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Chemical Reference Guide
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Description
Nitrous oxide at room temperature and atmospheric pressure is a colorless gas with a barely
perceptible sweet odor and taste. It is nonflammable but will support combustion. At elevated
temperatures, nitrous oxide decomposes into nitrogen and oxygen. Decomposition in the absence
of catalysts is negligible at temperatures below 1200°F (649°C). Nitrous oxide is moderately soluble
in water, alcohol, and oils. Unlike some higher oxides of nitrogen, nitrous oxide does not affect the
acidity of water solutions.
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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 Pharmacopoeia/National Formulary. [1]CGA G-8.2,
Commodity Specification for Nitrous Oxide, describes the requirements for particular grades of
nitrous oxide. [2] Other specifications to meet particular requirements are available from suppliers.
Table l, from CGA G-8.2, presents the component maxima, in parts per million (mole/mole) unless
otherwise shown, for specific grades of nitrous oxide, also known as quality verification levels. 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.
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Uses
The major use of nitrous oxide is for anesthesia and analgesia. It is also used for cryosurgery.
Nitrous oxide also finds use as an oxidizing gas for atomic absorption spectro photometry, a
propellant for pressure or aerosol products (whipped cream is most prevalent), and a fuel oxidant
for racing vehicles. Some products for this latter application are supplied with an additive to deter
abuse of the product. Nitrous oxide is also used in the manufacture of semiconductors.
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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 long-term exposure. The most strongly substantiated effect is neuropathy.
Epidemiological studies also suggest leto-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 long-term exposure effects, release of the product into
general work areas should be minimized. The National Institute for Occupational Safety and Health
(NIOSH) has recommended limits of 25 ppm for hospital operating rooms and 50 ppm for dental
offices measured on an eight-hour time-weighted average basis. Contact with liquid nitrous oxide
can freeze skin tissue and must be avoided. The American Conference of Governmental Industrial
Hygienists has adopted a time-weighted average threshold limit value of 50 ppm (90 mg/m3) for an
eight-hour workday exposure to nitrous oxide.
Warning: 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 life-sustaining
decisions.
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Materials of Construction
Nitrous oxide is non-corrosive 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 of some elastomers.
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Safe Storage, Handling, and Use
Nitrous oxide will support combustion. It must be kept away from oil, grease, and other combustible
materials. Never permit oil, grease or any other readily combustible substance to come in contact
with cylinders or other equipment containing nitrous oxide.
Store and use nitrous oxide with adequate ventilation. Containers that become exposed to fire,
including bulk storage tanks, could rupture violently if subject to localized heating.
See Chapter 5 for general guidelines concerning the safe storage and handling of compressed
gases, including nitrous oxide. Detailed recommendations for nitrous oxide storage locations are
given in CGA G-8.1, Standard for Nitrous Oxide Systems at Consumer Sites. Requirements for
nitrous oxide systems in hospitals and other health care facilities are found in NFPA 99, Standard
for Health Care Facilities.
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Disposal
Nitrous oxide is not harmful to the environment and can be released to the atmosphere, provided
ventilation is adequate for protection of personnel in the immediate vicinity of the release point. Do
not release in the vicinity of building air intakes.
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Handling Leaks and Emergencies
Turn off ignition sources in the general area of the leak if possible. Nitrous oxide is nonflammable
but is an oxidizer which can cause or intensify fires. Evacuate the area to prevent asphyxiation.
Use self-contained breathing apparatus to enter the area. Provide as much ventilation as possible.
Avoid contact with liquid spills. Contact supplier for assistance.
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First Aid
People acutely exposed to high levels of nitrous oxide should be immediately removed from
exposure, after which symptoms should rapidly reverse. If obtundation (dulling or blunting of
sensitivity, such as to pain) is present, oxygen should be administered. Mechanical ventilation
should be instituted in the event of respiratory arrest. Vomiting may occur as the person awakes. In
order to prevent aspiration, exposed individuals should be placed on their side with their head at
the level of or slightly lower than their body.
Editor’s note: The following was extracted from the 1996 Grollier’s Encylopedia CD for Macintosh
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Oxygen
Oxygen is a gaseous chemical element in Group VA of the periodic table. The chemical symbol for
atomic oxygen is O, its atomic number is 8, and its atomic weight is 15.9994.Elemental oxygen is
known principally in the gaseous form as the diatomic molecule, which makes up 20.95% of the
volume of dry air. Diatomic oxygen is colorless, odorless, and tasteless.
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Physical and Chemical Properties
Three naturally occurring isotopes of oxygen have been found: one with mass 16 (99. 759%of all
oxygen), one with mass 17 (0.037%); and one with mass 18 (0.204%). The rarer isotopes,
principally the latter, find their major use in labeling experiments used by scientists to follow the
steps of chemical reactions.
If oxygen at a pressure of one atmosphere is cooled, it will liquefy at 90.18 K (-182.97 deg C;
-297.35 deg F), the normal boiling point of oxygen, and it will solidify at 54.39 K (-218.76 deg C;
-361.77 deg F), the normal melting point of oxygen. The liquid and solid forms of oxygen have a
pale blue color. Several different structures are known for solid oxygen: solid type III, from the
lowest temperatures achievable to 23.66 K; type II, from 23.66 to 43.76 K; and type I,from 43.76 to
54.39 K. The critical temperature for oxygen, the temperature above which it is impossible to liquefy
the gas no matter how much pressure is applied, is 154.3 K (-118.9 deg C; -181.9 deg F). The
pressure of liquid and gaseous oxygen coexisting in equilibrium at the critical temperature is 49.7
atmospheres.
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Molecular diatomic oxygen is a fairly stable molecule requiring a dissociation energy (the energy
required to dissociate one mole of molecular oxygen in its ground state into two moles of atomic
oxygen in its ground state) of 493.6 kilojoules per mole. The molecule is dissociated by ultraviolet
radiation of any wavelength shorter than 193 nm. Solar radiation striking stratospheric oxygen
dissociates it into atomic oxygen for this reason. The atomic oxygen formed in this fashion is
capable of reacting with oxygen to form ozone.
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Corrosion
Many direct, uncatalyzed reactions of oxygen do not occur rapidly at room temperature. This fact
has a number of important consequences. One of these consequences has to do with the use of
metals as structural materials. Metals that are used in construction, such as iron (principally as
steel) and aluminum, form highly stable oxides. For example, the oxidation of aluminum has a
significant tendency to occur. However, in spite of this tendency, the reaction occurs so slowly at
room temperature that it can be said for most practical purposes not to occur at all, and for this
reason aluminum is an appropriate and widely used structural material. The slowness of this
reaction is due in part to the stability of the oxygen-oxygen bond and in part because of a very thin,
protective layer of oxide that forms on the surface of the aluminum. The oxidation of iron is a
complex process involving impurities in the iron, as well as water and carbon dioxide. This oxidative
destruction, or rusting, of iron and steel—which are among our most important structural materials—
is extremely costly to modern societies.
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Reactivity
There is a marked difference between the rates of reactions with oxygen at room temperature and
the rates at elevated temperatures. Many substances that do not react rapidly with oxygen in air at
temperatures below 100 degrees C will do so at 1000 degrees C with a strong evolution of heat
(exothermically). For example, coal and petroleum can be stored indefinitely at the temperatures
encountered under normal climatic conditions, but they readily oxidize, exothermically, at elevated
temperatures.
The most common compounds of oxygen are those in which the element exhibits a valence of two.
This fact is associated with the electronic structure of atomic oxygen; this atom requires two
additional electrons to fill its outermost energy level. Examples of divalent oxides are numerous
among well-known substances such as water; carbon dioxide; aluminum oxide; silicon dioxide; the
silicates, calcium carbonate or limestone; and sulfur dioxide. Oxygen is also known to have other
valences, such as in the peroxides, of which hydrogen peroxide is an example.
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The direct reaction of oxygen with another element frequently follows the pattern discussed above;
that is, it does not occur rapidly or at all at room temperature but is strongly exothermic, and once
oxidation is initiated the evolved heat raises the temperature of the reactants such that the reaction
is self-sustaining. Examples of such reactions are with the elements magnesium, carbon, and
hydrogen. Magnesium and carbon burn in air once the reaction is initiated, and a hydrogen-oxygen
mixture can react explosively when the reaction is initiated by a flame or spark. The explosion of a
hydrogen-oxygen mixture is an extremely fast reaction and occurs because of the formation of
atomic oxygen in the exploding mixture.
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Uses
Pure oxygen is used extensively in technological processes. It is used in the welding, cutting, and
forming of metals, as in oxyacetylene welding, in which oxygen reacts with acetylene to form an
extremely hot flame. Oxygen is added to the inlet air (3 to 5%) in modern blast furnaces to increase
the temperature in the furnace; it is also used in the basic oxygen converter for steel production, in
the manufacture of chemicals, and for rocket propulsion.
Oxygen is also used in the partial combustion of methane (natural gas) or coal (taken here to be
carbon) to make mixtures of carbon monoxide and hydrogen called synthesis gas, which is in turn
used for the manufacture of methanol. Processes in which combustible liquids are produced from
coal will become increasingly important as petroleum resources become further depleted.
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Nitrous Oxide at a Glance
Chemical Symbol: N20
Synonyms: Nitrogen monoxide, dinitrogen monoxide, laughing gas
CAS Registry Number: 10024-97-2
DOT Classification: Nonflammable gas
DOT Label: Nonflammable gas
Transport Canada Classification: 2.2
UN Number: UN 1070 (liquefied gas); UN 2201 (refrigerated liquid)
PHYSICAL CONSTANTS
U.S. Units SI Units
Chemical formula N2O N2O
Molecular weight 44.0128 44.0128
Specific volume
at 59°F (15°C) and 1 atm 8.538 ft3/Ib 0.533 m3/kg
at 70°F (21-1°C) and 1 atm 8.726 ft3/lb 0.5447 m3/kg
Specific gravity of
the gas (air= 1) 1.5297 1.5297
Density of the gas
at 59°F (15°C) and 1 atm 0.1172 Ib/ft3 1.877 kg/m3
at 70°F (21.1°C) and 1 atm 0.1146 Ib/ft3 1.947 kg/m3
Critical density 28.15 Ib/ft3 450.4 kg/m3
Boiling point at 1 atm -127.4°F - 88.5°C
Latent heat of vaporization
at boiling point 161.8 Btu/Ib 376.1 kJ/kg
at 32°F (0°C) 107.5 Btu/Ib 249.9 kJ/kg
at 70°F (21-1°C) 77.7 Btu/Ib 180.6 kJ/kg
Latent heat of fusion
at triple point 63.9 Btu/Ib 148.5 kJ/kg
Specific heat of the gas
at 59°F (15°C) and 1 atm Cp 0.207 Btu/(Ib)(°F) 0.866 kJ/(kg)(°C)
at 59°F (150°C) and 1 Cv. 0.158 Btu/(Ib)(°F) 0.665 kJ/(kg)(°C)
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U.S. Units SI Units
Ratio of specific heats
at 59°F (15°C) and 1 atm Cp/Cv 1.303 1.303
Solubility in water, vol.and 1 atm
at 32°F (O°C) 1.3 1.3
at 68°F (20°C) 0.68 0.68
at 77°F (25°C) 0.59 0.59
Viscosity of the gas
at 32°F (O°C) 0.326 Ib/(ft)(hr) 0.135 x 10-3 Pa(s)
at 80°F (27°C) 0.359 Ib/(ft)(hr) 0.149 x 10-3 Pa(s)
Thermal conductivity of the
gas at 32°F (0°C) 0.0083 Btu (ft)/h(ft2)(°F) 0.0144 W/m(°C)
at 212°F (100°C) 0.0135 Btu (ft)/h(ft2)(°F) 0.0233 W/m(°C)
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Previous
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This has been a sample page from
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How To Install and Use Nitrous Oxide
Injection Systems For Maximum Horsepower
by Joe Pettitt
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Includes information on nitrous basics and advance
nitrous theory. Written with the assistance of Nitrous
Oxide Systems
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Nitrous oxide injection is one of the potentially easiest, least
expensive, and fastest ways to substantially increase engine
horsepower. This new title, authored with the assistance of one of
the industry's largest manufacturer of nitrous equipment, provides
the latest technical information available regarding the proper
installation and use of this high performance, yet potentially
damaging equipment.
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Click below to view sample
pages from each chapter.
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"How to Install and Use Nitrous Oxide is filled with information
on nitrous, including the basics of advanced nitrous theory.
Photos, charts, and graphs accompany the text and illustrate
key points. Hands-on sections of the book cover how to plumb
a nitrous system and how to set up an engine to handle nitrous.
There's information on ignition timing, compression, wiring,
solenoids, octane, and fuel delivery." -- SPORT TRUCK, April
1999
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Chap. 1 - Introduction to Nitrous
Chap. 2 - How Nitrous Works
Chap. 3 - The Nitrous System
Chap. 4 - Installation Tech
Chap. 5 - Operating and Tuning
Chap. 6 - Basic Engine
Chap. 7 - Advanced Tuning
Chap. 8 - Nitrous Fuel Injection
Chap. 9 - Dyno Sessions
Chap. 10 - Real World Project
Chap. 11 - Chemical Reference
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8-3/8 X 10-7/8
128 pages
300 b/w photos
Item: SA50
Price: $18.95
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Click here to buy now!
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This is a great book that anyone using, or considering using a
nitrous oxide system will love!
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