User:Jaeyune/sandbox

1. Definitions of Non-faradaic promotions of catalysis 1) NEMCA effects 2) EPOC effects

2. Concepts of Non-faradaic promotion of catalysis 1) Principles 2) Theories

3. Classifications of Non-faradaic promotions of catalysis 1) Non-aqueous catalytic systems (high-temperature, higher than 200C) 2) Aqueous catalytic systems (low temperature, ambient temperature)

Electrochemical promotion of catalysis (EPOC) or non-faradaic electrochemical modification of catalytic activity (NEMCA) refers to the enhancement of electroless non-faradaic catalytic reactions at the electrode surface along with a given interfacial potential. The EPOC or NEMCA effects were firstly discovered by M. Stoukides and C. Vayenas in the 1980s and have been widely studied by various research groups for more than 100 heterogeneous catalytic reactions of gaseous molecules occurring at either metal or metal oxide surfaces interfaced with a solid electrolyte. By contrast, EPOC or NEMCA effects in an aqueous electrolyte solution at room temperature have rarely been addressed so far.Jaeyune (talk) 23:03, 15 April 2017 (UTC)

References (conventiaonl high temperature systems) [1] J. Phys. Chem. 1988, 92, 5083-5085 [2] Phys. Chem. Chem. Phys., 2010, 12, 9811–9815 [3] J. Am. Chem. Soc. 1997, 119, 11550-11551 [4] J Appl Electrochem (2010) 40:885–902

(Aqueous systems) [1] Nature 1994, 370, 45 (H2 oxidation) [2] J. Am. Chem. Soc. 2011, 133, 5425–5431 (Hydrazine oxidation) [3] J. Phys. Chem. 1996, 100, 14803-14814 (H2 oxidation)

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Wiki draft

Electrochemical Promotion of Catalysis (EPOC) effect

1. Introduction of EPOC effects

Electrochemical Promotion of Catalysis (EPOC) effect refers to the pronounced enhancement of catalytic reactions or the significant changes in catalytic properties of the conductive catalyst in the presence of electrical currents or interfacial potentials. Additionally, the EPOC effect is known to be utilized in a reversible manner to influence the selectivity of heterogenous catalytic reactions. The electronically conductive catalyst is usually in metallic or metal oxide states with the form of a porous film deposited on the solid electrolyte (O^2- or mixed O^2- electronic conductor). The EPOC effects were firstly discovered by M. Stoukides and C. Vayenas in the early 1980s and have been widely studied by various research groups for more than 100 heterogeneous catalytic reactions of mostly gaseous molecules occurring at either metal or metal oxide. The EPOC effect has been regarded as an intriguing phenomenon which can link electrocatalysis and heterogeneous thermal catalysis.^[1,2]

2. The examples and research area

According to previous reports, the EPOC effect can be observed in a wide range of catalytic reactions with several kinds of metal or metal oxide catalysts mostly coupled with solid electrolytes. Versatile catalytic reactions including hydrogenations, dehydrogenations, oxidations, reductions, isomerizations, and chemical decompositions have been known to be promoted electrochemically on various transition metal and oxide catalysts (Pt, Pd, Rh, Ag, Au, Ni, Cu, Fe, IrO₂, RuO₂) deposited on O^2- (YSZ), Na⁺ or K⁺, H⁺, F^-, aqueous, CeO₂ conductors, and molten salts.^[3] Main focus and purpose of numerous studies regarding the EPOC effect have been reported so far can be classified as follows:^[4] 1) elucidation of examples for the EPOC effects on specific catalytic reactions with environmental or industrial interest (NOx reduction and hydrocarbons oxidations), 2) mechanistic investigation of the origin of the EPOC effect (mainly focusing on oxygen ion conductors), 3) large-scale application and commercialization of the chemical reactions promoted by the EPOC effect along with development of novel compact monolithic reactors and 4) Utilization and incorporation of the EPOC effect in high or low temperature fuel cell systems.

3. The proposed mechanistic origin of the EPOC effects

Earlier mechanistic proposals for the EPOC phenomenon with solid electrolytes mainly emphasized on tuning of the local work function of the conductive catalyst surface by spilled-over species which are in-situ generated during electrochemical polarization processes. It has been proposed that the spilled-over species can subsequently modulate the chemisorption strength between surface adsorbates (intermediates) and catalyst binding sites, thereby influencing the rate or selectivity of the target reactions. Particularly in the case of O^2- conducting electrolyte systems, for instance, the migrated anionic O species from the solid electrolyte to the metal-gas interface has been suggested as the origin of the corresponding EPOC effects along with identification of the migrated charged species on the surface via spectroscopic methods. On the other hand, the idea about modification of the local work function to explain the origin of EPOC was recently criticized with a different view that heterogeneous catalysis needs to be explained by more recent concepts such as d-band center theory, rather than the surface work function, which might play a trivial role in understanding of surface reactions.

4. EPOC effects in an aqueous electrolyte solution at ambient temperature

In contrast to solid electrolyte systems under the condition of high temperature (usually higher than 200 C), EPOC has rarely been reported in low-temperature aqueous systems (particularly at room temperature). Only a few examples have been demonstrated for the EPOC in an aqueous electrolyte solution at ambient temperature: H₂ oxidation at Pt catalyst surface in alkaline solutions,^[5] hydrocarbon isomerization reaction occurring at the nanoparticulate Pt catalyst,^[6] CO oxidation,^[7] and hydrazine oxidation operating at the Ni alloy catalyst in alkaline media,^[8] and CO₂ reduction at the Pd-based gas diffusion electrode.^[9] Even though the perturbation of the local work function and tuning of surface binding strengths of intermediate species were suggested as the origin for the EPOC effects in the liquid electrolyte systems as similar to the EPOC examples of high temperature solid electrolyte systems, thorough theoretical studies supported by clear experimental evidence have never been addressed so far. Very recently, it was additionally hypothesized for the cases of the hydrazine oxidation and the CO₂ reduction that the mechanistic origin of the EPOC phenomena observed in these cases can be contributed to structurally non-disparate transition states and/or surface bound intermediate species for the corresponding bifurcated faradaic and non-faradaic reactions.^[8,9]

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Revised draft

The Electrochemical Promotion of Catalysis (EPOC) effect

Introduction of the EPOC effects

The Electrochemical Promotion of Catalysis (EPOC) effect in the realm of chemistry refers to the pronounced enhancement of catalytic reactions or significant changes in the catalytic properties of a conductive catalyst in the presence of electrical currents or interfacial potentials. Additionally, the EPOC effect can be utilized in a reverse manner in order to influence the selectivity of versatile heterogeneous catalytic reactions. In most cases, the electronically conductive catalyst is in metallic or metal oxide states in the form of a porous film deposited on a solid electrolyte (O2- or mixed O2- electronic conductor). The EPOC effect was firstly discovered by M. Stoukides and C. Vayenas in the early 1980s and have been widely studied by various research groups for more than 100 heterogeneous catalytic reactions of mostly gaseous molecules. The EPOC effect has been evaluated as an important phenomenon which can closely link electrocatalysis and thermal catalysis.[1,2]

Examples and research fields

The EPOC effect can be observed in a wide range of catalytic reactions with several kinds of metal or metal oxide catalysts mostly coupled with solid electrolytes. Versatile catalytic reactions including hydrogenations, dehydrogenations, oxidations, reductions, isomerizations, and chemical decompositions have been known to be promoted electrochemically on various transition metal and oxide catalysts (e.g., Pt, Pd, Rh, Ag, Au, Ni, Cu, Fe, IrO2, RuO2) deposited on O2- (YSZ), Na+ or K+, H+, F-, aqueous, CeO2 conductors, and molten salts.[3] The main focus and purpose of numerous studies regarding the EPOC effect have been reported so far can be classified as follows:[4] 1) the elucidation of examples for the EPOC effects on specific catalytic reactions with environmental or industrial interest (ex. NOx reduction and hydrocarbons oxidations), 2) the mechanistic investigation of the origin of the EPOC effects (mainly focusing on the system with oxygen-ion conducting electrolytes), 3) the large-scale application and commercialization of the chemical reactions promoted by the EPOC effects along with development of novel compact monolithic reactors and 4) the utilization and incorporation of the EPOC effect in high or low temperature fuel cell systems.

The proposed mechanistic origins of the EPOC effects

Earlier mechanistic proposals for the EPOC phenomenon with solid electrolytes mainly emphasized tuning of the local work function of the surface of conductive catalysts by spilled-over species, which are in-situ generated during electrochemical polarization processes. It has been proposed that the spilled-over species can subsequently modulate the chemisorption strength between surface adsorbates (intermediates) and catalyst binding sites, thereby influencing the rate or selectivity of the target reactions singnificantly. Particularly in the case of oxygen-ion-conducting electrolyte systems, for instance, the migrated anionic O species from the solid electrolyte to the metal-gas interface has been suggested as the origin of the corresponding EPOC effects along with the evidence that the migrated charged species on the surface can be identified via in-situ spectroscopic methods. On the other hand, the hypothesis of modification of the local work function to explain the origin of EPOC was recently criticized with a different view that heterogeneous catalysis needs to be explained by more recent concepts such as d-band center theory, rather than the surface work function, which might play a more trivial role in understanding of surface reactions.

EPOC effects in an aqueous electrolyte solution at ambient temperatures

In contrast to solid electrolyte systems under high temperatures (usually higher than 200 C), EPOC has rarely been reported in low-temperature aqueous systems (particularly at room temperature). Only a few examples have been demonstrated for the EPOC in an aqueous electrolyte solution at ambient temperature: H2 oxidation at Pt catalyst surface in alkaline solutions,[5,6] hydrocarbon isomerization reaction occurring at the nanoparticulate Pt catalyst,[6], hydrazine oxidation operating at the Ni alloy catalyst in alkaline media,[7] and CO2 reduction at the Pd-based gas diffusion electrode.[8] Even though the perturbation of the local work function and tuning of surface binding strengths of intermediate species were suggested as the origin for the EPOC effects in the liquid electrolyte systems as similar to the EPOC examples of high temperature solid electrolyte systems, thorough theoretical studies supported by clear experimental evidence have not been addressed. Very recently, it was additionally hypothesized for the cases of the hydrazine oxidation and the CO2 reduction that the mechanistic origin of the EPOC phenomena observed in these cases can be contributed to structurally non-disparate transition states and/or surface bound intermediate species for the corresponding bifurcated faradaic and non-faradaic reactions.[8,9]

References [main review 1] J Appl Electrochem (2010) 40:885–902 [review1] Progress in Surface Science 85 (2010) 241–278 [old paper 1] J. Phys. Chem. 1988, 92, 5083-5085 [2] Phys. Chem. Chem. Phys., 2010, 12, 9811–9815 [3] J. Am. Chem. Soc. 1997, 119, 11550-11551

[5] Nature 1994, 370, 45 (H2 oxidation) [6] J. Phys. Chem. 1996, 100, 14803-14814 (H2 oxidation) [7] J. Am. Chem. Soc. 1997, 119, 11550-11551 (Isomerization) [8] J. Am. Chem. Soc. 2011, 133, 5425–5431 (Hydrazine oxidation) [9] Chem. Sci., 2017, 8, 2569–2573 (CDR)

Jaeyune (talk) 21:56, 16 May 2017 (UTC)

Jaeyune (talk) 21:11, 9 May 2017 (UTC)