{ "id": "epf1pmyhp5", "slug": "urea-electrooxidation", "title": "Urea electrooxidation", "updated": "2026-10-25", "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.analytical-chemistry", "label": "Analytical chemistry", "api_url": "https://www.edgepedia.org/api/v1/topics/physical.chemistry.methods.analytical-chemistry" }, { "id": "physical.chemistry.methods.electroanalysis-and-electrochemistry", "label": "Electroanalysis and electrochemistry", "api_url": "https://www.edgepedia.org/api/v1/topics/physical.chemistry.methods.electroanalysis-and-electrochemistry" }, { "id": "physical.chemistry.methods.electroanalysis-and-electrochemistry.electrode-kinetics-and-electron-transfer", "label": "Electrode kinetics and electron transfer", "api_url": "https://www.edgepedia.org/api/v1/topics/physical.chemistry.methods.electroanalysis-and-electrochemistry.electrode-kinetics-and-electron-transfer" } ], "geo": [ { "id": "geo.nongeo.t1946.physical.chemistry.methods.electroanalysis-and-electrochemistry", "label": "Non-geographic · 1946 to 2000: Electroanalysis and electrochemistry", "api_url": "https://www.edgepedia.org/api/v1/geo/geo.nongeo.t1946.physical.chemistry.methods.electroanalysis-and-electrochemistry", "path": [ { "id": "geo.nongeo", "label": "Non-geographic", "api_url": "https://www.edgepedia.org/api/v1/geo/geo.nongeo" }, { "id": "geo.nongeo.t1946", "label": "Non-geographic · 1946 to 2000", "api_url": "https://www.edgepedia.org/api/v1/geo/geo.nongeo.t1946" }, { "id": "geo.nongeo.t1946.physical", "label": "Physical world and mathematics", "api_url": "https://www.edgepedia.org/api/v1/geo/geo.nongeo.t1946.physical" }, { "id": "geo.nongeo.t1946.physical.chemistry", "label": "Chemistry", "api_url": "https://www.edgepedia.org/api/v1/geo/geo.nongeo.t1946.physical.chemistry" }, { "id": "geo.nongeo.t1946.physical.chemistry.methods", "label": "Chemical principles and methods", "api_url": "https://www.edgepedia.org/api/v1/geo/geo.nongeo.t1946.physical.chemistry.methods" }, { "id": "geo.nongeo.t1946.physical.chemistry.methods.analytical-chemistry", "label": "Analytical chemistry", "api_url": "https://www.edgepedia.org/api/v1/geo/geo.nongeo.t1946.physical.chemistry.methods.analytical-chemistry" }, { "id": "geo.nongeo.t1946.physical.chemistry.methods.electroanalysis-and-electrochemistry", "label": "Electroanalysis and electrochemistry", "api_url": "https://www.edgepedia.org/api/v1/geo/geo.nongeo.t1946.physical.chemistry.methods.electroanalysis-and-electrochemistry" } ] }, { "id": "geo.nongeo.t2001.physical.chemistry.methods.analytical-chemistry", "label": "Non-geographic · 2001 to 2020: Analytical chemistry", "api_url": "https://www.edgepedia.org/api/v1/geo/geo.nongeo.t2001.physical.chemistry.methods.analytical-chemistry", "path": [ { "id": "geo.nongeo", "label": "Non-geographic", "api_url": "https://www.edgepedia.org/api/v1/geo/geo.nongeo" }, { "id": "geo.nongeo.t2001", "label": "Non-geographic · 2001 to 2020", "api_url": "https://www.edgepedia.org/api/v1/geo/geo.nongeo.t2001" }, { "id": "geo.nongeo.t2001.physical", "label": "Physical world and mathematics", "api_url": "https://www.edgepedia.org/api/v1/geo/geo.nongeo.t2001.physical" }, { "id": "geo.nongeo.t2001.physical.chemistry", "label": "Chemistry", "api_url": "https://www.edgepedia.org/api/v1/geo/geo.nongeo.t2001.physical.chemistry" }, { "id": "geo.nongeo.t2001.physical.chemistry.methods", "label": "Chemical principles and methods", "api_url": "https://www.edgepedia.org/api/v1/geo/geo.nongeo.t2001.physical.chemistry.methods" }, { "id": "geo.nongeo.t2001.physical.chemistry.methods.analytical-chemistry", "label": "Analytical chemistry", "api_url": "https://www.edgepedia.org/api/v1/geo/geo.nongeo.t2001.physical.chemistry.methods.analytical-chemistry" } ] } ], "excerpt": "Urea electrooxidation is the electrochemical oxidation of urea at an anode, a six-electron reaction used to produce hydrogen with about 30% less energy than water electrolysis.", "snippet": "Urea electrooxidation is the electrochemical oxidation of urea at an anode, a six-electron reaction used to produce hydrogen with about 30% less energy than water electrolysis.", "node": "physical.chemistry.methods.electroanalysis-and-electrochemistry.electrode-kinetics-and-electron-transfer", "markdown": "# Urea electrooxidation\n\nUrea electrooxidation is the electrochemical oxidation of urea at an anode surface, a six-electron reaction studied as a low-voltage alternative to water oxidation for hydrogen production, as the anode reaction of direct urea fuel cells, and as a route to remove urea from urine and wastewater. In alkaline solution the overall anode reaction is CO(NH2)2 + 6OH− → N2 + 5H2O + CO2 + 6e−, and coupled with hydrogen evolution at the cathode the theoretical cell potential is 0.37 V, against 1.23 V for water electrolysis.[1](https://doi.org/10.1039/b905974a) • [2](https://pmc.ncbi.nlm.nih.gov/articles/PMC9457967/) The reaction matters because it can reduce the energy consumption of hydrogen production while treating nitrogen-containing wastewater.[3](https://pubs.rsc.org/en/content/articlelanding/2026/cc/d6cc01805j)\n\n| Key fact | Value |\n|---|---|\n| Anode half-reaction (alkaline) | CO(NH2)2 + 6OH− → N2 + 5H2O + CO2 + 6e−[4](https://www.sciencedirect.com/science/article/abs/pii/S0013468613012437) |\n| Theoretical cell potential (UOR‖HER) | 0.37 V vs 1.23 V for water electrolysis[1](https://doi.org/10.1039/b905974a) |\n| Ni(OH)2/NiOOH redox potential | 0.49 V vs SHE; sets the operating potential[2](https://pmc.ncbi.nlm.nih.gov/articles/PMC9457967/) |\n| Practical anode potential on Ni catalysts | ≥1.3–1.4 V vs RHE for measurable currents[5](https://www.jceem.com/article_235952.html) |\n| Measured energy saving vs water electrolysis | 10–30% reduction in energy consumption[6](https://iopscience.iop.org/article/10.1149/1945-7111/acf87e) |\n| Typical electrolyte | 0.33 M urea (approximating human urine) in 0.5–5 M KOH[1](https://doi.org/10.1039/b905974a) • [7](https://hal.science/hal-03940269v1/file/Revised%20manuscript%20with%20changes%20highlighted%20in%20yellow%20background.pdf) |\n| Major N products on Ni(OH)2 | Nitrite and cyanate in ≈1:1 ratio; N2 minor[8](https://doi.org/10.1002/anie.202209839) |\n\n## How it works\n\nThe accepted pathway on nickel electrodes is a chemical regeneration (EC′) mechanism. Ni(OH)2 is electrochemically oxidized to NiOOH, NiOOH chemically oxidizes urea and is reduced back to Ni(OH)2, and the cycle repeats. [In situ](https://www.edgepedia.org/in-situ) surface-enhanced [Raman spectroscopy](https://www.edgepedia.org/raman-spectroscopy) confirmed this sequence and detected carbonate ions at 0.50 V vs Hg/HgO, showing CO2 is a product.[4](https://www.sciencedirect.com/science/article/abs/pii/S0013468613012437) Because Ni(OH)2 oxidizes to NiOOH at 0.49 V vs SHE, the applied potential is governed by the nickel redox couple rather than by the thermodynamic potential of urea itself.[2](https://pmc.ncbi.nlm.nih.gov/articles/PMC9457967/) Kinetic work confirmed that oxidation begins only after significant Ni3+ forms on the surface.[9](https://doi.org/10.1016/j.electacta.2012.07.007)\n\n[Density functional theory](https://www.edgepedia.org/density-functional-theory) found a bridge-coordinated urea adsorption structure to be energetically favorable, and identified desorption of the *COO intermediate (yielding CO32−) as the rate-determining step, with a computed cost of 1242.2 kJ/mol.[2](https://pmc.ncbi.nlm.nih.gov/articles/PMC9457967/) • [10](https://www.cell.com/chem-catalysis/pdf/S2667-1093%2823%2900428-1.pdf) Three urea dissociation pathways are distinguished: intramolecular N–N coupling to N2 at Ni3+ sites, C–N cleavage leading to nitrite, and intermolecular N–N coupling via an ammonia intermediate.[10](https://www.cell.com/chem-catalysis/pdf/S2667-1093%2823%2900428-1.pdf) Competing descriptions invoke direct oxidation on high-valence Ni4+ species and a lattice-oxygen-involved pathway.[3](https://pubs.rsc.org/en/content/articlelanding/2026/cc/d6cc01805j) • [11](https://doi.org/10.1002/anie.201909832)\n\nEarly work reported anode gas of 96.1% N2,[1](https://doi.org/10.1039/b905974a) but quantitative product analyses later showed that on Ni(OH)2-based anodes urea oxidation predominantly yields a ≈1:1 mixture of nitrite and cyanate, with N2 a minor product,[8](https://doi.org/10.1002/anie.202209839) and that nitrite can form with over 80% faradaic efficiency on NiOOH.[12](https://chemistry-europe.onlinelibrary.wiley.com/doi/10.1002/cplu.202300739) Reactor modeling with complete mass balances found most products remain in the liquid phase, with gas not exceeding 12% of the urea converted.[7](https://hal.science/hal-03940269v1/file/Revised%20manuscript%20with%20changes%20highlighted%20in%20yellow%20background.pdf) • [6](https://iopscience.iop.org/article/10.1149/1945-7111/acf87e)\n\n## How it is done\n\nThe reference working electrode is the nickel oxyhydroxide modified nickel (NOMN) electrode: a Ni foil, Ni gauze, Ti foil, or Ti gauze substrate electroplated with 10 ± 0.1 mg of Ni from a Watts bath, activated by polarity switching at 6.25 A/m2.[13](https://patents.google.com/patent/US20090095636) KOH outperforms LiOH and NaOH because K+ promotes C–O bond release and CO2 detachment, the rate-determining step.[14](https://www.mdpi.com/2073-4344/12/3/337) Urea concentrations of 0.33 M approximate human urine; 5 M KOH was used in the original demonstration, where nickel outperformed Pt, Pt–Ir, and Rh with a current density near 100 mA cm−2.[1](https://doi.org/10.1039/b905974a) • [15](https://chemistry-europe.onlinelibrary.wiley.com/doi/full/10.1002/celc.202300637)\n\nEvaluation relies on cyclic voltammetry, linear sweep voltammetry, and rotating disk voltammetry.[9](https://doi.org/10.1016/j.electacta.2012.07.007) Tafel analysis on nickel in alkaline medium gave reaction orders of 0.3 in urea and 2 in OH−, with a urea diffusion coefficient of 0.85 × 10−5 cm2 s−1.[9](https://doi.org/10.1016/j.electacta.2012.07.007)\n\n## Origin\n\n[Anodic oxidation](https://www.edgepedia.org/anodic-oxidation) of urea was reported in 1973 by S. J. Yao, S. K. Wolfson, B. K. Ahn, and C. C. Liu in Nature as an electrochemical approach to de-ureation in the dialysis context.[16](https://doi.org/10.1038/241471a0) The modern field began when Bryan K. Boggs, Rebecca L. King, and Gerardine G. Botte reported direct conversion of urine and urea to pure hydrogen with a nickel catalyst in Chemical Communications in 2009,[1](https://doi.org/10.1039/b905974a) using a Hoffmann apparatus to extract H2 and N2 at 1.5 V.[2](https://pmc.ncbi.nlm.nih.gov/articles/PMC9457967/) A US provisional patent was filed on the electrolytic production of ammonia and hydrogen from urea and urine.[13](https://patents.google.com/patent/US20090095636) Follow-up work by the same group established the mechanism: a DFT analysis of urea dissociation on NiOOH by Damilola A. Daramola, [Deepika Singh](https://www.edgepedia.org/deepika-singh), and Gerardine G. Botte (2010),[17](https://doi.org/10.1021/jp105159t) and the experimental mechanism study of Vedasri Vedharathinam and Gerardine G. Botte (2012).[9](https://doi.org/10.1016/j.electacta.2012.07.007) Later milestones include the intramolecular N–N coupling pathway ([Wei Chen](https://www.edgepedia.org/wei-chen) and colleagues, 2020),[18](https://doi.org/10.1002/anie.202015773) nickel ferrocyanide as a high-performance catalyst (Shi-Kui Geng and colleagues, 2021),[19](https://doi.org/10.1038/s41560-021-00899-2) and the quantitative nitrite-and-cyanate product analysis (Stephen W. Tatarchuk, Jury J. Medvedev, Feng Li, Yulia Tobolovskaya, and Anna Klinkova, 2022).[8](https://doi.org/10.1002/anie.202209839)\n\n## Variants\n\nNickel-based materials are favored because of low cost, high activity, and high stability.[20](https://link.springer.com/article/10.1007/s11581-023-05107-7) Among Ni(OH)2 polymorphs, α-Ni(OH)2 outperforms β-Ni(OH)2 with higher current response (3.0 vs 1.6 mA cmECSA−2), lower Tafel slope (89 vs 121 mV dec−1), and higher apparent rate constant (6.13 × 103 vs 1.58 × 103 mol−1 s−1).[2](https://pmc.ncbi.nlm.nih.gov/articles/PMC9457967/) Nickel ferrocyanide (Ni2Fe(CN)6) operates by a two-step mechanism: urea decomposes to NH3 at the Ni2+ site, then NH3 is electrochemically oxidized to N2 at the Fe site.[10](https://www.cell.com/chem-catalysis/pdf/S2667-1093%2823%2900428-1.pdf)\n\nAtomic-scale design now targets selectivity directly. Oxyanion-engineered Ni-SOX catalysts reach 323.4 mA cm−2 at 1.65 V in 1 M KOH + 0.33 M urea with 99.3 ± 0.4% N-product selectivity, versus 82.6 ± 0.7% for the unmodified NiOX.[21](https://doi.org/10.1038/s41467-023-41588-w) Asymmetric Ni–O–Ti sites on Ti foam achieve 99% N2 selectivity, against below 55% for documented symmetric Ni–O–Ni catalysts and 10–30% for Ni foam, with stability over 10,000 cycles and 10 days.[22](https://doi.org/10.1038/s41467-024-50343-8) A Cl-mediated mechanism on Pt uses adsorbed chloride to form N-chlorourea intermediates that convert to N2 via intermolecular N–N coupling, confirmed by isotope labeling showing only 14N15N and 14N14N signals; Pt sustained over 200 h of operation while Ni(OH)2 and RuO2 decayed within 2 h under chloride conditions.[23](https://www.nature.com/articles/s41467-025-57798-3)\n\n## Applications\n\n**Hydrogen production.** [Urea electrolysis](https://www.edgepedia.org/urea-electrolysis) at 1.4 V cell potential delivered pure hydrogen at the cathode while water electrolysis does not proceed appreciably there, and required 30% less energy than water electrolysis at the same current.[1](https://doi.org/10.1039/b905974a) • [6](https://iopscience.iop.org/article/10.1149/1945-7111/acf87e) In practical electrolyzers, Pt-catalyzed acidic Cl-mediated urine electrolysis consumes 4.05 kWh Nm−3 H2 at 300 mA cm−2, versus 5.62 kWh Nm−3 for Ni-based urea electrolysis and 4.70–5.00 kWh Nm−3 for water electrolysis.[23](https://www.nature.com/articles/s41467-025-57798-3)\n\n**Direct urea fuel cells.** Raising KOH concentration from 0.1 M to 4 M shifts the urea oxidation onset from +0.36 V to +0.25 V vs Ag/AgCl, and 5 M KOH raised open-circuit voltage from 0.4 to 0.55 V and maximum power density from 1.7 to 11.2 mW cm−2.[15](https://chemistry-europe.onlinelibrary.wiley.com/doi/full/10.1002/celc.202300637)\n\n**Wastewater treatment.** An AEM electrolyzer with NiO/Co3O4 anodes and NiCoP cathodes treated urea wastewater at 600 mA cm−2 initial current density with about 53% average urea treatment efficiency and roughly 3.5-fold higher H2 yield than overall water splitting, at 1.94 V, 220 mV below overall water splitting.[24](https://link.springer.com/article/10.1007/s40820-024-01585-0) A solar-powered reactor using real urine produced 75.7 mL h−1 H2 and 25.2 mL h−1 N2 with 9.6% solar-to-H2 efficiency and 96% total nitrogen removal after 6 h.[22](https://doi.org/10.1038/s41467-024-50343-8)\n\n## Limitations and alternatives\n\n**Failure modes.** The CO or CO* intermediate binds strongly to nickel-based catalysts and blocks active sites, causing poisoning; cyclic voltammetry and polarity switching can recover activity.[14](https://www.mdpi.com/2073-4344/12/3/337) CO2 generated at the anode reacts with OH− to form carbonate and bicarbonate, which can precipitate with metal cations and foul electrodes or separators, especially at high current densities and elevated temperatures.[5](https://www.jceem.com/article_235952.html) Real urine adds chloride, phosphate, ammonium, creatinine, and other contaminants that affect conductivity, catalysis, and corrosion, and performance in urine is typically inferior to pure urea solution.[5](https://www.jceem.com/article_235952.html) At high current densities [UOR](https://www.edgepedia.org/urea-oxidation-reaction) competes strongly with the oxygen evolution reaction, lowering faradaic efficiency and accelerating passivation and dissolution of metal centers.[3](https://pubs.rsc.org/en/content/articlelanding/2026/cc/d6cc01805j)\n\n**The overpotential gap.** Although the theoretical cell potential is 0.37 V, measurable currents on conventional Ni-based catalysts require ≥1.3–1.4 V vs RHE, and industrial hydrogen production needs cell voltages of 1.35–1.6 V, giving a 10–30% reduction in electrical energy per kg H2 versus OER-based electrolyzers.[5](https://www.jceem.com/article_235952.html) A thermodynamic re-evaluation by Protsenko argued that the commonly quoted 0.37 V value arises from inconsistent stoichiometries and that the true open-circuit voltage of the relevant pathway is closer to 0.07 V; the 0.37 V figure remains the widely cited value.[5](https://www.jceem.com/article_235952.html) On the theoretical saving itself, published comparisons disagree: one review states up to ~94% less energy would be required than water splitting based on 0.07 V versus 1.23 V equilibrium potentials,[12](https://chemistry-europe.onlinelibrary.wiley.com/doi/10.1002/cplu.202300739) while measured demonstrations report about 30%.[6](https://iopscience.iop.org/article/10.1149/1945-7111/acf87e)\n\n## References\n\n1. [Bryan K. Boggs, Rebecca L. King, Gerardine G. Botte (2009). Urea electrolysis: direct hydrogen production from urine. Chemical Communications.](https://doi.org/10.1039/b905974a)\n2. [Recent Development of Nickel-Based Electrocatalysts for Urea Electrolysis in Alkaline Solution](https://pmc.ncbi.nlm.nih.gov/articles/PMC9457967/)\n3. [Revealing the reaction pathways and interfacial regulation mechanisms of urea electro-oxidation on nickel-based catalysts (Chem. Commun., 2026, review)](https://pubs.rsc.org/en/content/articlelanding/2026/cc/d6cc01805j)\n4. [Direct evidence of the mechanism for the electro-oxidation of urea on Ni(OH)2 catalyst in alkaline medium (in situ surface-enhanced Raman study, Electrochimica Acta)](https://www.sciencedirect.com/science/article/abs/pii/S0013468613012437)\n5. [Urea Oxidation Reaction as an Alternative Anodic Pathway for Energy-Efficient Hydrogen Generation (review)](https://www.jceem.com/article_235952.html)\n6. [New Insights into Urea Electro-Oxidation: Complete Mass-Balances and Proof of Concept with Real-Matrix Effluent (Hopsort et al., J. Electrochem. Soc. 170 093507, 2023)](https://iopscience.iop.org/article/10.1149/1945-7111/acf87e)\n7. [Indirect urea electrooxidation by nickel(III) in alkaline medium: kinetic, mechanism and reactor modeling (manuscript deposited on HAL)](https://hal.science/hal-03940269v1/file/Revised%20manuscript%20with%20changes%20highlighted%20in%20yellow%20background.pdf)\n8. [Stephen W. Tatarchuk and colleagues (2022). Nickel‐Catalyzed Urea Electrolysis: From Nitrite and Cyanate as Major Products to Nitrogen Evolution. Angewandte Chemie International Edition.](https://doi.org/10.1002/anie.202209839)\n9. [Vedasri Vedharathinam, Gerardine G. Botte (2012). Understanding the electro-catalytic oxidation mechanism of urea on nickel electrodes in alkaline medium. Electrochimica Acta.](https://doi.org/10.1016/j.electacta.2012.07.007)\n10. [Urea oxidation reaction electrocatalysts: Correlation of structure, activity, and selectivity (Chem Catalysis, 2023)](https://www.cell.com/chem-catalysis/pdf/S2667-1093%2823%2900428-1.pdf)\n11. [Longsheng Zhang and colleagues (2019). A Lattice‐Oxygen‐Involved Reaction Pathway to Boost Urea Oxidation. Angewandte Chemie International Edition.](https://doi.org/10.1002/anie.201909832)\n12. [Mechanistic Analysis of Urea Electrooxidation Pathways: Key to Rational Catalyst Design (ChemPlusChem, 2024)](https://chemistry-europe.onlinelibrary.wiley.com/doi/10.1002/cplu.202300739)\n13. [US20090095636A1 - Electrolytic Cells and Methods for the Production of Ammonia and Hydrogen](https://patents.google.com/patent/US20090095636)\n14. [Advanced Nickel-Based Catalysts for Urea Oxidation Reaction: Challenges and Developments (Catalysts, 2022)](https://www.mdpi.com/2073-4344/12/3/337)\n15. [Advancements in Ni-based Catalysts for Direct Urea Fuel Cells: A Comprehensive Review](https://chemistry-europe.onlinelibrary.wiley.com/doi/full/10.1002/celc.202300637)\n16. [S. J. YAO and colleagues (1973). Anodic Oxidation of Urea and an Electrochemical Approach to De-ureation. Nature.](https://doi.org/10.1038/241471a0)\n17. [Damilola A. Daramola, Deepika Singh, Gerardine G. Botte (2010). Dissociation Rates of Urea in the Presence of NiOOH Catalyst: A DFT Analysis. The Journal of Physical Chemistry A.](https://doi.org/10.1021/jp105159t)\n18. [Wei Chen and colleagues (2020). Unveiling the Electrooxidation of Urea: Intramolecular Coupling of the N−N Bond. Angewandte Chemie International Edition.](https://doi.org/10.1002/anie.202015773)\n19. [Shi-Kui Geng and colleagues (2021). Nickel ferrocyanide as a high-performance urea oxidation electrocatalyst. Nature Energy.](https://doi.org/10.1038/s41560-021-00899-2)\n20. [Urea electrooxidation: Research progress and application of supported nickel-based catalysts (Ionics, 2023)](https://link.springer.com/article/10.1007/s11581-023-05107-7)\n21. [Xintong Gao and colleagues (2023). Boosting urea electrooxidation on oxyanion-engineered nickel sites via inhibited water oxidation. Nature Communications.](https://doi.org/10.1038/s41467-023-41588-w)\n22. [Guangming Zhan and colleagues (2024). Highly selective urea electrooxidation coupled with efficient hydrogen evolution. Nature Communications.](https://doi.org/10.1038/s41467-024-50343-8)\n23. [Urine electrooxidation for energy-saving hydrogen generation (Nature Communications, 2025)](https://www.nature.com/articles/s41467-025-57798-3)\n24. [Scalable Electrocatalytic Urea Wastewater Treatment Coupled with Hydrogen Production by Regulating Adsorption Behavior of Urea Molecule (Nano-Micro Letters, 2024)](https://link.springer.com/article/10.1007/s40820-024-01585-0)\n\n---\n*Topic: Encyclopedia › Physical world and mathematics › Chemistry › Chemical principles and methods › Analytical chemistry › Electroanalysis and electrochemistry › Electrode kinetics and electron transfer*\n\n*Initially written Sep 29, 2026 · Reviewed: Sep 30, 2026 · Edited: Oct 15, 2026; Oct 25, 2026 · Last review: Sep 30, 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/urea-electrooxidation", "markdown_url": "https://www.edgepedia.org/urea-electrooxidation.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": "\"Urea electrooxidation\", Edgepedia (EdgeChat), https://www.edgepedia.org/urea-electrooxidation. Edgepedia Community License 1.0.", "credit_md": "\"[Urea electrooxidation](https://www.edgepedia.org/urea-electrooxidation)\", Edgepedia (EdgeChat), [https://www.edgepedia.org/urea-electrooxidation](https://www.edgepedia.org/urea-electrooxidation). [Edgepedia Community License 1.0](https://www.edgepedia.org/edgepedia/license).", "credit_html": "\"Urea electrooxidation\", Edgepedia (EdgeChat), https://www.edgepedia.org/urea-electrooxidation. Edgepedia Community License 1.0.", "speakable": "Urea electrooxidation is the electrochemical oxidation of urea at an anode, a six-electron reaction used to produce hydrogen with about 30% less energy than water electrolysis." }