Welcome to LookChem.com Sign In|Join Free

Cas Database

80937-33-3

80937-33-3

Identification

  • Product Name:oxygen

  • CAS Number: 80937-33-3

  • EINECS:

  • Molecular Weight:31.9988

  • Molecular Formula: O2

  • HS Code:

  • Mol File:80937-33-3.mol

Synonyms:oxygen

Post Buying Request Now
Entrust LookChem procurement to find high-quality suppliers faster

Safety information and MSDS view more

  • Signal Word:no data available

  • Hazard Statement:no data available

  • First-aid measures: General adviceConsult a physician. Show this safety data sheet to the doctor in attendance.If inhaled If breathed in, move person into fresh air. If not breathing, give artificial respiration. Consult a physician. In case of skin contact Wash off with soap and plenty of water. Consult a physician. In case of eye contact Rinse thoroughly with plenty of water for at least 15 minutes and consult a physician. If swallowed Never give anything by mouth to an unconscious person. Rinse mouth with water. Consult a physician.

  • Fire-fighting measures: Suitable extinguishing media Use water spray, alcohol-resistant foam, dry chemical or carbon dioxide. Wear self-contained breathing apparatus for firefighting if necessary.

  • Accidental release measures: Use personal protective equipment. Avoid dust formation. Avoid breathing vapours, mist or gas. Ensure adequate ventilation. Evacuate personnel to safe areas. Avoid breathing dust. For personal protection see section 8. Prevent further leakage or spillage if safe to do so. Do not let product enter drains. Discharge into the environment must be avoided. Pick up and arrange disposal. Sweep up and shovel. Keep in suitable, closed containers for disposal.

  • Handling and storage: Avoid contact with skin and eyes. Avoid formation of dust and aerosols. Avoid exposure - obtain special instructions before use.Provide appropriate exhaust ventilation at places where dust is formed. For precautions see section 2.2. Store in cool place. Keep container tightly closed in a dry and well-ventilated place.

  • Exposure controls/personal protection:Occupational Exposure limit valuesBiological limit values Handle in accordance with good industrial hygiene and safety practice. Wash hands before breaks and at the end of workday. Eye/face protection Safety glasses with side-shields conforming to EN166. Use equipment for eye protection tested and approved under appropriate government standards such as NIOSH (US) or EN 166(EU). Skin protection Wear impervious clothing. The type of protective equipment must be selected according to the concentration and amount of the dangerous substance at the specific workplace. Handle with gloves. Gloves must be inspected prior to use. Use proper glove removal technique(without touching glove's outer surface) to avoid skin contact with this product. Dispose of contaminated gloves after use in accordance with applicable laws and good laboratory practices. Wash and dry hands. The selected protective gloves have to satisfy the specifications of EU Directive 89/686/EEC and the standard EN 374 derived from it. Respiratory protection Wear dust mask when handling large quantities. Thermal hazards

Supplier and reference price

  • Manufacture/Brand
  • Product Description
  • Packaging
  • Price
  • Delivery
  • Purchase

Relevant articles and documentsAll total 430 Articles be found

Adsorption and reactivity of nitrogen oxides (NO2, NO, N2O) on Fe-zeolites

Rivallan, Mickael,Ricchiardi, Gabriele,Bordiga, Silvia,Zecchina, Adriano

, p. 104 - 116 (2009)

Nitrous oxide decomposition and temperature programmed desorption tests on Fe-ZSM-5 and Fe-silicalite show that the catalytic conversion mechanism of N2O into N2 and O2 over Fe-zeolites is more complex than expected. Nitro

Tuning the O2 Binding Affinity of Cobalt(II) Centers by Changing the Structural and Electronic Properties of the Distal Substituents on Azole-Based Chelating Ligands

Nishiura, Toshiki,Chiba, Yosuke,Nakazawa, Jun,Hikichi, Shiro

, p. 14218 - 14229 (2018)

The effects of the substituents on the chelating ligands located in the secondary coordination sphere on the O2 affinity of cobalt(II) centers have been explored. The combination of facially capping tridentate tris(pyrazolyl)borates (= TpMe2,4R) and bidentate bis(imidazolyl)borates (= [B(ImN-Me)2MeX]- LX) yields square-pyramidal cobalt(II) complexes. The structural properties of the substituent groups X attached to the boron center of LX affect the arrangement of X in the resulting cobalt(II) complexes [CoII(TpMe2,4R)(LX)]. When the boron-attached moiety of X is a relatively bulky sp3-CH2Y group (i.e., X:Y = Me:H and nBu:nPr), the alkyl group X faces the cobalt center, whereas for isopropoxy (OiPr) and phenyl (Ph) groups, of which the boron-attached atoms are a less hindered oxygen atom and a planer sp2-carbon, respectively, the X group is arranged away from the cobalt center. This flexible behavior of LX is reflected in the O2 affinity of the cobalt(II) center, which depends on the extent to which the complex sphere is shielded by the ligands. The dependence of the cobalt(II) oxidation potential on the X substituent of LX is inconsistent with the O2 affinity. On the other hand, the electronic properties of R, which is attached to the fourth position of the pyrazolyl rings in the rigid TpMe2,4R ligand, are reflected in the electrochemical properties and O2 affinity of the cobalt center.

Decomposition of Nitrous Oxide on Palladium Crystal Planes

Eley, Daniel D.,Klepping, Anthony H.,Moore, Peter B.

, (1985)

The catalysed decomposition of N2O in the range 830 - 1000 K and 0.05 - 1.0 Torr (1 Torr ca. 133 Pa) has been examined on Pd single-crystal surfaces and polycrystalline wires and compared with earlier work.The relative reaction velocities at 1000 deg K an

Oxidatively induced reductive elimination of dioxygen from an η2-peroxopalladium(II) complex promoted by electron-deficient alkenes

Popp, Brian V.,Stahl, Shannon S.

, p. 2804 - 2805 (2006)

The first example of associative displacement of dioxygen from a peroxopalladium(II) complex is reported. Electron-deficient alkenes, p-X-trans-β-nitrostyrene (X = OCH3, CH3, H, F, Br, CF3, NO2), react quantitatively with (bc)Pd(η2-O2) (bc = bathocuproine) in dichloromethane at room temperature to form the corresponding palladium(0)-alkene complexes. Mechanistic studies indicate that ligand substitution proceeds through an associative mechanism, and the electronic characteristics of the reactions are consistent with an oxidatively induced reductive elimination pathway. Copyright

Reversible O2 binding to a dinuclear copper(I) complex with linked tris(2-pyridylmethyl)amine units: Kinetic-thermodynamic comparisons with mononuclear analogues

Lee, Dong-Heon,Wei, Ning,Murthy, Narasimha N.,Tyeklár, Zoltán,Karlin, Kenneth D.,Kaderli, Susan,Jung, Bernhard,Zuberbühler, Andreas D.

, p. 12498 - 12513 (1995)

The kinetics and thermodynamics of reaction of O2 with copper(I) complexes can provide fundamental information relevant to chemical and biological systems. Using diode-array variable-temperature (180-296 K) stopped-flow kinetic methods, we report detailed information on the O2 reactivity (in EtCN) of dicopper(I) complex [(D1)Cu(I)2(RCN)2]2+ (2a) (R = Me or Et) [D1 = dinucleating ligand with a -CH2CH2- group linking two tris(2-pyridylmethyl)amine (TMPA) units at a 5-pyridyl position of each tetradentate moiety]. A comparative study of mononuclear complex [(TMPAE)Cu(RCN)]+ (1a') [TMPAE has a -C(O)OCH3 ester substituent in the 5-position of one pyridyl group of TMPA] has been carried out. The results are compared with data from the previously investigated complex [(TMPA)Cu(RCN)]+ (1a). The syntheses of D1 and 2a-(ClO4)2 are described; an X-ray structure reveals two pentacoordinate Cu(I) ions (Cu···Cu = 11.70 A?), each bound by the N4-tetradentate and an EtCN molecule. Cyclic voltammetric data for 1a' and 2a are reported. At 193 K in EtCN, 2a reacts with O2 (Cd/C2 = 2:1, manometry) to produce an intensely purple colored solution of adduct [(D1)Cu2(O2)]2+ (2c), λ(max) = 540 nm (ε = 11 100 M-1 cm-1). This peroxo-dicopper(II) species reacts with PPh3, liberating O2 and producing the isolatable bis-phosphine adduct [(D1)Cu2(PPh3)2]2+. The kinetic investigation provides spectral characterization of transient Cu/O2 1:1 adducts generated upon oxygenation of cold solutions of 1a' or 2a. [(TMPAE)Cu(O2)]+ (1b') forms reversibly (λ(max) = 415 nm) with k1 = (8.2 ± 0.4) x 103 M-1 s-1 and K1 = k1/k-1 = (284 ± 9) M-1 at 183 K, with ΔH1° = (-32 ± 1) kJ mol-1, ΔS1° = (-127 ± 3) J K-1 mol-1. Two types of Cu(II)-O2- complexes form in the reaction of 2a: a 2:1 open form (i.e., [(D1)Cu2(O2)(EtCN)]2+, 2b) and a bis-O2 2:2 open adduct (i.e., [(D1)Cu2(O2)2]2+, 2b'). For the formation of 2b, k1 = (1.63 ± 0.01) x 104 M-1 s-1 and K1 = (2.03 ± 0.04) x 103 M-1 at 183 K. Complexes 2b and 2b' have identical spectroscopic properties (λ(max) = 416 nm, ? = 4500 M-1 cm-1) per Cu-O2 unit, and their rate constants are statistically related. Intermediates 1b' and 2b further convert into (μ-peroxo)dicopper(II) [(2 Cu):(1O2)] complexes. [{(TMPAE)Cu}2(O2)]2+ (1c') (λ(max) = 532 nm, ? = 9380 M-1 cm-1) forms in a second-order reaction of 1b' with 1a' with K1K2 = (2.1 ± 0.4) x 1011 M-2 at 183 K (ΔH12° = -77 ± 1 kJ mol-1 and AS12° = -203 ± 5 J K-1 mol-1), while [(D1)Cu2(O2)]2+ (2c) (λ(max) = 540 nm, ? = 11 100 M-1 cm-1) is generated from 2b in an intramolecular reaction,with k2 = (3.51 ± 0.05) x 101 s-1 and k(on) = k1k2/k-1 = (7.1 ± 0.2) x 104 M-1 s-1 (183 K). The overall formation of 2c is faster than for 1c' or [{(TMPA)Cu}2(O2)]2+ (1c) because of a more positive entropy of activation (ΔS(on)paragraph = (-139 ± 3) J K-1 mol-1 for 2c vs ΔS(on)paragraph = (-201 ± 5) J K-1 mol-1 for 1c). However, this significantly enhanced kinetic reactivity (for 2a → 2c) is not reflected by an analogous increase in thermodynamic stability. [(D1)Cu2(O2)]2+ (2c) is enthalpically less stable (ΔH12° = (-34.8 ± 0.4) kJ -1) than Cu2O2 species 1c and 1c' (ΔH12° = -81 to -77 kJ mol-1, respectively), which are formed from mononuclear precursors. There is a substantially larger overall formation entropy for 2c [ΔS12° = (-89.3 ± 1.5) J K-1 mol-1 compared to -220 and -203 J K-1 mol-1 for 1c and 1c', respectively] since Cu2O2 formation is an intramolecular, rather than intermolecular, process. Examination of other kinetic parameters and spectral differences provides complementary information that 2c has a strained structure. In fact, 2c is not the ultimate oxidation product: relief of steric constraints occurs at higher temperatures by a slow rearrangement (λ(max) = 540 nm → λ(max) = 529 nm) producing {Cu2O2}(n) oligomers containing intermolecular Cu-O2-Cu bonds. A particularly stable trimer species [{(D1)Cu2(O2)}3]6+ (2d) was characterized, with ΔH3° = (-153 kJ mol-1)/3 = -51 kJ mol-1 per Cu2O2 unit, intermediate between that seen for 2c, 1c, and 1c'.

N2O decomposition over Fe-zeolites: Structure of the active sites and the origin of the distinct reactivity of Fe-ferrierite, Fe-ZSM-5, and Fe-beta. A combined periodic DFT and multispectral study

Sklenak, Stepan,Andrikopoulos, Prokopis C.,Boekfa, Bundet,Jansang, Bavornpon,Novakova, Jana,Benco, Lubomir,Bucko, Tomas,Hafner, Juergen,Ddeek, Jii,Sobalik, Zdenk

, p. 262 - 274 (2010)

The N2O decomposition over Fe-ferrierite, Fe-beta, and Fe-ZSM-5 has been recently studied [K. Jisa, J. Novakova, M. Schwarze, A. Vondrova, S. Sklenak, Z. Sobalik, J. Catal. 262 (2009) 27] and a superior activity of Fe-ferrierite with respect to Fe-beta and Fe-ZSM-5 has been shown. In this study, we investigated (1) plausible active sites for the N2O decomposition over Fe-ferrierite and (2) the origin of the distinct reactivity of Fe-ferrierite, Fe-ZSM-5 and Fe-beta employing a combined theoretical (periodic DFT) and experimental (UV-vis-NIR spectroscopy, IR spectroscopy, 29Si MAS NMR spectroscopy and catalytic batch experiments) approach. We evidenced that two Fe(II) cations accommodated in two adjacent six-membered rings in the eight-membered ring channel (β sites) of Fe-ferrierite (the calculated Fe-Fe distance is 7.4 ) form the active site responsible for the superior activity of this catalyst in the N2O decomposition in the absence of NO. Similar structures can be formed in Fe-beta. However, the probability of their formation is very low. For Fe-ZSM-5, the geometrical arrangement of the cationic positions is far from that in Fe-ferrierite and it is not suitable for the N2O decomposition. Therefore, the predicted order of the activity of the Fe(II) exchanged zeolites agrees with our experimental findings and it is: Fe-ferrierite ? Fe-beta > Fe-ZSM-5. We further showed that the accommodation of divalent cations in rings forming cationic sites can lead to significant rearrangements of the local structures of the zeolite framework, and therefore, the precise structure of sites binding a divalent cation cannot be derived from results of X-ray diffraction experiments, but can be inferred from theoretical calculations.

Adsorbed Oxygen Species Formed by the Decomposition of N2O on Li/MgO Catalysts

Nakamura, Masato,Yanagibashi, Hiroshi,Mitsuhashi, Hiroyuki,Takezawa, Nobutsune

, p. 2467 - 2472 (1993)

A considerable amount of adsorbed oxygen species were produced by the decomposition of N2O on Li/MgO.The amount of the oxygen species greatly increases by Li(I)-doping on MgO.Over 0.7 wtpercent Li/MgO, the amount of the oxygen species formed was 10.67 μmol m-2.The temperature-programmed desorption of the oxygen species revealed that two types of adsorbed oxygen species were present on Li/MgO; one (α-oxygen species) desorbed in proportion to the second order in the amount of the adsorbed species with an activation energy of 141 kJ mol-1, giving a peak (α-oxygen peak) at 673-693 K; the other (β-oxygen species) desorbed in proportion to the first order in the amount of the adsorbed species with an activation energy of 219 kJ mol-1, giving a peak (β-oxygen peak) at 753-768 K.A weak α-oxygen peak occurred on MgO and no β-oxygen peak was discerned.On Li/MgO, a β-oxygen peak appeared along with an α-oxygen peak.At higher Li-loadings the β-oxygen peak was more intense than the α-oxygen peak.The sites for these oxygen species were suggested to be derived by the addition of Li(I) on MgO.It was suggested that the α-oxygen species were present at the surface sites on higher index faces of MgO, whereas the β-oxygen species were present at oxygen vacancies in the vicinity of Li(I) substituting for Mg(II).The hydrolysis of these adsorbed oxygen species yielded an appreciable amount of H2O2, suggesting that these species were primarilly present as surface peroxide on MgO and Li/MgO.

A comparative XAS and X-ray diffraction study of new binuclear Mn(III) complexes with catalase activity. Indirect effect of the counteranion on magnetic properties

Fernandez, Gema,Corbella, Montserrat,Alfonso, Montserrat,Stoeckli-Evans, Helen,Castro, Isabel

, p. 6684 - 6698 (2004)

Four new binuclear Mn(III) complexes with carboxylate bridges have been synthesized: [{Mn(nn)(H2O)}2(μ-ClCH2-COO) 2(μ-O)](ClO4)2 with nn = bpy (1) or phen (2) and [{Mn(bpy)(H2O)}2(μ-RCOO)2(μ-O)] (NO3)2 with RCOO = ClCH2COO (3) or CH 3COO (4). The characterization by X-ray diffraction (1 and 3) and X-ray absorption spectroscopy (XAS) (1-4) displays the relevance of this spectroscopy to the elucidation of the structural environment of the manganese ions in this kind of compound. Magnetic susceptibility data show an antiferromagnetic coupling for all the compounds: J = -2.89 cm-1 (for 1), -8.16 cm-1 (for 2), -0.68 cm-1 (for 3), and -2.34 cm-1 (for 4). Compounds 1 and 3 have the same cation complex [{Mn(bpy)(H2O)}2(μ-ClCH2COO) 2(μ-O)]2+, but, while 1 shows an antiferromagnetic coupling, for 3 the magnetic interaction between Mn(III) ions is very weak. The four compounds show catalase activity, and when the reaction stopped, Mn(II) compounds with different nuclearity could be obtained: binuclear [{Mn(phen) 2}(μ-ClCH2COO)2](ClO4) 2, trinuclear [Mn3(bpy)2(μ-ClCH 2COO)6], or mononuclear complexes without carboxylate. Two Mn(II) compounds without carboxylate have been characterized by X-ray diffraction: [Mn(NO3)2(bpy)2][Mn(NO 3)(bpy)2(H2O)]NO3 (5) and [Mn(bpy)3](ClO4)2·0.5 C 6H4-1,2-(COOEt)2·O.5H2O (8).

Kinetics of N2O Decomposition on the Surface of γ-Al2O3 doped with Sodium Ions

Kordulis, Christos,Vordonis, Leonidas,Lycourghiotis, Alexis,Pomonis, Phillipos

, p. 627 - 634 (1987)

The kinetics of N2O decomposition on a series of specimens prepared by doping γ-Al2O3 with various amounts of Na+ ions has been studied at various temperatures using a flow-bed reactor working under atmospheric pressure.This doping promotes the adsorption of oxygen anions produced from surface decomposition, presumably via the formation of surface species +...O-...Na+>, bringing about a transformation of the rate equation from R=k into R=kbN2OPN2O/bO2P1/2O2 (where bN2O and bO2 are adsorption coefficients and PN2O and PO2 are partial pressures).Moreover, a decrease in catalytic activity, expressed either as fractional conversion or rate of reaction, was observed on increasing the surface coverage C, of γ-Al2O3 with Na+ ions determined by X-ray photoelectron spectroscopy.Specifically, the dependence of the catalytic activity on the surface coverage of γ-Al2O3 is described by the relationship 1n(1/R) = 15.4+(281/K)C (where K is a proportionality constant) and it was concluded that the deactivation observed is due to the promotion of the O2 adsorption caused by the Na+ ions.Finally, the linear dependence of the surface coverage of γ-Al2O3 on the sodium content strongly suggests that the dispersion of the sodium supported species is constant irrespective of the surface concentration of sodium.

Formation of the surface NO during N2O interaction at low temperature with iron-containing ZSM-5

Bulushev, Dmitri A.,Renken, Albert,Kiwi-Minsker, Lioubov

, p. 305 - 312 (2006)

Interaction of N2O at low temperatures (473-603 K) with Fe - ZSM-5 zeolites (Fe, 0.01-2.1 wt %) activated by steaming and/or thermal treatment in He at 1323 K was studied by the transient response method and temperature-programmed desorption (TPD). Diffuse reflectance infrared fourier transform spectroscopy (DRIFTS) of NO adsorbed at room temperature as a probe molecule indicated heterogeneity of surface Fe(II) sites. The most intensive bands were found at 1878 and 1891 cm-1, characteristic of two types mononitrosyl species assigned to Fe2+(NO) involved in bi- and oligonuclear species. Fast loading of atomic oxygen from N2O on the surface and slower formation of adsorbed NO species were observed. The initial rate of adsorbed NO formation was linearly dependent on the concentration of active Fe sites assigned to bi- and oligonuclear species, evolving oxygen in the TPD at around 630-670 K. The maximal coverage of a zeolite surface by NO was estimated from the TPD of .NO at ~700 K. This allowed the simulation of the dynamics of the adsorbed NO formation at 523 K, which was consistent with the experiments. The adsorbed NO facilitated the atomic oxygen recombination/desorption, the rate determining step during N2O decomposition to O2 and N2, taking place at temperatures ≥563 K.

The RuII(OH2)-RuIV(O) Couple in a Ruthenium Complex of 2-(Phenylazo)pyridine: Homogeneous Catalysis of the Oxidation of Water to Dioxygen

Goswami, Sreebrata,Chakravarty, Akhil R.,Chakravorty, Animesh

, p. 1288 - 1289 (1982)

In acidic solution II(OH2)(py)L2>2+ can be oxidised to IV(O)(py)L2>2+ in a single reversible step (E0298 = 1.20 V) and the oxidised complex catalyses the dehydrogenation of water to dioxygen in the presence of Ce4+ .

Photodecaging of a Mitochondria-Localized Iridium(III) Endoperoxide Complex for Two-Photon Photoactivated Therapy under Hypoxia

Chao, Hui,Gasser, Gilles,Ji, Liangnian,Karges, Johannes,Ke, Libing,Kuang, Shi,Liao, Xinxing,Wei, Fangmian,Xiong, Kai

supporting information, p. 4091 - 4101 (2022/03/03)

Despite the clinical success of photodynamic therapy (PDT), the application of this medical technique is intrinsically limited by the low oxygen concentrations found in cancer tumors, hampering the production of therapeutically necessary singlet oxygen (1O2). To overcome this limitation, we report on a novel mitochondria-localized iridium(III) endoperoxide prodrug (2-O-IrAn), which, upon two-photon irradiation in NIR, synergistically releases a highly cytotoxic iridium(III) complex (2-IrAn), singlet oxygen, and an alkoxy radical. 2-O-IrAn was found to be highly (photo-)toxic in hypoxic tumor cells and multicellular tumor spheroids (MCTS) in the nanomolar range. To provide cancer selectivity and improve the pharmacological properties of 2-O-IrAn, it was encapsulated into a biotin-functionalized polymer. The generated nanoparticles were found to nearly fully eradicate the tumor inside a mouse model within a single treatment. This study presents, to the best of our knowledge, the first example of an iridium(III)-based endoperoxide prodrug for synergistic photodynamic therapy/photoactivated chemotherapy, opening up new avenues for the treatment of hypoxic tumors.

Pt-core silica shell nanostructure: a robust catalyst for the highly corrosive sulfuric acid decomposition reaction in sulfur iodine cycle to produce hydrogen

Khan, Hassnain Abbas,Jung, Kwang-Deog,Ahamad, Tansir,Ubaidullah, Mohd,Imran, Muhammad,Alshehri, Saad M.

, p. 1247 - 1252 (2021/02/03)

The platinum core silica shell catalyst has facilitated stable sulfuric acid decomposition at higherature which was not possible over bare Pt nanoparticles due to sintering and agglomeration. Helium (He) gas supplies the heat (550-900 °C) in a high temperature gas cooled reactor (VHTR). The major challenge is designing a stable catalyst for the variable heat efficiency of He. Pt catalysts loaded on different supports, such as SiC, Al2O3, SiC-Al2O3, BaSO4, TiO2, SBA-15, and SiO2, have been extensively studied but they have not provided a simple method to form robust catalysts for sulfuric acid decomposition. The core-shell scheme, whereby nanoparticles are enclosed by protecting agents (CTAB) and are covered by a silica shell, delivered mesopores and exhibited higher activity and stability over testing for more than 100 h. TEM images confirmed that the Pt particles on the Pt@mSiO2 catalyst are more stable during sulfuric acid decomposition, and no significant evidence of agglomeration or sintering of the Pt core particles was found, despite some broken shells and dislocated Pt nanoparticles from the silica core. ICP-OES analysis of the spent catalysts after 100 h showed minimal Pt loss (9.0%). These types of catalysts are highly desirable for practical applications. This journal is

Electrocatalytic Water Oxidation with α-[Fe(mcp)(OTf)2] and Analogues

D'Agostini, Silvia,Kottrup, Konstantin G.,Casadevall, Carla,Gamba, Ilaria,Dantignana, Valeria,Bucci, Alberto,Costas, Miquel,Lloret-Fillol, Julio,Hetterscheid, Dennis G.H.

, p. 2583 - 2595 (2021/03/03)

The complex α-[Fe(mcp)(OTf)2] (mcp = N,N′-dimethyl-N,N′-bis(pyridin-2-ylmethyl)-cyclohexane-1,2-diamine and OTf = trifluoromethanesulfonate anion) was reported in 2011 by some of us as an active water oxidation (WO) catalyst in the presence of sacrificial oxidants. However, because chemical oxidants are likely to take part in the reaction mechanism, mechanistic electrochemical studies are critical in establishing to what extent previous studies with sacrificial reagents have actually been meaningful. In this study, the complex α-[Fe(mcp)(OTf)2] and its analogues were investigated electrochemically under both acidic and neutral conditions. All the systems under investigation proved to be electrochemically active toward the WO reaction, with no major differences in activity despite the structural changes. Our findings show that WO-catalyzed by mcp-iron complexes proceeds via homogeneous species, whereas the analogous manganese complex forms a heterogeneous deposit on the electrode surface. Mechanistic studies show that the reaction proceeds with a different rate-determining step (rds) than what was previously proposed in the presence of chemical oxidants. Moreover, the different kinetic isotope effect (KIE) values obtained electrochemically at pH 7 (KIE ~10) and at pH 1 (KIE = 1) show that the reaction conditions have a remarkable effect on the rds and on the mechanism. We suggest a proton-coupled electron transfer (PCET) as the rds under neutral conditions, whereas at pH 1 the rds is most likely an electron transfer (ET).

Effects of SiO2-based scaffolds in TiO2 photocatalyzed CO2 reduction

Cruciani, Giuseppe,Di Michele, Alessandro,Forghieri, Giulia,Ghedini, Elena,Menegazzo, Federica,Signoretto, Michela,Tieuli, Sebastiano,Zanardo, Danny

, (2021/08/18)

CO2 photoreduction has claimed as appealing process to upgrade a waste gas into valuable fuels or chemicals. Titanium dioxide (TiO2) is one of the most popular material used as catalyst for this reaction, having however a poor activity. The utilization of transparent, insulating and highly porous scaffolds to support a photoactive phase has been reported as one of the possible strategies to improve the performances of this material. In this work, two silica-based materials with different porosity type and level, were involved as support for the TiO2 and assessed in the gas-phase CO2 photoreduction with H2O. The morphological, structural and surface properties were then evaluated by means of different characterization techniques, aiming to correlate them with the catalytic activity and selectivity. The TiO2-SiO2 composites revealed a comparable activity compared to pure TiO2, despite the low fraction of photoactive phase due to improved light harvesting and reagents adsorption on the composites. The CO2 capture/photoconverting ability was evaluated, to explore the potentiality as multifunctional material.

The tin sulfates Sn(SO4)2and Sn2(SO4)3: Crystal structures, optical and thermal properties

Daub, Michael,H?mmer, Matthias,H?ppe, Henning A.,Hillebrecht, Harald,Klenner, Steffen,Netzsch, Philip,Neuschulz, Kai,P?ttgen, Rainer,Struckmann, Mona,Wickleder, Mathias S.

, p. 12913 - 12922 (2021/10/12)

We report the crystal structures of two tin(iv) sulfate polymorphs Sn(SO4)2-I (P21/c (no. 14), a = 504.34(3), b = 1065.43(6), c = 1065.47(6) pm, β = 91.991(2)°, 4617 independent reflections, 104 refined parameters, wR2 = 0.096) and Sn(SO4)2-II (P21/n (no. 14), a = 753.90(3), b = 802.39(3), c = 914.47(3) pm, β = 92.496(2)°, 3970 independent reflections, 101 refined parameters, wR2 = 0.033). Moreover, the first heterovalent tin sulfate Sn2(SO4)3 is reported which adopts space group P1 (no. 2) (a = 483.78(9), b = 809.9(2), c = 1210.7(2) pm, α = 89.007(7)°, β = 86.381(7)°, γ = 73.344(7)°, 1602 independent reflections, 152 refined parameters, wR2 = 0.059). Finally, SnSO4-the only tin sulfate with known crystal structure-was revised and information complemented. The optical and thermal properties of all tin sulfates are investigated by FTIR, UV-vis, luminescence and 119Sn M?ssbauer spectroscopy as well as thermogravimetry and compared.

Process route upstream and downstream products

Process route

methanol
67-56-1

methanol

ethane
74-84-0

ethane

carbon dioxide
124-38-9,18923-20-1

carbon dioxide

carbon monoxide
201230-82-2

carbon monoxide

hydrogen
1333-74-0

hydrogen

oxygen
80937-33-3

oxygen

Conditions
Conditions Yield
at 450 ℃; for 0.0125h; under 1800.18 Torr;
europium(III) oxide

europium(III) oxide

chlorine
7782-50-5

chlorine

oxygen
80937-33-3

oxygen

europium(III) chloride
10025-76-0

europium(III) chloride

Conditions
Conditions Yield
at 550°C, in presence of CO;
iron(III) oxide

iron(III) oxide

iron(II) oxide
1345-25-1

iron(II) oxide

oxygen
80937-33-3

oxygen

Conditions
Conditions Yield
dissocn. of Fe2O3 in glass to O2 and FeO about 1300°C;;
decompn. of Fe2O3 to FeO and oxygen;;
dissocn. of Fe2O3 in glass to O2 and FeO about 1300°C;;
decompn. of Fe2O3 to FeO and oxygen;;
gold oxide

gold oxide

oxygen
80937-33-3

oxygen

Conditions
Conditions Yield
In neat (no solvent); reaction at heating in a CO2 stream;;
In neat (no solvent); reaction at heating in a CO2 stream;;
cobalt(III) oxide

cobalt(III) oxide

oxygen
80937-33-3

oxygen

Conditions
Conditions Yield
In neat (no solvent); reaction by heating in a CO2 stream at beginning red heat;;
In neat (no solvent); reaction by heating in a CO2 stream at beginning red heat;;
indium(III) oxide

indium(III) oxide

chlorine
7782-50-5

chlorine

(indium trichloride)2

(indium trichloride)2

oxygen
80937-33-3

oxygen

indium(III) chloride
10025-82-8

indium(III) chloride

Conditions
Conditions Yield
Cl2/Ar mixt. flowing over In2O3 (const. temp. in range 500-700°C,gas flow rate 2ml/min, complete satn. of carrier gas by vapours of gase ous products, duration 3 h); monitoring by gravimetric and chem. anal.;
neodymium(III) oxide

neodymium(III) oxide

chlorine
7782-50-5

chlorine

oxygen
80937-33-3

oxygen

neodymium trichloride
10024-93-8

neodymium trichloride

Conditions
Conditions Yield
In neat (no solvent); equilibrium at 200 - 300°C;; Kinetics;
at 400°C, equilibrium reaction;
dipotassium peroxodisulfate

dipotassium peroxodisulfate

sulfuric acid
7664-93-9

sulfuric acid

water
7732-18-5

water

potassium hydrogensulfate
7646-93-7

potassium hydrogensulfate

dihydrogen peroxide
7722-84-1

dihydrogen peroxide

oxygen
80937-33-3

oxygen

Conditions
Conditions Yield
In water; investigations within the system K2S2O8-H2SO4-H2O at 100 °C, formation of O3 at higher concentrations of H2SO4, mechanism discussed;;
Conditions
Conditions Yield
In gas; heating;
water
7732-18-5

water

hydrogen
1333-74-0

hydrogen

dihydrogen peroxide
7722-84-1

dihydrogen peroxide

oxygen
80937-33-3

oxygen

Conditions
Conditions Yield
With Ar or Kr or Xe; In water; Sonication; Ar or Kr or Xe saturated water was sonicated (200 kHz, 200 W) for 10 min. at 7 °C.; not isolated; Kinetics;
In neat (no solvent); Sonication; under Ar; detected by gas chromy. and spectrophotometry; Kinetics;
In neat (no solvent); Sonication; under Ar; detected by gas chromy. and spectrophotometry; Kinetics;
With catalyst: NaTaO3#dotLa/Au or NaTaO3#dotLa/ITO; In water; Electrochem. Process; in three-electrode quartz cell with Pt counter electrode and satd. Ag/AgCl ref. electrode; 0.1 M K2SO4 (pH = 6.4) as electrolyte; 500 W Hg lamp as light source; electrolyte was satd. with N2, O2 or H2; detd. voltammetrically;
With catalyst: NaTaO3/Au or NaTaO3/ITO; In water; Electrochem. Process; in three-electrode quartz cell with Pt counter electrode and satd. Ag/AgCl ref. electrode; 0.1 M K2SO4 (pH = 6.4) as electrolyte; 500 W Hg lamp as light source; electrolyte was satd. with N2, O2 or H2; detd. voltammetrically;
With catalyst: TiO2/Au or TiO2/ITO or TiO2/Ti; In water; Electrochem. Process; in three-electrode quartz cell with Pt counter electrode and satd. Ag/AgCl ref. electrode; 0.1 M K2SO4 (pH = 6.4) as electrolyte; 500 W Hg lamp as light source; electrolyte was satd. with N2, O2 or H2; detd. voltammetrically;
With PuO2; In neat (no solvent); other Radiation; radiolysis on PuO2; Kinetics;

Global suppliers and manufacturers

Global( 0) Suppliers
  • Company Name
  • Business Type
  • Contact Tel
  • Emails
  • Main Products
  • Country
close
Post a RFQ

Enter 15 to 2000 letters.Word count: 0 letters

Attach files(File Format: Jpeg, Jpg, Gif, Png, PDF, PPT, Zip, Rar,Word or Excel Maximum File Size: 3MB)

1

What can I do for you?
Get Best Price

Get Best Price for 80937-33-3
Post Buying Request Now
close
Remarks: The blank with*must be completed