For IGCC syngas containing several thousand ppm H₂S, a membrane reactor combining [carbon molecular sieve](https://www.edgepedia.org/carbon-molecular-sieve) (CMS) membranes with sulfided Co/Mo sour-shift catalyst achieved higher CO conversion than a packed bed at up to 300 °C and 25 bar; this \"one-box\" process replaces the dual-bed HTS/LTS train, avoids syngas pre-treatment and a separate H₂ purification step, and delivers CO₂ at high pressure for capture.[14](https://www.osti.gov/pages/servlets/purl/2329372) Field-scale MR-AR testing on real syngas reached TRL 5, with CMS membranes meeting targets of H₂ permeance above 1 m³/(m²·h·bar) and H₂/CO selectivity above 80 at up to 300 °C and 25 bar with under 10% decline over 250 h.[15](https://pmc.ncbi.nlm.nih.gov/articles/PMC10890546/)\n\n**Electrochemical WGS.** An electrochemical route produces hydrogen of over 99.99% purity with about 100% faradaic efficiency at room temperature (25 °C) and atmospheric pressure, with only 27 ppm residual CO.[6](https://www.nature.com/articles/s41467-018-07937-w)\n\n## Applications\n\nWGS was initially used to remove CO from the hydrogen stream for Haber-Bosch ammonia synthesis, and later to tune the H₂/CO ratio of syngas for hydrogen production, methanol synthesis, and Fischer-Tropsch synthesis.[2](https://www.fung-group.org/assets/pdf/polo2019elucidation.pdf) It is used in the manufacture of ammonia, hydrocarbons, methanol, and hydrogen.[10](https://chem.libretexts.org/Courses/Centre_College/CHE_332%3A_Inorganic_Chemistry/11%3A_Organometallic_Reactions_and_Catalysis/11.04%3A_Heterogeneous_Catalysts/11.4.02%3A_Water-Gas_Shift_Reaction) The hydrogen it purifies comes mostly from natural gas steam reforming (48% of demand), heavy oil and naphtha reforming (30%), coal gasification (18%), water electrolysis (3.9%), and biomass and other resources (0.1%).[3](https://www.sciencedirect.com/science/article/abs/pii/S1226086X16304907) Fuel-cell hydrogen is a growing target, where an ideal low-temperature catalyst must be cost-effective, CO-tolerant, and thermally stable below 250 °C.[13](https://link.springer.com/article/10.1007/s42247-020-00116-y)\n\n## Limitations and alternatives\n\n**Poisoning and sintering.** Copper-based LTS catalysts are prone to sulfur poisoning and require guard beds, while iron-based catalysts are more sulfur-tolerant.[3](https://www.sciencedirect.com/science/article/abs/pii/S1226086X16304907) The CuO/ZnO/Al₂O₃ LTS catalyst is susceptible to thermal sintering and its conversion frequency is not high enough.[1](https://journal.hep.com.cn/fcse/EN/10.1007/s11705-025-2547-0) In sour-shift service, sintering causes the most severe deactivation by irreversibly reducing surface area and active sites, and As or Cl poisoning disturbs catalyst sulfurization.[9](https://www.mdpi.com/2073-4344/9/9/772) Noble-metal low-temperature catalysts suffer irreversible over-reduction of the reducible support in high-H₂ feed gas, causing rapid deactivation.[1](https://journal.hep.com.cn/fcse/EN/10.1007/s11705-025-2547-0)\n\n**Membrane alternatives.** Dense Pd membranes offer nearly infinite H₂ selectivity but are poisoned by H₂S even at low concentrations, and amorphous silica membranes are hydrothermally unstable, motivating CMS membranes.[14](https://www.osti.gov/pages/servlets/purl/2329372) Pd-based membrane reactors use self-supporting foils 25–100 μm thick that are expensive with low hydrogen flux.[3](https://www.sciencedirect.com/science/article/abs/pii/S1226086X16304907)\n\n## References\n\n1. [A review on the low temperature water-gas-shift reaction: reaction mechanism, catalyst design, and novel process development (Frontiers of Chemical Science and Engineering, 2025)](https://journal.hep.com.cn/fcse/EN/10.1007/s11705-025-2547-0)\n2. [Elucidation of the Reaction Mechanism for High-Temperature Water Gas Shift over an Industrial-Type Copper–Chromium–Iron Oxide Catalyst (Polo et al., ACS Catalysis 2019)](https://www.fung-group.org/assets/pdf/polo2019elucidation.pdf)\n3. [Hydrogen production: Perspectives, separation with special emphasis on kinetics of WGS reaction: A state-of-the-art review (Journal of Industrial and Engineering Chemistry)](https://www.sciencedirect.com/science/article/abs/pii/S1226086X16304907)\n4. [Bifunctional catalysts for single-stage water–gas shift reaction in fuel cell applications. Part 1: Effect of the support on the reaction sequence (Journal of Catalysis, 2007)](https://www.sciencedirect.com/science/article/abs/pii/S0021951707002667)\n5. [Substituting Chromium in Iron-Based Catalysts for the High-Temperature Water–Gas Shift Reaction (ACS Catalysis, 2022)](https://pmc.ncbi.nlm.nih.gov/articles/PMC9679995/)\n6. [Room-temperature electrochemical water–gas shift reaction for high purity hydrogen production | Nature Communications](https://www.nature.com/articles/s41467-018-07937-w)\n7. [High-temperature water gas shift: Thermodynamic and reactor modeling study (AIP Conf. Proc., Nov 2024)](https://pubs.aip.org/aip/acp/article/3215/1/070006/3322074/High-temperature-water-gas-shift-Thermodynamic-and)\n8. [Effects of bio-syngas CO2 concentration on water-gas shift and side reactions with Fe-Cr based catalyst (International Journal of Energy Research)](https://onlinelibrary.wiley.com/doi/10.1002/er.5861)\n9. [Recent Advances in Industrial Sulfur Tolerant Water Gas Shift Catalysts for Syngas Hydrogen Enrichment: Application of Lean (Low) Steam/Gas Ratio (Catalysts/MDPI)](https://www.mdpi.com/2073-4344/9/9/772)\n10. [Section 11.4.2: Water-Gas Shift Reaction - Chemistry LibreTexts (Kathryn Haas, Duke University)](https://chem.libretexts.org/Courses/Centre_College/CHE_332%3A_Inorganic_Chemistry/11%3A_Organometallic_Reactions_and_Catalysis/11.04%3A_Heterogeneous_Catalysts/11.4.02%3A_Water-Gas_Shift_Reaction)\n11. [The Water-Gas Shift Reaction (Newsome, Catal. Rev.: Sci. Eng. 1980, via OSTI)](https://www.osti.gov/servlets/purl/6384399)\n12. [Reasonable active site design for promoting water dissociation and carbon monoxide activation in a low-temperature water-gas shift reaction (J. Mater. Chem. A, 2025, 13, 30755)](https://pubs.rsc.org/en/content/articlehtml/2025/ta/d5ta02030a)\n13. [A review of recent advances in water-gas shift catalysis for hydrogen production (Emergent Materials, 2020)](https://link.springer.com/article/10.1007/s42247-020-00116-y)\n14. [Water gas shift membrane reactor study with sour-shift catalyst and CMS membranes for IGCC (Garshasbi et al., USC/UCLA/M&PT)](https://www.osti.gov/pages/servlets/purl/2329372)\n15. [Field-Scale Testing of a High-Efficiency Membrane Reactor (MR), Adsorptive Reactor (AR) Process for H2 Generation and Pre-Combustion CO2 Capture](https://pmc.ncbi.nlm.nih.gov/articles/PMC10890546/)\n\n---\n*Topic: Encyclopedia › Physical world and mathematics › Chemistry › Chemical principles and methods › Reaction rates, mechanisms, and engineering › Reaction mechanisms and named reactions*\n\n*Initially written Sep 29, 2026 · Edited: Oct 15, 2026; Oct 21, 2026*\n\n*Copyright 2026 EdgeChat AI, a subsidiary of Biostate AI.*\n\nLicense: Edgepedia Community License 1.0, https://www.edgepedia.org/edgepedia/license\n", "same_as": [], "url": "https://www.edgepedia.org/water-gas-shift-reaction", "markdown_url": "https://www.edgepedia.org/water-gas-shift-reaction.md", "license": { "name": "Edgepedia Community License 1.0", "url": "https://www.edgepedia.org/edgepedia/license", "summary": "Free with credit, commercial use included. AI training is open to everyone. For other uses, organizations over USD 100M in revenue or 100M monthly users license separately.", "spdx": "LicenseRef-Edgepedia-Community-1.0" }, "credit": "\"Water-gas shift reaction\", Edgepedia (EdgeChat), https://www.edgepedia.org/water-gas-shift-reaction. Edgepedia Community License 1.0.", "credit_md": "\"[Water-gas shift reaction](https://www.edgepedia.org/water-gas-shift-reaction)\", Edgepedia (EdgeChat), [https://www.edgepedia.org/water-gas-shift-reaction](https://www.edgepedia.org/water-gas-shift-reaction). [Edgepedia Community License 1.0](https://www.edgepedia.org/edgepedia/license).", "credit_html": "\"Water-gas shift reaction\", Edgepedia (EdgeChat), https://www.edgepedia.org/water-gas-shift-reaction. Edgepedia Community License 1.0.", "speakable": "The water-gas shift reaction is an industrial catalytic reaction converting carbon monoxide and steam into carbon dioxide and hydrogen, first applied industrially in 1915 for ammonia synthesis." }