10024-97-2

Basic information

• Product Name: NITROUS OXIDE
• Synonyms: hyponitrousacidanhydride;Lachgas;n20;N2O;Nitral;Nitrogen oxide (N2O);nitrogenhypoxide;nitrogenoxide(n2o)
• CAS NO: 10024-97-2
• Molecular Formula: N₂O
• Molecular Weight: 44.01
• EINECS: 233-032-0
• Product Categories: refrigerants;Inorganics
• Mol File: 10024-97-2.mol
• Article Data: 548

Chemical Properties

• Melting Point: −91 °C(lit.)
• Boiling Point: −88 °C(lit.)
• Appearance: /colorless gas
• Density: 1.23 g/cm3 (-89 ºC)
• Vapor Density: 1.53 (15 °C, vs air)
• Vapor Pressure: 51.7 mm Hg ( 21 °C)
• Refractive Index: 1.380
• Solubility: At 20 °C and at a pressure of 101 kPa, 1 volume dissolves in about 1.5 volumes of water.
• PKA: -16.68±0.53(Predicted)
• Water Solubility: 670,000 mg l-1
• Stability: Oxidant, strongly supports combustion. May react violently with some materials. Thermal decomposition yields toxic products. Inc
• Merck: 13,6687
• BRN: 8137358
• CAS DataBase Reference: NITROUS OXIDE(CAS DataBase Reference)
• NIST Chemistry Reference: NITROUS OXIDE(10024-97-2)
• EPA Substance Registry System: NITROUS OXIDE(10024-97-2)

Safety Data

• Hazard Codes: O
• Statements: 8
• Safety Statements: 38
• RIDADR: UN 1070 2.2
• WGK Germany: 1
• RTECS: QX1350000
• F: 4.5-31
• HazardClass: 2.2
• Hazardous Substances Data: 10024-97-2(Hazardous Substances Data)

Usage

Description

dinitrogen monoxide’s (N2O) common name is nitrous oxide.Nitrous oxide is a colorless, nonfl ammable, nontoxic gas with a slightly sweet odor and taste. Nitrous oxide is produced by the thermal decomposition of ammonium nitrate at approximately 240°C: NH4NO3(g) → N2O(g) + 2H2O(g).Nitrous oxide is an important greenhouse gas. Its atmospheric residence time is 120 years. A molecule of N2O has 310 times the potential for absorbing heat compared to a molecule of CO2. Nitrous oxide is stable and unreactive on the earth’s surface, but it can be transported to the stratosphere where it absorbs energy and is converted into reactive forms of nitrogen such as nitric oxide and the nitrate radical contributing to ozone destruction.

Chemical Properties

Different sources of media describe the Chemical Properties of 10024-97-2 differently. You can refer to the following data:
1. A colorless gas without appreciable odor or a slightly sweetish odor and taste. One L at 0°C and at a pressure of 760 mm of mercury weighs about 1.97 g. One volume dissolves in about 1.4 volumes of water at 20°C and at a pressure of 760 mm of mercury. It is freely soluble in alcohol and soluble in ether and in oils. It is prepared by thermal decomposition of ammonium nitrate.
2. Colourless gas with sweetish odour
3. Nitrous oxide is a colorless gas. Slightly sweet odor. Shipped as a liquefied compressed gas.
4. Nitrous oxide is a nonflammable, colorless and odorless, sweettasting gas. It is usually handled as a compressed gas, stored in metal cylinders.
5. Nitrous oxide has a slight sweetish, odor and taste. This gas is also reported as without appreciable odor. At 0°C and a pressure of 760 mm of mercury, 1 L weighs about 1.97 g.

Physical properties

Colorless gas with faint sweet odor and taste; heavier than air, density in air 1.53 (air=1); gas density 1.977 g/L at 0°C; noncombustible gas; supports combustion; liquefies to a colorless liquid at -88.5°C; liquid density 1.226 g/mL at -89°C; freezes to a cubic crystalline solid at -90.8°C; dipole moment 0.166 ; critical temperature 36.5°C; critical pressure 71.7 atm; solubility in water: 130 mL gas dissolves in 100mL water at 0°C and 56.7 mL in 100 mL water at 25°C; soluble in alcohol, ether and sulfuric acid.

History

nitrous oxide was prepared in 1772 by Joseph Priestley (1733 1804) . Priestley called nitric oxide nitrous air, nitrogen dioxide nitrous acid vapor, and nitrous oxide phlogisticated nitrous air, but also referred to the dioxide. Priestley prepared nitric oxide by reacting nitric acid with a metal such as copper: 3Cu(s) + 8HNO3(aq) 2NO(g) + 3Cu(NO3)2(aq) + 4H2O(l).He prepared nitrous oxide by reducing nitric oxide using iron: 2NO(g) + H2O(l) + Fe(s) N2O(g) + Fe(OH)2(aq).For example, the year of discovery for nitrous oxide ranges between 1772 and 1793. Humphrey Davy (1778 1829) examined the physiological effects of nitrous oxide and in 1799 wrote Researches Chemical and Philosophical, Chiefly Concerning Nitrous Oxide.

Uses

Different sources of media describe the Uses of 10024-97-2 differently. You can refer to the following data:
1. Nitrous oxide is called laughing gas and has been used as a recreational inhalant, anesthetic, oxidizer, and propellant. Nitrous oxide is widely used as an anesthetic in dental surgery, which accounts for approximately 90% of its use. It is used by the dairy industry as a foaming agent for canned whipping creams. The gas is used as an anesthetic, especially in dentistry and minor surgery. It produces mild hysteria and laughter preceding the anesthetic effect, for which reason it also is called “laughing gas.” It is used as an aerosol propellant, an aerating agent for whipped cream, and an oxidizing agent at high temperatures. Nitrous oxide also is used in the preparation of nitrites and as a flame gas in flame atomic absorption spectrometry of metals.
2. Nitrous oxide is used in the productionof nitrites, in rocket fuel, as an inhalationanesthesia and analgesic agent.
3. Nitrous Oxide is a noncombustible gas used as a propellant in certain dairy and vegetable fat whipped toppings contained in pressurized containers.
4. Nitrous oxide was discovered by Priestley. It is found in the atmosphere in trace concentrations. The gas is used as an anesthetic, especially in dentistry and minor surgery. It produces mild hysteria and laughter preceding the anesthetic effect, for which reason it also is called “laughing gas.” It is used as an aerosol propellant, an aerating agent for whipped cream, and an oxidizing agent at high temperatures. Nitrous oxide also is used in the preparation of nitrites and as a flame gas in flame atomic absorption spectrometry of metals.
5. Nitrous oxide is still commonly used in combination with a volatile agent to maintain anaesthesia. However, there is growing concern regarding its toxic effects and cost. Consequently, medical air in combination with oxygen is now being used increasingly during anaesthesia.

Preparation

Prepared by thermal decomposition of ammonium nitrate NH4NO3 → N2O↑ + 2H2O

Definition

Different sources of media describe the Definition of 10024-97-2 differently. You can refer to the following data:
1. ChEBI: A nitrogen oxide consisting of linear unsymmetrical molecules with formula N2O. While it is the most used gaseous anaesthetic in the world, its major commercial use, due to its solubility under pressure in vegetable fats combined with ts non-toxicity in low concentrations, is as an aerosol spray propellant and aerating agent for canisters of 'whipped' cream.
2. A colorless gas with a faintly sweet odor and taste. It is appreciably soluble in water (1.3 volumes in 1 volume of water at 0°C) but more soluble in ethanol. It is prepared commercially by the careful heating of ammonium nitrate: NH4NO3(s) = N2O(g) + 2H2O(g) Dinitrogen oxide is fairly easily decomposed on heating to temperatures above 520°C, giving nitrogen and oxygen. The gas is used as a mild anesthetic in medicine and dentistry, being marketed in small steel cylinders. It is sometimes called laughing gas because it induces a feeling of elation when inhaled.

Production Methods

Different sources of media describe the Production Methods of 10024-97-2 differently. You can refer to the following data:
1. Prepared (1) by reaction of silver hyponitrite Ag2N2O2 and hydrogen chloride in anhydrous ether, an evaporation of the resulting solution, (2) by reaction of hydroxylamine H2NOH plus nitrous acid HONO.
2. Nitrous oxide is prepared by heating ammonium nitrate to about 170°C. This reaction also forms water.

Biological Functions

N2O (commonly called laughing gas) produces its anesthetic effect without decreasing blood pressure or cardiac output. Although it directly depresses the myocardium, cardiac depression is offset by an N2O– mediated sympathetic stimulation. Likewise, respiration is maintained.Tidal volume falls, but minute ventilation is supported by a centrally mediated increase in respiratory rate. However, since the respiratory depressant effect of N2O are synergistic with drugs such as the opioids opioids and benzodiazepines, N2O should not be considered benign. Deep levels of anesthesia are unattainable, even when using the highest practical concentrations of N2O (N2O 60–80% with oxygen 40–20%). Although unconsciousness occurs at these inspired levels, patients exhibit signs of CNS excitation, such as physical struggling and vomiting. If the airway is unprotected, vomiting may lead to aspiration pneumonitis, since the protective reflexes of the airway are depressed. On the other hand, lower inspired concentrations (25–40%) of N2O produce CNS depression without excitatory phenomena and are more safely used clinically. CNS properties of low inspired tension of N2O include periods of waxing and waning consciousness, amnesia, and extraordinarily effective analgesia. N2O 25% produces the gas’s maximum analgesic effect.With this concentration, responses to painful surgical manipulations are blocked as effectively as they would be with a therapeutic dose of morphine. Such low inspired concentrations of N2O are used in dentistry and occasionally for selected painful surgical procedures (i.e., to relieve the pain of labor). Since the tissue solubility of N2O is low, the CNS effects are rapid in onset, and recovery is prompt when the patient is returned to room air or oxygen. The most common use of N2O is in combination with the more potent volatile anesthetics. It decreases the dosage requirement for the other anesthetics, thus lowering their cardiovascular and respiratory toxicities. For example, an appropriate anesthetic maintenance tension for N2O and halothane would be N2O 40% and halothane 0.5%.With this combination in a healthy patient, anesthesia is adequate for major surgery, and the dose-dependent cardiac effects of halothane are reduced.

General Description

Different sources of media describe the General Description of 10024-97-2 differently. You can refer to the following data:
1. Nitrous oxide is a gas at room temperature and is supplied asa liquid under pressure in metal cylinders. Nitrous oxide is a“dissociative anesthetic” and causes slight euphoria and hallucinations.
2. NITROUS OXIDE is a colorless, sweet-tasting gas. NITROUS OXIDE is also known as "laughing gas". Continued breathing of the vapors may impair the decision making process. NITROUS OXIDE is noncombustible but NITROUS OXIDE will accelerate the burning of combustible material in a fire. NITROUS OXIDE is soluble in water. Its vapors are heavier than air. Exposure of the container to prolonged heat or fire can cause NITROUS OXIDE to rupture violently and rocket. NITROUS OXIDE is used as an anesthetic, in pressure packaging, and to manufacture other chemicals.

Reactivity Profile

NITROUS OXIDE is an oxidizing agent. Nonflammable but supports combustion. Can explode at high temperature (after vaporization). Vapors can undergo a violent reaction with aluminum, boron, hydrazine, lithium hydride, phenyllithium, phosphine, sodium, tungsten carbide [Bretherick, 5th ed., 1995, p. 1686]. Contact of the cold liquefied gas with water may result in vigorous or violent boiling. If the water is hot, a liquid "superheat" explosion may occur. Pressures may build to dangerous levels if liquefied gas contacts water in a closed container [Handling Chemicals Safely 1980].

Hazard

Supports combustion, can form explosive mixture with air. Narcotic in high concentration. Central nervous system impairment, hematologic effects, and embryo/fetal damage. Questionable carcinogen.

Health Hazard

Different sources of media describe the Health Hazard of 10024-97-2 differently. You can refer to the following data:
1. Inhalation causes intense analgesia; concentrations of over 40-60% cause loss of consciousness preceded by hysteria. Contact of liquid with eyes or skin causes frostbite burn.
2. Toxicity and irritant effects of nitrous oxidein humans are very low. It is an anesthetic.Inhalation of this gas at high concentrationscan produce depression of the central nervous system, decrease in body temperature,and fall in blood pressure. The LC50 valueof a 4-hour exposure in mice is in the rangeof 600 ppm.

Fire Hazard

Behavior in Fire: Will support combustion, and may increase intensity of fire. Containers may explode when heated.

Pharmaceutical Applications

Nitrous oxide and other compressed gases such as carbon dioxide and nitrogen are used as propellants for topical pharmaceutical aerosols. They are also used in other aerosol products that work satisfactorily with the coarse aerosol spray that is produced with compressed gases, e.g. furniture polish and window cleaner. The advantages of compressed gases as aerosol propellants are that they are less expensive, of low toxicity, and practically odorless and tasteless. In contrast to liquefied gases, their pressures change relatively little with temperature. However, there is no reservoir of propellant in the aerosol, and as a result the pressure decreases as the product is used, changing the spray characteristics. Misuse of a product by the consumer, such as using a product inverted, results in the discharge of the vapor phase instead of the liquid phase. Since most of the propellant is contained in the vapor phase, some of the propellant will be lost and the spray characteristics will be altered. Additionally, the sprays produced using compressed gases are very wet. However, recent developments in valve technology have reduced the risk of misuse by making available valves which will spray only the product (not propellant) regardless of the position of the container. Additionally, barrier systems will also prevent loss of propellant, and have found increased use with this propellant. Therapeutically, nitrous oxide is best known as an anesthetic administered by inhalation. When used as an anesthetic it has strong analgesic properties but produces little muscle relaxation. Nitrous oxide is always administered in conjunction with oxygen since on its own it is hypoxic.

Materials Uses

Nitrous oxide is noncorrosive and may therefore be used with any of the common, commercially available metals. Because of its oxidizing action, however, all equipment being prepared to handle nitrous oxide, particularly at high pressures, must be free of oil, grease, and other readily combustible materials. Nitrous oxide may cause swelling ofsome elastomers.

Clinical Use

The low potency of nitrous oxide (MAC＝ 104%) precludes it from being used alone for surgical anesthesia.To use it as the sole anesthetic agent the patient wouldhave to breathe in pure N2Oto the exclusion of oxygen. Thissituation would obviously cause hypoxia and potentially leadto death. Nitrous oxide can inactivate methionine synthase, aB12-dependent enzyme necessary for the synthesis of DNAand therefore should be used with caution in pregnant andB12-deficient patients. Nitrous oxide is also soluble in closedgas containing body spaces and can cause these spaces toenlarge when administered possibly leading to adverse occurrences(occluded middle ear, bowel distension, pneumothorax).Nitrous oxide is a popular anesthetic in dentistrywere it is commonly referred to as “laughing gas.” It is usedin combination with more potent anesthetics for surgicalanesthesia and remains a drug of recreational abuse.Nitrous oxide undergoes little or no metabolism.

Safety Profile

Moderately toxic by inhalation. Human systemic effects by inhalation: general anesthetic, decreased pulse rate without blood pressure fall, and body temperature decrease. An experimental teratogen. Experimental reproductive effects. Mutation data reported. An asphyxiant. Does not burn but is flammable by chemical reaction and supports combustion. Moderate explosion hazard; it can form an explosive mixture with air. Violent reaction with Al, B, hydrazine, LiH, LiC6H5, PH3, Na, tungsten carbide. Also self-explodes at high temperatures.

Safety

Nitrous oxide is most commonly used therapeutically as an anesthetic and analgesic. Reports of adverse reactions to nitrous oxide therefore generally concern its therapeutic use, where relatively large quantities of the gas may be inhaled, rather than its use as an excipient. The main complications associated with nitrous oxide inhalation occur as a result of hypoxia. Prolonged administration may also be harmful. Nitrous oxide is rapidly absorbed on inhalation.

Potential Exposure

Used as an anesthetic in dentistry and surgery; used as a gas in food aerosols, such as whipped cream; used in manufacture of nitrites; used in rocket fuels; in firefighting; diesel emissions. Large amounts of nitrous oxide will decrease the amount of available oxygen. Nitrous Oxide 2231 Oxygen should be routinely tested to ensure that it is at least 19% by volume.

Physiological effects

Nitrous oxide's primary physiological effect is central nervous system (CNS) depression. At high concentrations, anesthetic levels can be obtained, but the low potency of nitrous oxide necessitates concomitant administration of other depressant drugs. Nitrous oxide has been associated with several side effects from longterm exposure. The most strongly substantiated effect is neuropathy. Epidemiological studies also suggest feto-toxic effects and higher incidents of spontaneous abortion in exposed personnel.Although no cause-and-effect relationship has been firmly established, exposure to the gas should be minimized. Inhalation of nitrous oxide without the provision of a sufficient oxygen supply may be fatal or cause brain damage. Due to the concern over longterm exposure effects, release of the product into general work areas should be minimized. NIOSH has recommended a maximum exposure on an 8-hour Time-Weighted Average (TWA) of 25 parts per million for anesthetic and analgesic administration. ACGIH recommends a Threshold Limit Value-Time-Weighted Average (TLV-TWA) of 50 ppm (90 mglm3) for nitrous oxide. The TLV- TWA is the time-weighted average concentration for a normal 8-hour workday and a 40-hour workweek, to which nearly all workers may be repeatedly exposed, day after day, without adverse effect. Warning: The misuse of nitrous oxide can cause death by reducing the oxygen necessary to support life. Nitrous oxide abuse can impair an individual's ability to make and implement lifesustaining decisions.

Carcinogenicity

The possible carcinogenicity of nitrous oxide has been studied in dentists and chairside assistants with occupational exposures. No effect was observed in male dentists, but a 2.4- fold increase in cancer of the cervix in heavily exposed female assistants was reported.7 Other epidemiological reports of workers exposed to waste anesthetic gases have been negative.1 Carcinogenic bioassays in animals have yielded negative results. Nitrous oxide was not genotoxic in a variety of assays.

storage

Nitrous oxide is essentially nonreactive and stable except at high temperatures; at a temperature greater than 500°C nitrous oxide decomposes to nitrogen and oxygen. Explosive mixtures may be formed with other gases such as ammonia, hydrogen, and other fuels. Nitrous oxide should be stored in a tightly sealed metal cylinder in a cool, dry place.

Shipping

UN1070 Nitrous oxide, compressed, Hazard Class: 2.2; Labels: 2.2-Nonflammable compressed gas; 5.1-Oxidizer; UN2201 Nitrous oxide, refrigerated liquid, Hazard Class: 2.2; Labels: 2.2-Nonflammable compressed gas; 5.1-Oxidizer. Cylinders must be transported in a secure upright position, in a well-ventilated truck. Protect cylinder and labels from physical damage. The owner of the compressed gas cylinder is the only entity allowed by federal law (49CFR) to transport and refill them. It is a violation of transportation regulations to refill compressed gas cylinders without the express written permission of the owner.

Purification Methods

Wash the gas with concentrated alkaline pyrogallol solution, to remove O2, CO2, and NO2, then dry it by passing it through columns of P2O5 or Drierite, and collecting in a dry trap cooled in liquid N2. It is further purified by freeze-pump-thaw and distillation cycles under vacuum [Ryan & Freeman J Phys Chem 81 1455 1977, Schenk in Handbook of Preparative Inorganic Chemistry (Ed. Brauer) Academic Press Vol I pp 484-485 1963].

Toxicity evaluation

Large amounts of released nitrous oxide can decrease the amount of available oxygen. Medical complications of nitrous oxide inhalation are due to varying degrees of hypoxia affecting primarily the heart and brain. By inactivating vitamin B12, a critical cofactor in hematopoiesis and lipid membrane formation, nitrous oxide can cause anemia and neuropathy via selective inhibition of methionine synthase, a key enzyme in methionine and folate metabolism.

Incompatibilities

Different sources of media describe the Incompatibilities of 10024-97-2 differently. You can refer to the following data:
1. Nitrous oxide is generally compatible with most materials encountered in pharmaceutical formulations, although it may react as a mild oxidizing agent.
2. Nitrous oxide is a weak oxidizer. Incompatible with oxidizers (chlorates, nitrates, peroxides, permanganates, perchlorates, chlorine, bromine, fluorine, etc.); contact may cause fires or explosions. Keep away from alkaline materials, strong bases, strong acids, oxoacids, epoxides. Violent reactions with organic peroxides, hydrazine, hydrogen, hydrogen sulfide; lithium, boron, lithium hydride, sodium, aluminum, phosphine. This chemical is a strong oxidizer @ .300C and self-explodes at high temperature. May form explosive mixtures with ammonia, carbon monoxide; hydrogen sulfide; oil, grease and fuels.

Waste Disposal

Disperse in atmosphere or spray on dry soda ash/lime with great care; then flush to sewer.

Regulatory Status

GRAS listed. Accepted for use as a food additive in Europe. Included in nonparenteral medicines licensed in the UK and USA. Included in the Canadian List of Acceptable Non-medicinal Ingredients.

GRADES AVAILABLE

Nitrous oxide is available in medical, commercial, and high-purity grades. The medical (USP) grade is the most widely used. Manufacturers typically produce nitrous oxide for this use to the specification published in the United States Pharmacopeia/National Formulary. CGA G-8.2, Commodity Specification for Nitrous Oxide, describes the requirements for particular grades of nitrous oxide. Other specifications to meet particular requirements are available from suppliers. The absence of a value in a listed quality verification level does not mean to imply that the limiting characteristic is or is not present, but merely indicates that the test is not required for compliance with the specification.

InChI:InChI=1/N2O/c1-2-3

Synthetic route

ammonia (7664-41-7) + oxygen (80937-33-3) → nitrogen (7727-37-9) + nitrogen(II) oxide (10102-43-9) + dinitrogen monoxide (10024-97-2)

Conditions	Yield
With oxygen In neat (no solvent) Fe-ZSM-5 catalyst prepared by ion exchange and heat-treated at 400, 425or 450 °C, 100 % NH3 conversion, 100 % N2 selectivity, 1000 ppm NH3 in 2 % O2-contg. He;	A 100% B 0% C 0%
With catalyst:Fe-mordenite In neat (no solvent) Fe-mordenite catalyst prepared by ion exchange and heat-treated at 425 °C, 92 % NH3 conversion, 99 % N2 selectivity, 1000 ppm NH3 in 2 %O2-contg. He;	A 92% B n/a C 0%
With catalyst:Fe-ZSM-5 In neat (no solvent) Fe-ZSM-5 catalyst prepared by ion exchange and heat-treated at 375 °C, 90 % NH3 conversion, 99 % N2 selectivity, 1000 ppm NH3 in 2 % O2-contg. He;	A 90% B n/a C 0%

[Fe2(2,6-bis[[bis(2-pyridylmethyl)amino]methyl]-4-methylphenolato)(propionato)(NO)2](triflate)2 → dinitrogen monoxide (10024-97-2)

Conditions	Yield
With cobaltocene In dichloromethane at 20℃; for 0.0166667h; Kinetics; Time; Temperature; Concentration;	100%

ammonia (7664-41-7) → nitrogen (7727-37-9) + nitrogen(II) oxide (10102-43-9) + dinitrogen monoxide (10024-97-2)

Conditions	Yield
With oxygen In neat (no solvent) Fe-mordenite catalyst prepared by ion exchange and heat-treated at 450 °C, 99 % NH3 conversion, 100 % N2 selectivity, 1000 ppm NH3 in 2 % O2-contg. He;	A 99% B 0% C 0%
With oxygen; platinum high excess O2,500 °C;	A <1 B n/a C n/a
With oxygen; platinum at 300 °C;	A n/a B <9 C n/a

[CuI(tris(2-pyridylmethyl)amine)(CH3CN)]2+ (114581-86-1) + nitrogen(II) oxide (10102-43-9) → [Cu(tris(2-pyridylmethyl)amine)(H2O)](2+) (133578-96-8) + dinitrogen monoxide (10024-97-2)

Conditions	Yield
In water room temp., pH = 7.0; reaction followed by gas chromy.;	A 99% B n/a

ammonium nitrate → nitrogen (7727-37-9) + nitrogen(II) oxide (10102-43-9) + Nitrogen dioxide (10102-44-0) + dinitrogen monoxide (10024-97-2)

Conditions	Yield
at 220-260°C, nearly 98% N2O, 2% N2; troces of NO and NO2 (0.001%);	A 2% B n/a C n/a D 98%

trifluoromethyldifluorophosphine (1112-04-5) + nitrogen(II) oxide (10102-43-9) → Trifluormethylphosphonsaeuredifluorid (19162-94-8) + dinitrogen monoxide (10024-97-2)

Conditions	Yield
20°C (7 d); oxydation;	A 98% B n/a

[(copper(II)(tris(2-pyridylmethyl)amine))2(μ-hyponitrite)](2+) + nitrogen(II) oxide (10102-43-9) → [copper(I)(tris(2-pyridylmethyl)amine)](1+) (188637-84-5) + [copper(II)(tris(2-pyridylmethyl)amine)(nitrito)](1+) + dinitrogen monoxide (10024-97-2)

Conditions	Yield
In tetrahydrofuran; methanol for 8h; Solvent; Inert atmosphere; Schlenk technique;	A 96% B 85% C 98%

{Cu2(NO)N6OC36H39}(2+) + tetrabutylammonium nitrite → {Cu2(O)N6OC36H39}(1+)*PF6(1-)={Cu2(O)N6OC36H39}PF6 + dinitrogen monoxide (10024-97-2)

Conditions	Yield
With P(C6H5)3 In not given byproducts: OP(C6H5)3; react. of 1 equiv. N(C4H9)4(NO2) with (Cu2(NO)N6OC36H39)(2+) in presence of P(C6H5)3 (1 equiv.);; elem. anal.;	A 60% B 97%
In not given byproducts: O2; react. of 1 equiv. N(C4H9)4(NO2) with (Cu2(NO)N6OC36H39)(2+);; elem. anal.;	A 60% B 79%

Cu2(I)(C6H3(O)(CH2N(C2H4-2-pyridyl)2)2)(1+) (90065-16-0) + nitrogen(II) oxide (10102-43-9) → {Cu2(O)N6OC36H39}(1+)*PF6(1-)={Cu2(O)N6OC36H39}PF6 + dinitrogen monoxide (10024-97-2)

Conditions	Yield
In dichloromethane exposure of (Cu2N6OC36H39)(1+) to NO(g) in CH2Cl2 at -80 °C, warming;;	A 55% B 96%

trans-hydroxotetraamminenitrosoruthenium(II) + nitric acid (7697-37-2) → trans-tetraamminenitratonitrosoruthenium(III) nitrate + water (7732-18-5) + Nitrogen dioxide (10102-44-0) + nitrosylchloride (2696-92-6) + dinitrogen monoxide (10024-97-2)

Conditions	Yield
In nitric acid byproducts: Cl2; to Ru complex was added concd. HNO3; mixt. heated under reflux for 5 min; cooled to room temp.; ppt. filtered off; washed (water, alc., ether); dried (vac.); recrystd. (aq. HNO3); elem. anal.;	A 95% B n/a C n/a D n/a E n/a

4-nitrosotetrahydro-2H-pyran-4-yl 2,2,2-trichloroacetate (1194657-31-2) → Tetrahydro-4H-pyran-4-one (29943-42-8) + dinitrogen monoxide (10024-97-2) + trichloroacetic acid (76-03-9)

Conditions	Yield
With water In methanol; aq. phosphate buffer at 20℃; for 24h; pH=7.4; Kinetics; Reagent/catalyst; Sealed tube;	A n/a B 95% C n/a

ammonia (7664-41-7) → nitrogen (7727-37-9) + dinitrogen monoxide (10024-97-2)

Conditions	Yield
With oxygen In gaseous matrix byproducts: NO; 0.2 g of catalyst, 1000 ppm NH3, 2% O2, He as balance, GHSV=2.0E+5 h**-1, at 450°C; mass spect.;	A 94% B 0%
With oxygen In gaseous matrix byproducts: NO; 0.2 g of catalyst, 1000 ppm NH3, 2% O2, He as balance, GHSV=2.0E+5 h**-1, at 400°C; mass spect.;	A 93% B 0%
With oxygen In gaseous matrix byproducts: NO; 0.2 g of catalyst, 1000 ppm NH3, 2% O2, He as balance, GHSV=2.0E+5 h**-1, at 400°C; mass spect.;	A 92% B 0%

trifluorormethanesulfonic acid (1493-13-6) + [Fe2(NO)4(μ-1,3-bis(dimethylamino)-2-propanolate)]2(κ4-N2O2) → [Fe2(NO)4(μ-1,3-bis(dimethylamino)-2-propanolate)(μ-OSO2CF3)] + dinitrogen monoxide (10024-97-2)

Conditions	Yield
In tetrahydrofuran at 0℃; for 1h; Schlenk technique; Inert atmosphere;	A n/a B 93%

4-nitrosotetrahydro-2H-pyran-4-yl 2,2-dichloropropanoate → Tetrahydro-4H-pyran-4-one (29943-42-8) + 2,2-Dichloropropionic acid (75-99-0) + dinitrogen monoxide (10024-97-2)

Conditions	Yield
With water In methanol; aq. phosphate buffer at 20℃; for 24h; pH=7.4; Kinetics; Reagent/catalyst; Sealed tube;	A n/a B n/a C 92%

C46H57Fe2N13O4S(2+)*2BF4(1-) → C43H49Fe2N10O2(2+) + 2C39H41N10O(1-)*2Fe(2+)*2Fe(3+)*4HO(1-) + dinitrogen monoxide (10024-97-2)

Conditions	Yield
With cobaltocene In dichloromethane for 0.0833333h; Sealed tube; Inert atmosphere;	A n/a B n/a C 91%

nitrogen(II) oxide (10102-43-9) → nitrogen (7727-37-9) + oxygen (80937-33-3) + Nitrogen dioxide (10102-44-0) + dinitrogen monoxide (10024-97-2)

Conditions	Yield
Irradiation (UV/VIS); irradn. with Al-glitter (wave length:1860,1930 and 1990 A);	A 90% B 90% C 10% D 10%
Irradiation (UV/VIS); irradn. with Al-glitter (wave length:1860,1930 and 1990 A);	A 90% B 90% C 10% D 10%
La0.7Ba0.3Mn0.8In0.1Cu0.1O3 In neat (no solvent) decomposition over catalyst at 1073 K;	A 69.4% B 42.3% C 27.1% D 0%

ammonia (7664-41-7) + oxygen (80937-33-3) → dinitrogen monoxide (10024-97-2)

Conditions	Yield
manganese(II) oxide In neat (no solvent) catalytic oxidn. of NH3 (300 °C, O2-excess);;	90%
byproducts: N2, NO; excess of O2; at 300 °C; catalyst MnO2/Fe2O3/(eventually) Bi2O3; yield depending on mole ratio O2:NH3 and flow rate;;	90%
cobalt(II) oxide In neat (no solvent) oxidation at 300°C;;

ammonia (7664-41-7) → dinitrogen monoxide (10024-97-2)

Conditions	Yield
With oxygen 300 °C,with air;	90%
Electrolysis; NH3 soln. contg. CO2;anod contains Pt,Pd or Fe;	14.6%
Electrolysis;

Nitrite + tin(ll) chloride → hydroxylamine (7803-49-8) + dinitrogen monoxide (10024-97-2) + trans-hyponitrous acid (19467-31-3, 173728-04-6)

Conditions	Yield
In water	A n/a B 90% C n/a

cis-nitrous acid (7782-77-6) + tin(ll) chloride → hydroxylamine (7803-49-8) + dinitrogen monoxide (10024-97-2) + trans-hyponitrous acid (19467-31-3, 173728-04-6)

Conditions	Yield
In water	A n/a B 90% C n/a

copper(II)-hyponitrite → nitrogen (7727-37-9) + nitrogen(II) oxide (10102-43-9) + copper(II) oxide + dinitrogen monoxide (10024-97-2)

Conditions	Yield
In neat (no solvent) decompn. at 225-230°C;;	A 2-6 B 3-5 C n/a D 90%
In neat (no solvent) decompn. at 225-230°C;;	A 2-6 B 3-5 C n/a D 90%

hydroxylamine (7803-49-8) → dinitrogen monoxide (10024-97-2) + nitrosyl hydride

Conditions	Yield
With hypochloric acid In aq. phosphate buffer at 37℃; pH=7.4;	A n/a B 90%

potassium nitrite (7758-09-0) + hydrazin sulfate → nitrogen (7727-37-9) + dinitrogen monoxide (10024-97-2) + trans-hyponitrous acid (19467-31-3, 173728-04-6)

Conditions	Yield
In not given at room temp. or upon boiling from equimolar amounts in 3% solns.; no formation of H2N2O2 even in concd. solns. at low temps.; mole ratio of N2O:N2 depends on the mole ratio nitrite:hydrazonium salt;;	A 11% B 89% C 0%

C52H70Fe2N14O5(3+)*3BF4(1-) → dinitrogen monoxide (10024-97-2)

Conditions	Yield
With cobaltocene In dichloromethane for 0.0833333h; Inert atmosphere;	89%
With silver; N,N,N,N-tetraethylammonium tetrafluoroborate In dichloromethane Inert atmosphere; Electrochemical reaction;	89%

hydroxylamine (7803-49-8) → nitrogen (7727-37-9) + dinitrogen monoxide (10024-97-2)

Conditions	Yield
With Hg2(NO3)2 In not given byproducts: Hg; addn. of 0.04 M NH2OH to 0.005 M Hg2(NO3)2 soln. buffered with acetate at 20°C, autocatalysis of reaction by Hg;;	A 13% B 87%
With Hg2(NO3)2; silver In not given byproducts: Hg; addn. of 0.04 M NH2OH to 0.005 M Hg2(NO3)2 soln. buffered with acetate at 20°C, autocatalysis of reaction by Hg, further catalysis by addn. of collodial Ag soln.;;	A 63% B 34%
With oxygen In not given byproducts: water; Electrolysis; N2O formed on cathode, N2 formed on anode;

[(copper(II)(tris(2-pyridylmethyl)amine))2(μ-hyponitrite)](2+) + nitrogen(II) oxide (10102-43-9) → [copper(II)(tris(2-pyridylmethyl)amine)(nitrito)](1+) + dinitrogen monoxide (10024-97-2)

Conditions	Yield
In methanol Inert atmosphere; Schlenk technique;	A 85% B n/a

Ketene (463-51-4) + nitrogen(II) oxide (10102-43-9) → fulminic acid (51060-05-0) + hydrogen cyanide (74-90-8) + carbon monoxide (201230-82-2) + water (7732-18-5) + dinitrogen monoxide (10024-97-2)

Conditions	Yield
byproducts: H2CO; Irradiation (UV/VIS); photolysis of CH2CO/NO/Ar mixt. with 200 W high pressure Hg lamp (photolysis of CH2CO generates CH2 radicals) in Duran glass tube (20 cm long, 4cm i.d.) at room temp. and ambient pressure;	A 84% B 15% C n/a D n/a E n/a

bis(η5.-pentamethylcyclopentadienyl)(η2-phenyltrimethylsilylacetylene)zirconium + dinitrogen monoxide (10024-97-2) → (η(5)-C5Me5)2Zr(OCPh=CSiMe3) (205107-24-0)

Conditions	Yield
In neat (no solvent) byproducts: N2; absence of air and moisture; 500 Torr N2O, room temp., 24 h; removal of gases; elem. anal.;	100%
In toluene byproducts: N2; absence of air and moisture; N2O-atmosphere, warming from -78°C to room temp., stirring for 30 min; rsolvent removal, recrystn. (hexane/O(SiMe3)2);	65%
In benzene absence of air and moisture;

(η(5)-C5Me5)2Zr(Me3SiC.tplbond.C(c-C5H9)) + dinitrogen monoxide (10024-97-2) → (η(5)-C5Me5)2Zr(OC(c-C5H9)=CSiMe3) (205107-25-1)

Conditions	Yield
In neat (no solvent) byproducts: N2; absence of air and moisture; 500 Torr N2O, room temp., 24 h; removal of gases; elem. anal.;	100%
In benzene absence of air and moisture;

(((p-tolyl)B(pyrazolyl)2)2Py)ScH + dinitrogen monoxide (10024-97-2) → (((p-tolyl)B(pyrazolyl)2)2Py)Sc-O-Sc(((p-tolyl)B(pyrazolyl)2)2Py)

Conditions	Yield
In benzene-d6 at 80℃; under 760.051 Torr; for 18h; Inert atmosphere; Schlenk technique;	100%

methane (34557-54-5) + dinitrogen monoxide (10024-97-2) → methanol (67-56-1) + formaldehyd (50-00-0) + carbon dioxide (124-38-9) + carbon monoxide (201230-82-2) + nitrogen (7727-37-9)

Conditions	Yield
In neat (no solvent) Kinetics; Oxidation of CH4 by N2O in presence of catalyst (773 K): deposited Cu(2+) on carbon;;	A 0.2% B 0.3% C 99.5% D 0% E n/a
In neat (no solvent) Kinetics; byproducts: C2H5OH (small quantity); oxidation of CH4 by N2O in presence of catalyst (773 K): deposited Ti(4+) on carbon;;	A 13.8% B 0% C 86.2% D 0% E n/a
In neat (no solvent) Kinetics; Oxidation of CH4 by N2O in presence of catalyst (773 K): deposited Co(2+) on carbon;;	A 0% B 0% C 75% D 25% E n/a

potassium amide + dinitrogen monoxide (10024-97-2) → potassium azide (20762-60-1)

Conditions	Yield
byproducts: KOH, NH3; 270-280 °C in rotating furnace; the white layer of KOH and KN3 dissolved in water, the soln. evaporated, KN3 crystd.;	99%
byproducts: KOH, NH3; 270-280 °C in rotating furnace; the white layer of KOH and KN3 dissolved in water, the soln. evaporated, KN3 crystd.;	99%
In ammonia byproducts: KOH, NH3; -70°C;
In ammonia byproducts: KOH, NH3; NH3 (liquid); -70°C;

nitrogen trifluoride (7783-54-2) + antimony pentafluoride (7783-70-2) + dinitrogen monoxide (10024-97-2) → NF2O(1+)*Sb2F11(1-) =(NF2O)(Sb2F11) (12528-55-1)

Conditions	Yield
byproducts: N2; 150°C;	99%
100°C;	0%

N[2-P(CHMe3)2-4-methylphenyl]2V(CH2tBu)2 (1039748-93-0) + dinitrogen monoxide (10024-97-2) → V(N[4-Me-2-(PiPr2)C6H3]2)(CHtBu)O*0.5C5H10

Conditions	Yield
In benzene V-complex reacted with N2O in benzene at 90°C;	99%

(η5-C5Me5)*W{N(iPr)C(Me)N(iPr)}(NSiMe3) + dinitrogen monoxide (10024-97-2) → (η5-C5Me5)W[N(iPr)C(Me)N(iPr)](nitrido)(OSiMe3)

Conditions	Yield
at 25℃; for 216h;	99%

bis[2,6-bis(1-naphthyl)phenyl]germylene (328396-60-7) + dinitrogen monoxide (10024-97-2) → bis[2,6-bis(1-naphthyl)phenyl]germanone (327179-04-4)

Conditions	Yield
In toluene left standing under N2 for 2 d; solvent evpd. in vacuo;	98%

potassium diphenylphosphanylborohydride + dinitrogen monoxide (10024-97-2) → KOPPh2BH3

Conditions	Yield
In tetrahydrofuran soln. of B compd. stirred at room temp. under N2O atm. until gas evolution stopped (ca. 5 min); evapd., elem. anal.;	98%

K[P((t)Bu)2BH3] + dinitrogen monoxide (10024-97-2) → K(1+)*OP(C(CH3)3)2BH3(1-)=K[(C(CH3)3)2OPBH3]

Conditions	Yield
In tetrahydrofuran soln. of B compd. stirred at room temp. under N2O atm. until gas evolution stopped (ca. 5 min); evapd., elem. anal.;	98%

[{(i-Bu)2(aminotroponiminate)Ge(i-Pr)(ZnCl2)}2] + dinitrogen monoxide (10024-97-2) → [{(i-Bu)2ATIGe(O)(i-Pr)(ZnCl2)}2]

Conditions	Yield
In tetrahydrofuran at 20℃; for 0.5h; Inert atmosphere; Schlenk technique;	98%

[(C(C6H4P(CH(CH3)2)2)2)IrCl] + dinitrogen monoxide (10024-97-2) → C25H36ClIrOP2

Conditions	Yield
In benzene-d6 at 20℃; under 760.051 Torr; for 24h;	98%

ethylenebis(1,3-di-tert-butylcyclopentadienyl)titanium (1033858-47-7) + dinitrogen monoxide (10024-97-2) → μ-oxotetrakis(1,3-di-tert-butylcyclopentadienyl)dititanium (827030-28-4) + di-μ-oxotetrakis(1,3-di-tert-butylcyclopentadienyl)dititanium (1033858-56-8)

Conditions	Yield
In pentane Ti complex dissolved in pentane; exposed to N2O (1 atm); solvent removed under vac.; extd. into hot toluene; cooled to room temp.and then to -20°C; crystals isolated; elem. anal.;	A 0% B 97%

(HC(CMeNC-2,6-i-Pr2C6H3)2)-germanium(II) hydride (382150-90-5) + dinitrogen monoxide (10024-97-2) → (HC(CMeNC-2,6-i-Pr2C6H3)2)-germanium(II) hydroxide (692776-46-8)

Conditions	Yield
In toluene under N2 or Ar; dry N2O bubbled into soln. of Ge compd. in toluene at room temp. for 30 min; volatiles removed in vac.; treated with n-hexane; filtered; dried in vac.;	95%

C20H46BN2P + dinitrogen monoxide (10024-97-2) → C20H46BN2OP

Conditions	Yield
In toluene at 20℃; under 760.051 Torr; for 24h; Cooling with liquid nitrogen; Inert atmosphere;	94%

[(2,6-(2,4,6-Me3C6H2)2C6H3)Ge-(1,3,4,5-tetramethylimidazol-2-ylidene)2][(3,5-(CF3)2C6H3)4B] + dinitrogen monoxide (10024-97-2) → [(2,6-(2,4,6-Me3C6H2)2C6H3)Ge(O)(1,3,4,5-tetramethylimidazol-2-ylidene)2][(3,5-(CF3)2C6H3)4B]

Conditions	Yield
In acetonitrile Inert atmosphere;	94%

Upstream product

• 14168-44-6 MEDINA 
• 7803-49-8 hydroxylamine 
• 64-18-6 formic acid 
• 7697-37-2 nitric acid 
• 12775-96-1 copper 
• 7632-00-0 sodium nitrite 
• 7783-99-5 silver(I) nitrite 
• 20667-12-3 silver(l) oxide 
• 7783-41-7 difluoroether 
• 22750-57-8 cesium azide 
• 3352-57-6 hydroxyl 
• 7727-37-9 nitrogen 
• 599-71-3 piloty's acid 
• 10028-15-6 ozone 

Downstream Products

• 124-38-9 carbon dioxide 
• 7727-37-9 nitrogen 
• 10102-43-9 nitrogen(II) oxide 
• 14700-96-0 clorine 
• 3352-57-6 hydroxyl 
• 7722-84-1 dihydrogen peroxide 
• 80937-33-3 oxygen 
• 14797-55-8 Nitrate 
• 1304-29-6 barium peroxide 
• 1310-82-3 rubidium monoxide radical 
• 10102-44-0 Nitrogen dioxide 
• 7446-11-9 sulfur trioxide 
• 7446-09-5 sulfur dioxide 
• 14967-78-3 nitric oxide anion 

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Rates of decomposition of ammonium nitrate in the liquid and vapor state have been measured at temperatures up to 400 deg C.The evidence indicates that an ionic mechanism operating at temperatures below 290 deg C is overtaken by a homolytic mechanism at higher temperatures.The activation energy increases to 193 kJ/mol, which is nearly equal to the N-O bond energy in HNO3.Water and NH3 strogly inhibit the ionic reaction at low temperature, but the effect fades away at high temperature.There is no primary H/D kinetic isotope effect.The reaction rates of liquid and vapor are nearly the same at high temperature.The rate at high temperature is given by (kT/h)e4.06e-23300/T.

Carbon-Nitrogen and Nitrogen-Nitrogen Bond Formation from Nucleophilic Attack at Coordinated Nitrosyls in Fe and Ru Heme Models

The conversion of inorganic NOx species to organo-N compounds is an important component of the global N-cycle. Reaction of a C-based nucleophile, namely the phenyl anion, with the ferric heme nitrosyl [(OEP)Fe(NO)(5-MeIm)]+ generates a mixture of the C-nitroso derivative (OEP)Fe(PhNO)(5-MeIm) and (OEP)Fe(Ph). The related reaction with [(OEP)Ru(NO)(5-MeIm)]+ generates the (OEP)Ru(PhNO)(5-MeIm) product. Reactions with the N-based nucleophile diethylamide results in the formation of free diethylnitrosamine, whereas the reaction with azide results in N2O formation; these products derive from attack of the nucleophiles on the bound NO groups. These results provide the first demonstrations of C-N and N-N bond formation from attack of C-based and N-based nucleophiles on synthetic ferric-NO hemes.

Thermal behaviour of ammonium nitrate prills coated with limestone and dolomite powder

The thermal behaviour of ammonium nitrate (AN) and its prills coated with limestone and dolomite powder was studied on the basis of commercial fertilizer-grade AN and six Estonian limestone and dolomite samples. Coating of AN prills was carried out on a plate granulator and a saturated solution of AN was used as a binding agent. The mass of AN prills and coating material was calculated based on the mole ratio of AN/(CaO + MgO) = 2:1. Thermal behaviour of AN and its coated prills was studied using combined TG-DTA-FTIR equipment. The experiments were carried out under dynamic heating conditions up to 900 °C at the heating rate of 10 °C min-1 and for calculation of kinetic parameters, additionally, at 2, 5 and 20 °C min-1 in a stream of dry air. A model-free kinetic analysis approach based on the differential isoconversional method of Friedman was used to calculate the kinetic parameters. The results of TG-DTA-FTIR analyses and the variation of the value of activation energy E along the reaction progress α indicate the complex character of the decomposition of neat AN as well as of the interactions occurring at thermal treatment of AN prills coated with limestone and dolomite powder.

Characterization and catalytic activity for the NO decomposition and reduction by CO of nanosized Co3O4

Nanosized Co3O4 prepared by a precipitation method was characterized by TEM, XRD, BET and TPD techniques, and studied for NO decomposition and reduction by CO. It is found that Co3O4 thus obtained has a specific surface area of 23.4 m2/g and an average particle size of 26 nm. Catalytic tests showed that full NO conversion to N2 was obtained above 300 °C. A redox mechanism between Co 3+ and Co2+ ions based on NO decomposition is proposed.

SURFACE STATES OF MoO3 ON ZrO2 AND CATALYTIC PROPERTIES FOR THE REACTION OF NO WITH H2

The adsorption and reaction of nitric oxide on reduced molybdena-zirconia were studied by means of e.s.r., i.r. and u.v. spectroscopies.On the surface, at least two types of nitrosyl complex exist.At an early stage of reduction, a diamagnetic dinitrosyl complex with i.r. bands at ca. 1790 and 1690 cm-1 formed on NO adsorption and was ascribed to Mo(4+)(NO)2.After reduction at a higher temperature, a paramagnetic dinitrosyl species appeared upon NO adsorption and was tentatively assigned to Mo(5+)(NO)2.Nitric oxide can adsorb on Mo(5+) in tetrahedral coordination, but not on Mo(5+) in octahedral coordination.This can be explained by the coordination being limited.For the reaction of NO with H2, the species of Mo(5+)(NO)2 was concluded to be a main active complex in the catalytic cycle.

Solid-gas reactions for nitroxyl (HNO) generation in the gas phase

We present a novel nitroxyl (HNO) generation method, which avoids the need of using a liquid system or extreme experimental conditions. This method consists of the reaction between a gaseous base and an HNO donor (Piloty's acid) in the solid phase, allowi

The influence of Ba addition on thermal stability and catalytic activity of Cu-based mixed oxide

Catalytic reduction of NO by CO was studied over La2-xBaxCuO4 (x = 0.0 or 0.4) mixed oxides prepared by coprecipitation method. The catalysts were characterized by X ray diffraction (XRD), O2 temperature-programmed desorption (O2-TPD), H2 temperature-programmed reduction (H2-TPR) and X-ray absorption near edge structure (XANES). NO + CO reaction was carried out in a fixed-bed flow reactor, from room temperature to 500 °C, at atmospheric pressure. Both fresh catalysts were active for the NO + CO reaction but when were submitted to thermal aging, the barium free catalyst significantly lost its activity. The partial substitution of La by Ba enhanced the thermal stability and although the activity of the catalyst has decreased, it remains high, approaching 100 % at 500 °C. These results can be associated with reducible copper species observed by XANES in the thermal aged catalyst containing Ba.

The Effects of Platinum Dispersion and Pt State on Catalytic Properties of Pt/Al2O3 in NH3 Oxidation

Dependence of NH3 oxidation on the state and dispersion of Pt species in Pt/γ-Al2O3 catalysts was investigated. Prereduced Pt/γ-Al2O3 catalysts containing Pt0 nanoparticles exhibited significantly higher activity than preoxidized ones with the same Pt dispersion. The most significant improvement of the catalytic activity (TOF increased by 30 times) was observed when the size of Pt0 particles increased from ～1 to ～8 nm. N2 selectivity was found to be mainly determined by the reaction temperature, with a minor influence of Pt particle size. Preoxidized catalysts containing ionic Pt were activated by the reaction medium, while partial deactivation was observed for the prereduced ones. The activity improvement was associated with the presence of Pt4+/Pt2+ species on the surface of preoxidized catalysts. The activity decrease of the prereduced catalysts was due to the partial oxidation and subsequent redispersion of Pt particles. Introduction of H2O and CO2 to the reaction mixture only moderately influenced NH3 oxidation activity shifting NH3 conversion curves by about +15 °C.