ライフサイエンスコーパス: electrolysis

1 Koutechy-Levich plots, and constant-current electrolysis).

2 ggesting a reliable cathode material for CO2 electrolysis.

3 rgy storage, including water, CO(2) and N(2) electrolysis.

4 bamazepine (>80%) was achieved within 3 h of electrolysis.

5 gnificant alteration after more than 80 h of electrolysis.

6 ity and mass activity towards alkaline water electrolysis.

7 es the most energy-inefficient step in water electrolysis.

8 talyst at the anode and cathode during water electrolysis.

9 ed with these TiO2 |MnP electrodes after 2 h electrolysis.

10 le to oxidize ethanol to CO(2) after 10 h of electrolysis.

11 ic voltammetry (CV) and controlled potential electrolysis.

12 voltammetry and controlled-potential (bulk) electrolysis.

13 ivation of the catalyst during the course of electrolysis.

14 showing substantial promise for use in water electrolysis.

15 ccessfully fabricated for bifunctional water electrolysis.

16 to monitor the activity and stability during electrolysis.

17 dition of As(III) during the course of water electrolysis.

18 s sunlight to electricity and H(2) via water electrolysis.

19 he local pH near the catalyst surface during electrolysis.

20 offers many advantages compared to a direct electrolysis.

21 corporated them into Al(OH)3(s) flocs during electrolysis.

22 f the catalyst was demonstrated by continued electrolysis.

23 hemical double layer under the conditions of electrolysis.

24 tributed to the ions produced as a result of electrolysis.

25 ion ratio against H2O2 production during H2O electrolysis.

26 ved leading to better destabilization during electrolysis.

27 n be produced at separate times during water electrolysis.

28 or in high-surface-area electrodes for water electrolysis.

29 oxygen depolarized cathode for chlor-alkali electrolysis.

30 the content of nitrite or nitrate ions upon electrolysis.

31 liquid extraction (pertraction) and membrane electrolysis.

32 physical properties of the electrodes after electrolysis.

33 bon losses in low-temperature carbon dioxide electrolysis.

34 tion reaction catalyst for alkaline seawater electrolysis.

35 ively unrefined for currently carbon dioxide electrolysis.

36 ectrode exhibits outstanding stability after electrolysis.

37 esistance to the acid corrosion during water electrolysis.

38 oelectrochemistry after controlled-potential electrolysis.

39 plore its use in fabrication of solar-driven electrolysis.

40 This electrolysis-activation strategy offers a safe, accessib

41 During a constant current electrolysis almost any oxidation and reduction reaction

42 ining the optimal straining effect for water electrolysis, along with experimental approaches for cre

43 rt-chain carboxylates to esters via membrane electrolysis and biphasic esterification.

44 increasingly used in solid oxide fuel cells, electrolysis and catalysis, it is desirable to obtain a

45 cation of direct current (DC), thus inducing electrolysis and creating localized pH changes around th

46 tions, which are the critical steps for both electrolysis and fuel cell operation, especially at redu

47 rmance, but also offer proof of concept that electrolysis and fuel cells can be unified in a single,

48 tified for alkaline and neutral medium water electrolysis and fuel cells.

49 cted to monitor protein concentration during electrolysis and gauge changes in the electrode surface

50 licate mineral dissolution with saline water electrolysis and H2 production to effect significant air

51 electrochemical flow cell system for sulfite electrolysis and hydrogen production, with potential app

52 strate significantly enhanced carbon dioxide electrolysis and improved durability.

53 evolution reaction (OER) in PEM based water electrolysis and metal air batteries remains one of the

54 renewable energy technologies such as water electrolysis and metal-air batteries.

55 s of overall water splitting by membraneless electrolysis and photocatalysis.

56 vity advantages of this approach relative to electrolysis and photoredox catalysis.

57 ) center, as observed with preparative scale electrolysis and verified with (13)CO2.

58 is rate limiting in both the forward (water electrolysis) and reverse (H2 electro-oxidation) reactio

59 of reactions, those initiated by electrons (electrolysis) and those initiated by gaseous neutral spe

60 ariety of applications, including catalysis, electrolysis, and photovoltaics.

61 sities of approximately 1 mA/cm(2) over 30-h electrolysis are achieved at a 2.5-V cell voltage, split

62 radicals (e.g., HO(*)) generated from water electrolysis are responsible for defect formation on gra

63 ology, whereas fundamental advances in CO(2) electrolysis are still needed to enable short-term and s

64 of lattice oxygen in the mechanism of water electrolysis as revealed through ab initio modelling.

65 ould be more suitable for Cu-catalyzed CO(2) electrolysis as these CO(2) sources would be relatively

66 nm) and polydispersity during just 15 min of electrolysis at -0.80 V (vs RHE).

67 diameter) are synthesized during a 4 h CO(2) electrolysis at 0.1 A cm(-2).

68 Controlled-potential electrolysis at 1.61 V vs NHE at pH 7.2 resulted in sust

69 volution takes place in controlled potential electrolysis at a relatively low overpotential of 640 mV

70 and cimetidine was achieved within 30 min of electrolysis at an applied potential of 3.5 V (0.7 A L(-

71 thode lattice that determines carbon dioxide electrolysis at elevated temperatures.

72 Hydrogen evolution can be easily achieved by electrolysis at large potentials that can be lowered wit

73 roves the reaction kinetics, and enables the electrolysis at low temperatures.

74 After checking electrolysis at the reported potential and at a more neg

75 This nickel was not added to the electrolysis baths deliberately, but it was found to be

76 When coupled to electrolysis, biodegradation of 1,4-dioxane was sustaine

77 the costs of hydrogen production from water electrolysis by serving as stable, low-cost supports for

78 ll the technologies for H2 production, steam electrolysis by solid oxide electrolysis cells (SOECs) h

79 This work demonstrated that bulk electrolysis can be achieved in a few seconds in these a

80 dialysis membrane interface that eliminates electrolysis-caused protein oxidation/reduction and cons

81 l reaction proceeds through constant current electrolysis (CCE) by taking advantage of the dual role

82 into ethanol was investigated in a microbial electrolysis cell (MEC) driven by the exoelectrogen Geob

83 Consequently, we developed a microbial electrolysis cell (MEC) driven by the synergistic metabo

84 When a mixed-culture microbial electrolysis cell (MEC) is fed with a fermentable substr

85 The capacity of a microbial electrolysis cell (MEC) to produce hydrogen gas (H2) usi

86 c treatment system that combined a microbial electrolysis cell (MEC) with membrane filtration using e

87 ic performance with a H2-producing microbial electrolysis cell (MEC).

88 odel is proposed for the optimization of the electrolysis cell characteristics.

89 e found that the durability of the AEM-based electrolysis cell could be improved by incorporating a h

90 the precise matching of half reactions in an electrolysis cell is not generally necessary.

91 ture that integrates the light harvester and electrolysis cell to convert CO(2) into valuable chemica

92 At 50 degrees C, an AEM electrolysis cell using iridium oxide as the anode catal

93 The efficacy of our electrolysis cell was further demonstrated by a 20 L pro

94 We demonstrated an AEM-based electrolysis cell with a lifetime of >535 h.

95 lectrogenesis in the bioanode of a microbial electrolysis cell.

96 forming a microbial reverse-electrodialysis electrolysis cell.

97 ructures perform well as both fuel cells and electrolysis cells (for example, at 900 degrees C they d

98 catalysts limit the application of microbial electrolysis cells (MECs) for hydrogen (H(2)) production

99 in the rate of acetate removal in microbial electrolysis cells (MECs), but studies with fermentable

100 on study of ammonia recovery using microbial electrolysis cells (MECs).

101 d at -0.06 V (vs) SHE in duplicate microbial electrolysis cells (MECs).

102 roduced in microbial reverse-electrodialysis electrolysis cells (MRECs) using current derived from or

103 roduction, steam electrolysis by solid oxide electrolysis cells (SOECs) has attracted much attention

104 conversion systems such as solid oxide fuel/electrolysis cells and catalysts for thermochemical H2O

105 The electrolysis cells employ multilayer semiconductor anode

106 atively high redox potentials, and microbial electrolysis cells for reducing Cd(II) as this metal has

107 ons in small-scale, distributed, and on-site electrolysis cells powered by renewable electricity gene

108 cells that generate electricity or microbial electrolysis cells that produce hydrogen or methane.

109 dizing a fuel to produce electricity, and as electrolysis cells, electrolysing water to produce hydro

110 as mixing in the headspaces of high-pressure electrolysis cells, with implications for safety and ele

111 as graphene oxide or electrodes in microbial electrolysis cells.

112 electrode, SHE) in single-chamber microbial electrolysis cells.

113 Upon electrolysis, chloride is deposited at the Ag electrode

114 lsed voltammetric techniques and small-scale electrolysis combined with HPLC-MS/MS analyses.

115 on of the hydrogenation compartment from the electrolysis compartment therefore broadens the scope of

116 ntional extraction practices, direct sulfide electrolysis completely avoids generation of problematic

117 Here it is shown that the same electrolysis conditions, but with the addition of 7.7 wt

118 arly, 2-aminobutyrate is also observed under electrolysis conditions.

119 ough long-term potential cycles and extended electrolysis confirm the exceptional durability of the c

120 Compared with abiotic electrochemical electrolysis control, the microbial assisted graphite ox

121 Electrolysis converts electrical energy into chemical en

122 h current efficiency by controlled potential electrolysis (CPE).

123 catalytic electrodes for incorporation into electrolysis devices.

124 haloacetic acids and trihalomethanes) during electrolysis dramatically exceeded recommendations for d

125 idation" to benzoic acids; H2 is released by electrolysis, enabling additional reaction cycles.

126 cathode, respectively, achieving a very high electrolysis energy efficiency exceeding 80% at consider

127 The OER catalytic activity as well as electrolysis energy efficiency surpasses any previously

128 tside the electrolyzer that requires no post-electrolysis energy input.

129 drogen with high Faradaic efficiency in bulk electrolysis experiments over time intervals ranging fro

130 of nickel on anodes from extended-time bulk electrolysis experiments was confirmed by XPS.

131 DC-powered laboratory-scale electrolysis experiments were performed under static ano

132 e oxidation products, preparative scale bulk electrolysis experiments were undertaken.

133 Controlled potential electrolysis experiments with 1 at pH 8.0 at an applied

134 In preparative electrolysis experiments with a series of alcohol substr

135 In bulk electrolysis experiments, conducted at -1.2 V vs SCE usi

136 During bulk electrolysis experiments, gas chromatography and mass sp

137 lysis (FOWA) or analytical treatment of bulk electrolysis experiments.

138 icantly advances the development of seawater electrolysis for large-scale hydrogen production.

139 After electrolysis, full equilibration of the alkalized soluti

140 The preparative scale electrolysis generated epoxide-ring-opened/Friedel-Craft

141 al of eta = 360 mV, and controlled potential electrolysis generated more than 1000 turnovers at eta =

142 After three-hour electrolysis, glycerol is selectively oxidized to glycer

143 .3 nm increase to only 2.2 +/- 0.5 nm during electrolysis in 0.10 M NaHCO3 at -0.80 V (vs RHE).

144 (SO(2)) on Ag-, Sn-, and Cu-catalyzed CO(2) electrolysis in a flow-cell electrolyzer in near-neutral

145 The literature is largely based on electrolysis in a glass beaker or H-cells that often giv

146 with the established method of expansion by electrolysis in a Li(+) containing electrolyte, and then

147 performance, durable alkaline membrane water electrolysis in a solid-state cell.

148 These first-time results of water electrolysis in a solid-state membrane cell are promisin

149 The CNS synthesis splits CO(2) by electrolysis in molten carbonate and has a carbon negati

150 tion (1.1 kWh kg(-1) MCCA oil) than membrane electrolysis in series with pertraction (9.9 kWh kg(-1)

151 Here we demonstrate a paired electrolysis in the case of the oxidative condensation o

152 Developing efficient catalysts for electrolysis, in particular for the oxygen evolution in

153 two-electron reduction products during bulk electrolysis, including formate, aqueous formaldehyde, a

154 Controlled potential bulk electrolysis indicates that 94-99% of the nominal charge

155 s underwent structural transformation during electrolysis into electrocatalytically active cube-like

156 ssolved in a 750 degrees C molten Li2CO3, by electrolysis, into O2-gas at a nickel electrode, and at

157 Solid oxide electrolysis is a highly efficient, high temperature app

158 Among the hydrogen production methods, water electrolysis is a promising method because of its zero g

159 This work suggests that glucose electrolysis is an energy-saving and cost-effective appr

160 ne with one another to control the course of electrolysis is analyzed in detail, leading to procedure

161 Even when the electrolysis is carried out at -1.20 V, the higher-gener

162 ial impact of contaminants on carbon dioxide electrolysis is crucial for practical applications.

163 The low-cost hydrogen production from water electrolysis is crucial to the deployment of sustainable

164 Water electrolysis is one of the most promising methods to pro

165 , under which proton exchange membrane-based electrolysis is operational.

166 Electrolysis is participating in the trend toward contin

167 uel community based on strain-promoted water electrolysis is proposed.

168 h and flow, we conclude that continuous flow electrolysis is superior to batch, producing a good yiel

169 generation of dissolved hydrogen in situ via electrolysis, is described.

170 ectrochemical experiments revealed that bulk electrolysis may also be used to switch reversibly the c

171 tudies combining cyclic voltammetry and bulk electrolysis measurements enabled one to bring out four

172 , which is currently prepared using a costly electrolysis method with limited productivity.

173 e regenerated using the controlled-potential electrolysis method.

174 hat the designed cell used in flow injection electrolysis mode reduced the NaCl concentration from 0.

175 ated by converting the generated hydrogen in electrolysis mode to electricity without any hydrogen ad

176 Molten oxide electrolysis (MOE) is an electrometallurgical technique

177 serve as the "inert" anode for molten oxide electrolysis (MOE).

178 We then applied FND using an electrolysis needle.

179 ative to experimental controls following the electrolysis of 0.25 M Na2SO4 solutions when the anode w

180 ponding to the first voltammetric peak, bulk electrolysis of 1-5 affords the corresponding hydrodimer

181 neO](2+) takes place at 1420 mV vs NHE, bulk electrolysis of [Ru(II)-OH(2)](2+) at 1260 mV vs NHE at

182 Bulk electrolysis of a saturated CO2 solution in the presence

183 ical pathway in which ammonia is produced by electrolysis of air and steam in a molten hydroxide susp

184 ved in each i-t response due to the complete electrolysis of all of the above-mentioned redox species

185 Evolution of oxygen was detected during bulk electrolysis of aqueous Et-Fl(+) solutions at several po

186 rate that C-N bonds can be formed through co-electrolysis of CO and NH(3) with acetamide selectivity

187 Although electrolysis of CO(2) or CO(2)-derived CO can generate i

188 Our results indicate that co-electrolysis of CO(2) with an oxidant is a promising str

189 e presence of surface hydroxyl species by co-electrolysis of CO(2) with low concentrations of O(2) ca

190 ate could be detected upon preparative-scale electrolysis of CO2 on the same electrode in the presenc

191 Electrolysis of diatrizoate in the presence of specific

192 In our approach, electrolysis of DSP-bridged protein/peptide products, as

193 cteristics of the system are tested with the electrolysis of Li2O2.

194 Spike-like responses from electrolysis of NB or TCNQ in each experiment were obser

195 The EGB, obtained when electrolysis of p-benzoquinone, or 1,4-naphthoquinone, i

196 3(B)Fe-N2(-) couple and controlled-potential electrolysis of P3(B)Fe(+) at -45 degrees C demonstrates

197 ical titration methods and achieves complete electrolysis of protein samples within minutes.

198 rms the lack of methanol formation upon bulk electrolysis of PyH(+) solutions at Pt and provides a de

199 is of single emulsion droplets, or selective electrolysis of redox species in single emulsion droplet

200 Electrolysis of saline creates localized pH gradients th

201 ich the configuration can be altered via the electrolysis of saline solutions or deionized water.

202 Electrolysis of seawater is not only a promising approac

203 f single collision signals from the complete electrolysis of single emulsion droplets, or selective e

204 ts of single-collision signals from the bulk electrolysis of single emulsion droplets.

205 rate are two base chemicals produced through electrolysis of sodium chloride brine which find uses in

206 f collision signal is observed, representing electrolysis of the droplet contents.

207 oated nanocavity allows for rapid exhaustive electrolysis of the sampled material.

208 Metals cannot be extracted by electrolysis of transition-metal sulfides because as liq

209 mation and accumulation was minimized during electrolysis of wastewater containing 75 mM Cl(-).

210 by the MFC electrical performance drives the electrolysis of wastewater towards the self-generation o

211 was similar during chemical chlorination and electrolysis of wastewater, suggesting that organic bypr

212 Typical catalysts for the electrolysis of water at low pH are based on precious me

213 contact with the acceptor solution inhibited electrolysis of water for approximately 30 min at 500 mu

214 e attractive candidates as catalysts for the electrolysis of water in alkaline energy storage and con

215 ing EME, the electrode effectively inhibited electrolysis of water in the acceptor compartment, by ac

216 cal fuel in the form of molecular H2 via the electrolysis of water is regarded to be a promising appr

217 The electrolysis of water provides a link between electrical

218 The electrolysis of water to produce hydrogen and oxygen is

219 postprinting process was developed using the electrolysis of water to selectively remove the insulati

220 The electrolysis of water using renewable energy inputs is b

221 t suffering gas formation or pH changes from electrolysis of water.

222 nd cathode at low applied potential to avoid electrolysis of water.

223 separated from each other in time during the electrolysis of water.

224 Glucose electrolysis offers a prospect of value-added glucaric a

225 Electrolysis offers an attractive route to upgrade green

226 During water electrolysis on ceria, the increase in surface potential

227 ngly, this new setup minimized the effect of electrolysis on extraction performance while enabling hi

228 k of understanding of the mechanism of water electrolysis on perovskite surfaces.

229 oxygen nanobubbles were generated from water electrolysis on the surface of a Au/Pd alloy modified IT

230 tential, and 12 times faster than by abiotic electrolysis only.

231 tion eliminates the unwanted side effects of electrolysis or joule heating at electrodes compared to

232 er splitting for hydrogen production through electrolysis or photoelectrochemistry.

233 Coulombic efficiency over 50 cycles by bulk electrolysis owing to efficient, long-distance intrapart

234 orted piperidine (SiO(2)-Pip)], and the main electrolysis parameters (current density, charge consump

235 cm(2) with 29,000 turnovers per site over an electrolysis period of 2 h.

236 2 through at least 29 turnovers over an 15 h electrolysis period with a 45% Faradaic yield and no obs

237 low-cost, earth-abundant materials for water electrolysis/photolysis.

238 N(2) electrolysis, plasma-enabled N(2) activation, and electr

239 large scale by the environmentally-friendly electrolysis process is currently hampered by the slow k

240 s Galvanic Zn-CO(2) cell and a solar-powered electrolysis process successfully demonstrated the effic

241 ich is about 50-55 % of state-of-the-art HCl electrolysis processes.

242 Conventional water electrolysis produces H(2) and O(2) simultaneously, such

243 In all cases except 2b, the bulk electrolysis product is [R3S3](+), consistent with earli

244 d as an intermediate in the formation of the electrolysis product, the trisulfide [Ar3S3](+).

245 on different RAPs is accessible and that the electrolysis products are stable upon cycling.

246 -5 V), which reduces the quantity of gaseous electrolysis products below a threshold that interferes

247 Identified halogenated and oxygenated electrolysis products typically underwent further transf

248 TO by nanoITO-Ru(V)(O)(3+) leads to multiple electrolysis products.

249 organic contaminant treatment, test compound electrolysis rate constants were measured in authentic l

250 This pairing of an electrolysis reaction with the production of a chemical

251 This design minimizes contamination from the electrolysis reactions by keeping the particles distant

252 Together these results indicate that electrolysis reactions generating hypochlorous acid from

253 ions, where oxygen (O2) gas formed via water electrolysis reacts in the bulk of the plasma to form NO

254 self-powered reactor for in situ wastewater electrolysis, recovering nitrogen from wastewater.

255 The implementation of seawater electrolysis requires robust and efficient electrocataly

256 voids the high energy costs and emissions of electrolysis, requires signification "dilution" (~ 8 Mt)

257 Electrolysis revealed a stable amperometric curve and an

258 of the complex before and after 18+ hours of electrolysis reveals negligible decomposition under cata

259 Controlled potential electrolysis shows sustained water oxidation over multip

260 d kinetic barriers towards interfacial water electrolysis significantly expand the electrochemical st

261 tion did not appreciably deplete, the second electrolysis step may be used to partially compensate fo

262 emanding reduction-first pathway, while bulk electrolysis studies confirm a high product selectivity

263 Controlled potential electrolysis studies confirm that the product of isoprop

264 Cyclic voltammetry and controlled potential electrolysis studies demonstrate that the immobilized ca

265 , infrared spectroelectrochemistry, and bulk electrolysis studies.

266 H bands were detected in floated flocs after electrolysis, suggesting the sorption and subsequent rem

267 Also, mass shift before and after electrolysis suggests the linkage pattern of cross-links

268 Here we report a photovoltaic-electrolysis system with the highest STH efficiency for

269 ts demonstrate the potential of photovoltaic-electrolysis systems for cost-effective solar energy sto

270 Extended time-scale controlled potential electrolysis (t > hours) and spectroscopic (EPR and in s

271 D efforts towards efficient and stable water electrolysis technologies.

272 arbonate relative to lithium carbonate at an electrolysis temperature of 670 degrees C produced over

273 dium or 30 wt% of potassium carbonate, or at electrolysis temperatures less than 700 degrees C.

274 upport fast (reversible) HET for Fe(CN)6(4-) electrolysis, the first time this has been reported at a

275 iency for methanation of 80% during extended electrolysis, the highest Faradaic efficiency for room-t

276 gh a combination of voltammetry, preparative electrolysis, thiol-electrode modifications, and kinetic

277 ormation of Fe(II-III) (hydr)oxides at short electrolysis times (<20 min).

278 We demonstrate that at short electrolysis times (0.5 min), i.e., high charge dosage r

279 e study on a new technology for chlor-alkali electrolysis to be introduced in Germany.

280 Water electrolysis to hydrogen and oxygen is a well-establishe

281 ctrochemical process that uses neutral water electrolysis to produce a pH gradient in which CaCO(3) i

282 des that had been subjected to different pre-electrolysis treatments.

283 ice underwent either trigeminal stereotactic electrolysis (TSE), or sham operation, to ablate the oph

284 the performance and stability during sulfite electrolysis under alkaline conditions are evaluated.

285 4S] clusters in the 2+ and 3+ states by bulk electrolysis under an O2-free atmosphere.

286 ater and use of the GAC as the cathode of an electrolysis unit also debrominated sorbed CH3Br.

287 However, two-compartment membrane electrolysis unit without pertraction was not able to se

288 , hydrogen, if efficiently produced by water electrolysis using renewable energy input, would revolut

289 degrees C and 25 bar of steam pressure, the electrolysis voltage necessary for 2 mA cm(-2) current d

290 acidic cathode at 500 mA.cm(-2) with a total electrolysis voltage of ~2.2 V.

291 Although the principle of indirect electrolysis was established many years ago, new, exciti

292 Oxygen production through water electrolysis was not detected on the anode due to the pr

293 On the basis of these results, electrolysis was performed, resulting in the simultaneou

294 Bulk electrolysis was used to generate HA in a defined reduct

295 n an elevated residual current reading after electrolysis were eliminated.

296 ubstantial residual currents observed during electrolysis were found to be a result of NaCl back diff

297 d yield of 83% are obtained from the glucose electrolysis, which takes place via a guluronic acid pat

298 A gaseous HCl electrolysis with Fe(3+) /Fe(2+) redox-mediated cathode

299 t COD and NH4(+) can be removed after 2 h of electrolysis with minimal energy consumption (370 kWh/kg

300 ntaining nanoclusters in water via precision electrolysis with strict pH control and (ii) an improved