DINITROGEN OXIDE

CAS NUMBER: 10024-97-2

EC NUMBER: 233-032-0

MOLECULAR FORMULA: N2O

MOLECULAR WEIGHT: 44.013

IUPAC NAME: nitrous oxide

Dinitrogen Oxide is a colorless, sweet-tasting gas. 
Dinitrogen Oxide is also known as "laughing gas". 
Continued breathing of the vapors may impair the decision making process. 
Dinitrogen Oxide is noncombustible but it will accelerate the burning of combustible material in a fire. 
Dinitrogen Oxide is soluble in water. 
Dinitrogen Oxide's vapors are heavier than air. 
Dinitrogen Oxide Exposures of the container to prolonged heat or fire can cause it to rupture violently and rocket. 
Dinitrogen Oxide is used as an anesthetic, in pressure packaging, and to manufacture other chemicals.

Dinitrogen Oxide is a naturally occurring gas that is colorless and non flammable. 
Dinitrogen Oxide can be manufactured and used for a variety of things such as a pharmacologic agent to produce anesthesia, a food additive as a propellant, and an additive to fuels to increase available oxygen in combustion.

Dinitrogen Oxide, refrigerated liquid appears as a colorless liquid. 
Dinitrogen Oxide's Density 1.22 g / cm3 at its boiling point of -89°C. 
Dinitrogen Oxide's Vapor pressure is at about 745 psig at 70°F. 
Dinitrogen Oxide is Used to freeze foods and to manufacture other chemicals.

Dinitrogen Oxide, commonly known as laughing gas, nitrous, or nos, is a chemical compound, an oxide of nitrogen with the formula N2O. 
At room temperature, Dinitrogen Oxide is a colourless non-flammable gas, with a slight metallic scent and taste. 
At elevated temperatures, Dinitrogen Oxide is a powerful oxidiser similar to molecular oxygen.

Dinitrogen Oxide has significant medical uses, especially in surgery and dentistry, for its anaesthetic and pain reducing effects. 
Dinitrogen Oxide's colloquial name, "laughing gas", coined by Humphry Davy, is due to the euphoric effects upon inhaling it, a property that has led to its recreational use as a dissociative anaesthetic. 
Dinitrogen Oxide is on the World Health Organisation's List of Essential Medicines, the safest and most effective medicines needed in a health system.
Dinitrogen Oxide is also used as an oxidiser in rocket propellants, and in motor racing to increase the power output of engines.

Dinitrogen Oxide's atmospheric concentration reached 333 parts per billion (ppb) in 2020, increasing at a rate of about 1 ppb annually.
Dinitrogen Oxide is a major scavenger of stratospheric ozone, with an impact comparable to that of CFCs. 
Global accounting of N2O sources and sinks over the decade ending 2016 indicates that about 40% of the average 17 TgN/yr (Teragrams of Nitrogen per year) of emissions originated from human activity, and shows that emissions growth chiefly came from expanding agriculture and industry sources within emerging economies

USES OF DINITROGEN OXIDE
Rocket Motors:
Dinitrogen Oxide may be used as an oxidiser in a rocket motor. 
Dinitrogen Oxide has advantages over other oxidisers in that it is much less toxic, and because of its stability at room temperature it is also easier to store and relatively safe to carry on a flight. 
As a secondary benefit, it may be decomposed readily to form breathing air. 
Dinitrogen Oxide's high density and low storage pressure (when maintained at low temperature) enable it to be highly competitive with stored high-pressure gas systems.

In a 1914 patent, American rocket pioneer Robert Goddard suggested Dinitrogen Oxide and gasoline as possible propellants for a liquid-fuelled rocket.
Dinitrogen Oxide has been the oxidiser of choice in several hybrid rocket designs (using solid fuel with a liquid or gaseous oxidiser). 
The combination of Dinitrogen Oxide with hydroxyl-terminated polybutadiene fuel has been used by SpaceShipOne and others. 
Dinitrogen Oxide also is notably used in amateur and high power rocketry with various plastics as the fuel.

Dinitrogen Oxide also may be used in a monopropellant rocket. 
In the presence of a heated catalyst, N
2O will decompose exothermically into nitrogen and oxygen, at a temperature of approximately 1,070 °F (577 °C).
Because of the large heat release, the catalytic action rapidly becomes secondary, as thermal autodecomposition becomes dominant. 
In a vacuum thruster, this may provide a monopropellant specific impulse (Isp) of as much as 180 s. 

Dinitrogen Oxide is said to deflagrate at approximately 600 °C (1,112 °F) at a pressure of 309 psi (21 atmospheres).
At 600 psi, for example, the required ignition energy is only 6 joules, whereas N2O at 130 psi a 2,500-joule ignition energy input is insufficient

Internal Combustion Engine:
In vehicle racing, Dinitrogen Oxide (often referred to as just "nitrous") allows the engine to burn more fuel by providing more oxygen during combustion. 
The increase in oxygen allows for an increase in the injection of fuel, allowing the engine to produce more engine power. 
The gas is not flammable at a low pressure/temperature, but it delivers more oxygen than atmospheric air by breaking down at elevated temperatures, about 570 degrees F (~300C). 
Therefore, it often is mixed with another fuel that is easier to deflagrate. 
Dinitrogen Oxide is a strong oxidising agent, roughly equivalent to hydrogen peroxide, and much stronger than oxygen gas.

Dinitrogen Oxide is stored as a compressed liquid; the evaporation and expansion of liquid Dinitrogen Oxide in the intake manifold causes a large drop in intake charge temperature, resulting in a denser charge, further allowing more air/fuel mixture to enter the cylinder. 
Sometimes Dinitrogen Oxide is injected into (or prior to) the intake manifold, whereas other systems directly inject, right before the cylinder (direct port injection) to increase power.

The technique was used during World War II by Luftwaffe aircraft with the GM-1 system to boost the power output of aircraft engines. 
Originally meant to provide the Luftwaffe standard aircraft with superior high-altitude performance, technological considerations limited its use to extremely high altitudes. 
Accordingly, it was only used by specialised planes such as high-altitude reconnaissance aircraft, high-speed bombers and high-altitude interceptor aircraft. 
Dinitrogen Oxide sometimes could be found on Luftwaffe aircraft also fitted with another engine-boost system, MW 50, a form of water injection for aviation engines that used methanol for its boost capabilities.

One of the major problems of using Dinitrogen Oxide in a reciprocating engine is that it can produce enough power to damage or destroy the engine. 
Very large power increases are possible, and if the mechanical structure of the engine is not properly reinforced, the engine may be severely damaged, or destroyed, during this kind of operation. 
Dinitrogen Oxide is very important with Dinitrogen Oxide augmentation of petrol engines to maintain proper operating temperatures and fuel levels to prevent "pre-ignition" or "detonation" (sometimes referred to as "knock"). 
Most problems that are associated with Dinitrogen Oxide do not come from mechanical failure due to the power increases. 
Since Dinitrogen Oxide allows a much denser charge into the cylinder, it dramatically increases cylinder pressures. 
The increased pressure and temperature can cause problems such as melting the piston or valves. 
Dinitrogen Oxide also may crack or warp the piston or head and cause pre-ignition due to uneven heating.

Automotive-grade liquid Dinitrogen Oxide differs slightly from medical-grade Dinitrogen Oxide. 
A small amount of sulfur dioxide (SO2) is added to prevent substance abuse.
Multiple washes through a base (such as sodium hydroxide) can remove this, decreasing the corrosive properties observed when SO2 is further oxidised during combustion into sulfuric acid, making emissions cleaner.

Aerosol Propellant:
The gas is approved for use as a food additive (E number: E942), specifically as an aerosol spray propellant. 
Dinitrogen Oxide's most common uses in this context are in aerosol whipped cream canisters and cooking sprays.

The gas is extremely soluble in fatty compounds. 
In aerosol whipped cream, it is dissolved in the fatty cream until it leaves the can, when it becomes gaseous and thus creates foam. 
Used in this way, it produces whipped cream which is four times the volume of the liquid, whereas whipping air into cream only produces twice the volume. 
If air were used as a propellant, oxygen would accelerate rancidification of the butterfat, but Dinitrogen Oxide inhibits such degradation. 
Carbon dioxide cannot be used for whipped cream because it is acidic in water, which would curdle the cream and give it a seltzer-like "sparkling" sensation.

The whipped cream produced with Dinitrogen Oxide is unstable, however, and will return to a more liquid state within half an hour to one hour.
Thus, the method is not suitable for decorating food that will not be served immediately.
During December 2016, some manufacturers reported a shortage of aerosol whipped creams in the United States due to an explosion at the Air Liquide Dinitrogen Oxide facility in Florida in late August. 

With a major facility offline, the disruption caused a shortage resulting in the company diverting the supply of Dinitrogen Oxide to medical clients rather than to food manufacturing. 
The shortage came during the Christmas and holiday season when canned whipped cream use is normally at its highest.
Similarly, cooking spray, which is made from various types of oils combined with lecithin (an emulsifier), may use Dinitrogen Oxide as a propellant. Other propellants used in cooking spray include food-grade alcohol and propane.

Medicine:
Dinitrogen Oxide has been used in dentistry and surgery, as an anaesthetic and analgesic, since 1844.
In the early days, the gas was administered through simple inhalers consisting of a breathing bag made of rubber cloth.
Today, the gas is administered in hospitals by means of an automated relative analgesia machine, with an anaesthetic vaporiser and a medical ventilator, that delivers a precisely dosed and breath-actuated flow of Dinitrogen Oxide mixed with oxygen in a 2:1 ratio.

Dinitrogen Oxide is a weak general anaesthetic, and so is generally not used alone in general anaesthesia, but used as a carrier gas (mixed with oxygen) for more powerful general anaesthetic drugs such as sevoflurane or desflurane. 
Dinitrogen Oxide has a minimum alveolar concentration of 105% and a blood/gas partition coefficient of 0.46. 
The use of Dinitrogen Oxide in anaesthesia, however, can increase the risk of postoperative nausea and vomiting.

Dentists use a simpler machine which only delivers an N2O/O2 mixture for the patient to inhale while conscious.
The patient is kept conscious throughout the procedure, and retains adequate mental faculties to respond to questions and instructions from the dentist.

Inhalation of Dinitrogen Oxide is used frequently to relieve pain associated with childbirth, trauma, oral surgery and acute coronary syndrome (includes heart attacks). 
Dinitrogen Oxide's use during labour has been shown to be a safe and effective aid for birthing women.
Dinitrogen Oxide's use for acute coronary syndrome is of unknown benefit.

Recreational Use:
Recreational inhalation of Dinitrogen Oxide, with the purpose of causing euphoria and/or slight hallucinations, began as a phenomenon for the British upper class in 1799, known as "laughing gas parties".
Starting in the nineteenth century, widespread availability of the gas for medical and culinary purposes allowed the recreational use to expand greatly throughout the world. 
In the United Kingdom, as of 2014, Dinitrogen Oxide was estimated to be used by almost half a million young people at nightspots, festivals and parties.
The legality of that use varies greatly from country to country, and even from city to city in some countries.

Widespread recreational use of the drug throughout the UK was featured in the 2017 Vice documentary Inside The Laughing Gas Black Market, in which journalist Matt Shea met with dealers of the drug who stole it from hospitals, although with Dinitrogen Oxide canisters being readily available online, the incidents of hospital theft are expected to be extremely rare.
Dinitrogen Oxide is a significant issue cited in London's press is the effect of Dinitrogen Oxide canister littering, which is highly visible and causes significant complaint from communities.

Mechanism of Action:
The pharmacological mechanism of action of N2O in medicine is not fully known. 
However, it has been shown to directly modulate a broad range of ligand-gated ion channels, and this likely plays a major role in many of its effects. 
Dinitrogen Oxide moderately blocks NMDAR and β2-subunit-containing nACh channels, weakly inhibits AMPA, kainate, GABAC and 5-HT3 receptors, and slightly potentiates GABAA and glycine receptors.
Dinitrogen Oxide also has been shown to activate two-pore-domain K+channels.While N2O affects quite a few ion channels, its anaesthetic, hallucinogenic and euphoriant effects are likely caused predominantly, or fully, via inhibition of NMDA receptor-mediated currents.
In addition to its effects on ion channels, N2O may act to imitate nitric oxide (NO) in the central nervous system, and this may be related to its analgesic and anxiolytic properties.
Dinitrogen Oxide is 30 to 40 times more soluble than nitrogen.

The effects of inhaling sub-anaesthetic doses of Dinitrogen Oxide have been known to vary, based on several factors, including settings and individual differences;however, from his discussion, Jay (2008) suggests that it has been reliably known to induce the following states and sensations:
-Intoxication
-Euphoria/dysphoria
-Spatial disorientation
-Temporal disorientation
-Reduced pain sensitivity
A minority of users also will present with uncontrolled vocalisations and muscular spasms. 
These effects generally disappear minutes after removal of the Dinitrogen Oxide source

Anaesthetic Use:
The first time Dinitrogen Oxide was used as an anaesthetic drug in the treatment of a patient was when dentist Horace Wells, with assistance by Gardner Quincy Colton and John Mankey Riggs, demonstrated insensitivity to pain from a dental extraction on 11 December 1844.
In the following weeks, Wells treated the first 12 to 15 patients with Dinitrogen Oxide in Hartford, Connecticut, and, according to his own record, only failed in two cases.
In spite of these convincing results having been reported by Wells to the medical society in Boston in December 1844, this new method was not immediately adopted by other dentists. 
The reason for this was most likely that Wells, in January 1845 at his first public demonstration to the medical faculty in Boston, had been partly unsuccessful, leaving his colleagues doubtful regarding its efficacy and safety.
The method did not come into general use until 1863, when Gardner Quincy Colton successfully started to use it in all his "Colton Dental Association" clinics, that he had just established in New Haven and New York City.
Over the following three years, Colton and his associates successfully administered Dinitrogen Oxide to more than 25,000 patients.
Today, Dinitrogen Oxide is used in dentistry as an anxiolytic, as an adjunct to local anaesthetic.

Dinitrogen Oxide was not found to be a strong enough anaesthetic for use in major surgery in hospital settings, however. 
Instead, diethyl ether, being a stronger and more potent anaesthetic, was demonstrated and accepted for use in October 1846, along with chloroform in 1847.
When Joseph Thomas Clover invented the "gas-ether inhaler" in 1876, however, it became a common practice at hospitals to initiate all anaesthetic treatments with a mild flow of Dinitrogen Oxide, and then gradually increase the anaesthesia with the stronger ether or chloroform. 
Clover's gas-ether inhaler was designed to supply the patient with Dinitrogen Oxide and ether at the same time, with the exact mixture being controlled by the operator of the device. 
Dinitrogen Oxide remained in use by many hospitals until the 1930s.
Although hospitals today use a more advanced anaesthetic machine, these machines still use the same principle launched with Clover's gas-ether inhaler, to initiate the anaesthesia with Dinitrogen Oxide, before the administration of a more powerful anaesthetic.

As a Patent Medicine:
Colton's popularisation of Dinitrogen Oxide led to its adoption by a number of less than reputable quacksalvers, who touted it as a cure for consumption, scrofula, catarrh and other diseases of the blood, throat and lungs. 
Dinitrogen Oxide treatment was administered and licensed as a patent medicine by the likes of C. L. Blood and Jerome Harris in Boston and Charles E. Barney of Chicago

PRODUCTION:
Reviewing various methods of producing Dinitrogen Oxide is published
Industrial Methods:
Dinitrogen Oxide is prepared on an industrial scale by careful heating of ammonium nitrate at about 250 C, which decomposes into Dinitrogen Oxide and water vapour.

NH4NO3 → 2 H2O + N2O
The addition of various phosphate salts favours formation of a purer gas at slightly lower temperatures. 
This reaction may be difficult to control, resulting in detonation.

Laboratory Methods:
The decomposition of ammonium nitrate is also a common laboratory method for preparing the gas. 
Equivalently, it can be obtained by heating a mixture of sodium nitrate and ammonium sulfate:
2 NaNO3 + (NH4)2SO4 → Na2SO4 + 2 N2O + 4 H2O

Another method involves the reaction of urea, nitric acid and sulfuric acid:
2 (NH2)2CO + 2 HNO3 + H2SO4 → 2 N2O + 2 CO2 + (NH4)2SO4 + 2 H2O

Direct oxidation of ammonia with a manganese dioxide-bismuth oxide catalyst has been reported:[107] cf. Ostwald process.
2 NH3 + 2 O2 → N2O + 3 H2O

Hydroxylammonium chloride reacts with sodium nitrite to give Dinitrogen Oxide. 
If the nitrite is added to the hydroxylamine solution, the only remaining by-product is salt water. 
If the hydroxylamine solution is added to the nitrite solution (nitrite is in excess), however, then toxic higher oxides of nitrogen also are formed:
NH3OHCl + NaNO2 → N2O + NaCl + 2 H2O

Treating HNO3 with SnCl2 and HCl also has been demonstrated:
2 HNO3 + 8 HCl + 4 SnCl2 → 5 H2O + 4 SnCl4 + N2O

Hyponitrous acid decomposes to N2O and water with a half-life of 16 days at 25 °C at pH 1–3.

H2N2O2→ H2O + N2O

Atmospheric Occurrence:
Dinitrogen Oxide is a minor component of Earth's atmosphere and is an active part of the planetary nitrogen cycle. 
Based on analysis of air samples gathered from sites around the world, its concentration surpassed 330 ppb in 2017.
The growth rate of about 1 ppb per year has also accelerated during recent decades.
Dinitrogen Oxide's atmospheric abundance has grown more than 20% from a base level of about 270 ppb in year 1750

Emissions by Source:
As of 2010, it was estimated that about 29.5 million tonnes of N2O (containing 18.8 million tonnes of nitrogen) were entering the atmosphere each year; of which 64% were natural, and 36% due to human activity.
Most of the N2O emitted into the atmosphere, from natural and anthropogenic sources, is produced by microorganisms such as denitrifying bacteria and fungi in soils and oceans.
Soils under natural vegetation are an important source of Dinitrogen Oxide, accounting for 60% of all naturally produced emissions. 
Other natural sources include the oceans (35%) and atmospheric chemical reactions (5%).

A 2019 study showed that emissions from thawing permafrost are 12 times higher than previously assumed.
The main components of anthropogenic emissions are fertilised agricultural soils and livestock manure (42%), runoff and leaching of fertilisers (25%), biomass burning (10%), fossil fuel combustion and industrial processes (10%), biological degradation of other nitrogen-containing atmospheric emissions (9%) and human sewage (5%).
Agriculture enhances Dinitrogen Oxide production through soil cultivation, the use of nitrogen fertilisers and animal waste handling.
These activities stimulate naturally occurring bacteria to produce more Dinitrogen Oxide. 
Dinitrogen Oxide emissions from soil can be challenging to measure as they vary markedly over time and space, and the majority of a year's emissions may occur when conditions are favorable during "hot moments" and/or at favorable locations known as "hotspots".

Among industrial emissions, the production of nitric acid and adipic acid are the largest sources of Dinitrogen Oxide emissions. 
The adipic acid emissions specifically arise from the degradation of the nitrolic acid intermediate derived from nitration of cyclohexanone.

Biological Processes:
Natural processes that generate Dinitrogen Oxide may be classified as nitrification and denitrification. 
Specifically, they include: aerobic autotrophic nitrification, the stepwise oxidation of ammonia (NH3) to nitrite (NO−2) and to nitrate (NO−3) anaerobic heterotrophic denitrification, the stepwise reduction of NO−3 to NO−2, nitric oxide (NO), N2O and ultimately N2, where facultative anaerobe bacteria use NO−3 as an electron acceptor in the respiration of organic material in the condition of insufficient oxygen (O2) nitrifier denitrification, which is carried out by autotrophic NH3-oxidising bacteria and the pathway whereby ammonia (NH3) is oxidised to nitrite (NO−2), followed by the reduction of NO−2 to nitric oxide (NO), N2O and molecular nitrogen (N2) heterotrophic nitrification aerobic denitrification by the same heterotrophic nitrifiers fungal denitrification non-biological chemodenitrification.
These processes are affected by soil chemical and physical properties such as the availability of mineral nitrogen and organic matter, acidity and soil type, as well as climate-related factors such as soil temperature and water content.
The emission of the gas to the atmosphere is limited greatly by its consumption inside the cells, by a process catalysed by the enzyme Dinitrogen Oxide reductase

Dinitrogen Oxide is a colorless, sweet-tasting gas. 
Dinitrogen Oxide is also known as "laughing gas". 
Continued breathing of the vapors may impair the decision making process. 
Dinitrogen Oxide is noncombustible but it will accelerate the burning of combustible material in a fire. 
Dinitrogen Oxide is soluble in water. 
Dinitrogen Oxide's vapors are heavier than air. 
Exposure of the container to prolonged heat or fire can cause it to rupture violently and rocket. 
Dinitrogen Oxide is used as an anesthetic, in pressure packaging, and to manufacture other chemicals.

Dinitrogen Oxide, refrigerated liquid appears as a colorless liquid. 
Density 1.22 g / cm3 at its boiling point of -89°C. 

Dinitrogen Oxide (N2O), also called dinitrogen monoxide, laughing gas, or nitrous, one of several oxides of nitrogen, a colourless gas with pleasant, sweetish odour and taste, which when inhaled produces insensibility to pain preceded by mild hysteria, sometimes laughter.
A principal use of Dinitrogen Oxide is as an anesthetic in surgical operations of short duration; prolonged inhalation causes death. 
The gas is also used as a propellant in food aerosols.

Dinitrogen Oxide is a colourless gas that is commonly used for sedation and pain relief, but is also used by people to feel intoxicated or high.1

Dinitrogen Oxide is commonly used by dentists and medical professionals to sedate patients undergoing minor medical procedures.
Dinitrogen Oxide is also a food additive when used as a propellant for whipped cream, and is used in the automotive industry to enhance engine performance. 
Dinitrogen Oxide is also increasingly being used to treat people withdrawing from alcohol dependence. 
Dinitrogen Oxide is classified as a dissociative anaesthetic and has been found to produce dissociation of the mind from the body (a sense of floating), distorted perceptions and in rare cases, visual hallucinations

How is Dinitrogen Oxide used?
The gas is inhaled, typically by discharging nitrous gas cartridges (bulbs or whippets) into another object, such as a balloon, or directly into the mouth.
Inhaling Dinitrogen Oxide produces a rapid rush of euphoria and feeling of floating or excitement for a short period of time

PHYSICAL PROPERTIES OF DINITROGEN OXIDE:

-Molecular Weight: 44.013    

-Exact Mass: 44.001062628    

-Monoisotopic Mass: 44.001062628    

-Topological Polar Surface Area: 19.1 Ų    

-Form: gas

-Odor: Slightly sweetish

-Taste: Slightly sweetish

-Boiling Point: -88.46 °C

-Melting Point: -90.8 °C

-Solubility: Slightly soluble in water

-Density: 1.266 

-Vapor Density: 1.53

-Vapor Pressure: 51.3 atm

-Viscosity: 0.0145 cP

-Heat of Vaporization: 16.54 kJ/mol

-Surface Tension: 1.75 dynes/cm

-Ionization Potential: 12.89 eV

-Refractive Index: 1.000516

Dinitrogen Oxide—also called by various names such as hyponitrous acid anhydride, dinitrogen oxide, nitrogen monoxide, and factitious air—is the chemical compound represented as N2O; that is, composed of two atoms of nitrogen (N) and one atom of oxygen (O). 
Under normal temperatures and pressures, Dinitrogen Oxide is a non-flammable, colorless, and almost odorless gas that has a mildly sweet odor and taste. 
Besides Dinitrogen Oxide, the other oxides of nitrogen (gaseous mixtures of nitrogen and oxygen) are nitric oxide (NO), nitrogen dioxide (NO2), and nitrogen pentoxide (N2O5).
In nature, Dinitrogen Oxide is found in trace amounts within Earth's atmosphere due to the chemical reactions between nitrogen and oxygen. 
Dinitrogen Oxide is considered a greenhouse gas, with a regarded impact on global warming third to that of carbon dioxide (CO2) and methane (CH4). 
In addition, Dinitrogen Oxide is artificially produced by heating solid ammonium nitrate (NH4NO3).

Dinitrogen Oxide is commonly known as laughing gas due to the exhilarating effects of inhaling it.
Dinitrogen Oxide is used in surgery and dentistry for its anaesthetic and analgesic effects.
Dinitrogen Oxide is present in the atmosphere where it acts as a powerful greenhouse gas.

Dinitrogen Oxide is a colorless and odorless substance that’s also known as “laughing gas.”
When inhaled, the gas slows down the body’s reaction time. 
This results in a calm, euphoric feeling.

CHEMICAL PROPERTIES OF DINITROGEN OXIDE:

-Heavy Atom Count: 3    

-Formal Charge: 0    

-Complexity: 25.8    

-Isotope Atom Count: 0    

-Defined Atom Stereocenter Count: 0    

-Undefined Atom Stereocenter Count: 0    

-Defined Bond Stereocenter Count: 0    

-Undefined Bond Stereocenter Count: 0    

-Covalently-Bonded Unit Count: 1    

-Compound Is Canonicalized: Yes

-Color: Colorless

-XLogP3-AA: 0.5    

-Hydrogen Bond Donor Count: 0    

-Hydrogen Bond Acceptor Count: 2    

-Rotatable Bond Count: 0    

-LogP: 0.36

-Stability/Shelf Life: Stable under recommended storage conditions.

-Decomposition: This compound decomposes explosively at high temperatures.

STORAGE OF DINITROGEN OXIDE:

Dinitrogen Oxide should be stored in a dry environment.
Dinitrogen Oxide should be kept away from substances that react rapidly with gases.
Dinitrogen Oxide should be kept in a clean environment.

Dinitrogen Oxide should be stored in sturdy, durable cylinders.
Dinitrogen Oxide should be stored under 745 psi pressure.

Dinitrogen Oxide should be stored in blue steel cylinders as a colorless liquid.
Dinitrogen Oxide Can be stored at room temperature at 50 atm
The tank maintains this pressure until it is empty.

SYNONYMS:

nitrous oxide
Dinitrogen oxide
Dinitrogen monoxide
Laughing gas
Nitrogen oxide
Nitrogen oxide (N2O)
Factitious air
Hyponitrous acid anhydride
Nitrogen hypoxide
Stickdioxyd
oxyde nitreux
Oxido nitroso
protoxyde d'azote
Nitrous oxide, compressed
Lachgas
gaz hilarant
Diazyne 1-oxide
Distickstoffmonoxid
Stickstoff(I)-oxid
Nitrous oxide, refrigerated liquid
nitrogenium oxydulatum
Nitrous oxide (TN)
Nitrous oxide [Anaesthetics, volatile]
oxidodinitrogen(N--N)
Stickdioxyd [German]
Nitrous oxide [JAN]
Oxide, Nitrous
Gas, Laughing
Oxido nitroso [Spanish]
Protoxyde d'azote [French]
Nitrous oxide [USP:JAN]
Nitrous oxide (JP15/USP)
Nitrious oxide
Nitrous oxide [UN1070] [Nonflammable gas]
Diazyne 1-oxide #
1,2-Diazaethyne1-oxide
Nitrous oxide, JAN, USAN
Nitrous oxide (JP17/USP)