543-67-9

Basic information

• Product Name: N-PROPYL NITRITE
• Synonyms: n-C3H7ONO;Nitrous acid, n-propyl ester;Nitrous acid, propyl ester;nitrousacid,n-propylester;nitrousacid,propylester;nitrousacidpropylester;Propanol nitrite;propanolnitrite
• CAS NO: 543-67-9
• Molecular Formula: C₃H₇NO₂
• Molecular Weight: 89.09
• EINECS: 208-848-5
• Mol File: 543-67-9.mol

Chemical Properties

• Boiling Point: bp760 46-48°
• Flash Point: °C
• Appearance: /
• Density: d420 0.8864
• Vapor Pressure: 342mmHg at 25°C
• Refractive Index: nD20 1.3592; nD20 1.3613
• CAS DataBase Reference: N-PROPYL NITRITE(CAS DataBase Reference)
• NIST Chemistry Reference: N-PROPYL NITRITE(543-67-9)
• EPA Substance Registry System: N-PROPYL NITRITE(543-67-9)

Safety Data

• Hazardous Substances Data: 543-67-9(Hazardous Substances Data)

Usage

Uses

Used in Aerospace Industry:
N-PROPYL NITRITE is used as a jet propellant for its ability to provide the necessary thrust and energy for jet engines. Its properties make it a suitable choice for this application, despite its inherent risks.
Used in Chemical Industry:
N-PROPYL NITRITE is used as a solvent in the chemical industry, where its ability to dissolve certain substances makes it a valuable asset. Its use in this context is carefully managed due to its toxicity and flammability.
Used as a Dielectric Fluid:
In the electrical industry, N-PROPYL NITRITE is utilized as a dielectric fluid. Its properties allow it to effectively insulate and protect electrical components, making it a preferred choice for this application. However, its use is strictly regulated to ensure safety and minimize the risk of accidents.

Air & Water Reactions

Highly flammable.

Reactivity Profile

N-PROPYL NITRITE is an oxidizing agent. If mixed with reducing agents, including hydrides, sulfides and nitrides, may begin a vigorous reaction that culminates in a detonation. Reacts with inorganic bases to form explosive salts.

Health Hazard

TOXIC; inhalation, ingestion or contact (skin, eyes) with vapors, dusts or substance may cause severe injury, burns or death. Reaction with water or moist air will release toxic, corrosive or flammable gases. Reaction with water may generate much heat that will increase the concentration of fumes in the air. Fire will produce irritating, corrosive and/or toxic gases. Runoff from fire control or dilution water may be corrosive and/or toxic and cause pollution.

Fire Hazard

Non-combustible, substance itself does not burn but may decompose upon heating to produce corrosive and/or toxic fumes. Vapors may accumulate in confined areas (basement, tanks, hopper/tank cars etc.). Substance will react with water (some violently), releasing corrosive and/or toxic gases and runoff. Contact with metals may evolve flammable hydrogen gas. Containers may explode when heated or if contaminated with water.

InChI:InChI=1/C3H7NO2/c1-2-3-6-4-5/h2-3H2,1H3

Upstream product

• 71-23-8 propan-1-ol 
• 106-94-5 propyl bromide 
• 107-08-4 1-iodo-propane 
• 16499-18-6 propyloxyl 
• 74-98-6 propane 
• 627-13-4 propyl nitrate 
• 563-28-0 sulfuric acid monopropyl ester; potassium-salt 

Downstream Products

• 598-05-0 di-1-propyl sulfate 
• 107-10-8 propylamine 
• 123-38-6 propionaldehyde 
• 50-00-0 formaldehyd 
• 108-03-2 1-Nitropropane 
• 107-12-0 propiononitrile 
• 15216-10-1 N-nitrosoazetidine 
• 71-23-8 propan-1-ol 
• 930-55-2 N-nitrosopyrrolidine 
• 100-75-4 N-nitrosopiperidine 
• 59-89-2 N-nitrosomorpholine 
• 20917-49-1 N-nitrosoheptamethyleneimine 
• 16339-07-4 1-methyl-4-nitroso-piperazine 
• 1956-45-2 2-acetylthiophene oxime 

Relevant articles and documents

Method and device for continuously preparing alkyl nitrite through channelization

The invention discloses a method and device for continuously preparing alkyl nitrite through channelization. The method comprises the following steps: storing alkyl alcohol and concentrated HCl aqueous solution in a first container and storing sodium nitrite aqueous solution in a second container; continuously conveying the solution in the first container and the second container into a static mixer for mixing by a first metering pump and a second metering pump respectively, enabling mixed solution to continuously enter a tubular reactor for reaction at the temperature of -20 DEG C-5 DEG C for1-250s, enabling feed liquid after reaction to enter a liquid separation tank and performing aftertreatment on the feed liquid in the liquid separation tank, so as to obtain alkyl nitrite. The preparation method disclosed by the invention has the advantages of being good in process safety and easy in control of reaction conditions, achieving continuous production, being high in product yield andachieving large-scale production only through less investment in the industry.

Process for Producing C1-C4 Alkyl Nitrite

A process of producing C1-C4 alkyl nitrite, comprising the following steps: a) firstly feeding nitrogen oxide and oxygen into Reactor I, contacting with an aluminosilicate catalyst, and reacting to produce an effluent I containing NO2 and unreacted NO; b) feeding the effluent I and C1-C4 alkanol into Reactor II, and reacting to produce an effluent II containing C1-C4 alkyl nitrite; and c) separating the effluent II containing C1-C4 alkyl nitrite to obtain C1-C4 alkyl nitrite; wherein reactor I is a fixed bed reactor, and Reactor II is a rotating high-gravity reactor; said nitrogen oxide in step a) is NO, or a mixed gas containing NO and one or more of N2O3 and NO2, wherein the molar number of NO is greater than that of NO2, if any; and the molar ratio of NO in nitrogen oxide to oxygen is 4-25:1.

Process for Producing Cl-C4 Alkyl Nitrite

The present invention relates to a process for producing C1-C4 alkyl nitrite, comprising loading a resin catalyst layer and/or a porous filler layer into a reactor, passing nitrogen oxide, oxygen and C1-C4 alkanol as raw materials through the resin catalyst layer and/or porous filler layer in a counter current, parallel current or cross current manner, reacting under the conditions including a reaction temperature of from 0 to 150° C., a reaction pressure of from ?0.09 to 1.5 MPa, a molar ratio of C1-C4 alkanol/nitrogen oxide of 1-100:1, a molar ratio of nitrogen oxide/oxygen of 4-50:1, to obtain an effluent containing C1-C4 alkyl nitrite, wherein said nitrogen oxide is NO, or a mixed gas containing NO and one or more selected from N2O3 and NO2.

NEW METHOD FOR THE MANUFACTURE OF THERAPEUTIC COMPOUNDS AND COMPOSITIONS, COMPOUNDS AND COMPOSITIONS PRODUCED THEREWHITH, AND THEIR USE

Organic nitrites can be produced from a compound which is a mono/polyhydric alcohol or an aldehyde- or ketone-derivate thereof after de-aeration of the same, using NO gas, and stored in an environment saturated with gaseous NO. Organic nitrites produced according to the invention exhibit less impurities and improved storage stability compared to conventionally produced nitrites. The organic nitrites of the invention can easily be formulated into pharmaceutical compositions and have utility for the treatment of various conditions.

Gas phase kinetics of the reaction system of 2NO2 ? N 2O4 and simple alcohols between 293-358 K

The reversible reactions between nitrogen dioxide and alcohols (CH 3OH, CH3CH2OH, CH3CH 2CH2OH, CH3CHOHCH3) have been studied in the gas phase, using the spectrophotometric method. RONO (R = CH 3, CH3CH2, CH3CH2CH 2, CH3CHCH3) were identified by UV spectra. The equilibrium constants as well as the bimolecular rate constants were determined by computer modeling, using the programme MINICHEM. We calculated the following values for the forward rate constants k3av: (3.0±0.9)×10-18, (8.0±2.4)×10 -18, (5.4±1.6)×10-18, (2.0±0.6) ×10-18 cm3 molec-1 s-1 and the equilibrium constants Kav: 100±30, 40±12, 109±33, 39±12 at 298 K for the reactions with methanol, ethanol, 1-propanol and 2-propanol, respectively. The temperature dependence of the rate constants and the equilibrium constants were studied and it allowed to obtain the activation energy for the forward and for the reverse reaction, as well as thermochemical parameters. The equilibrium constants and the rate constants suggest that symmetrical N2O4 is the reactive species.

Dispersed fluorescence spectroscopy of primary and secondary alkoxy radicals

Dispersed fluorescence (DF) spectra of 1-propoxy, 1-butoxy, 2-propoxy, and 2-butoxy radicals have been observed under supersonic jet cooling conditions by pumping different vibronic bands of the B-X laser induced fluorescence excitation spectrum. The DF spectra were recorded for both conformers of 1-propoxy, three conformers of the possible five of 1-butoxy, the one possible conformer of 2-propoxy, and two conformers of the possible three of 2-butoxy. Analysis of the spectra yields the energy separations of the vibrationless levels of the ground X and low-lying A electronic state as well as their vibrational frequencies. In all cases, the vibrational structure of the DF spectra is dominated by a CO stretch progression yielding the vco stretching frequency for the X state and in most cases for the A state. In addition to the experimental work, quantum chemical calculations were carried out to aid the assignment of the vibrational levels of the X state and for some conformers the A state as well. Geometry optimizations of the different conformers of the isomers were performed and their energy differences in the ground states were determined. The results of the calculation of the energy separations of the close-lying X and A states of the different conformations are provided for comparison with the experimental observations.

Atmospheric fate of alkoxy radicals: Branching ratio of evolution pathways for 1-propoxy, 2-propoxy, 2-butoxy and 3-pentoxy radicals

As the last step of VOC oxidation in the atmosphere, the evolution of alkoxy radicals determines the nature and the concentration of the secondary compounds formed. Branching ratios between decomposition and reaction with O2 of 1-propoxy, 2-propoxy, 2-butoxy, and 3-pentoxy radicals were measured at room temperature and 1 atm in a simulation chamber using FTIR spectroscopy as an analytical device. The ratio varied depending on the leaving alkyl group and the class of alkoxy. No additional decomposition due to excited radicals was observed. The results could be used directly for tropospheric simulation purposes. Formaldehyde might be a photolytic source of HOx through the production of H and HCO radicals and acetaldehyde is the key precursor of the toxic NOx reservoir, peroxy-acetyl nitrate. In the lower troposphere, 1-propoxy and 2-propoxy radicals react mainly with O2 while decomposition is an important reaction pathway for 2-butoxy and 3-pentoxy. Consequently, C1 and C2 aldehyde production from the two longer chain alkoxys will occur very close to the area of initial VOC oxidation, while for the alkoxys exhibiting a minor decomposition pathway, the formaldehyde or acetaldehyde production will take place after oxidation of all the intermediate secondary compounds, far from the emission area of the primary compound.

Rate constants for the reactions of C2H5O, i-C3H7O, and n-C3H7O with NO and O2 as a function of temperature

The rate constants of the reactions of ethoxy, i-propoxy and n-propoxy radicals with O2 and NO was investigated as function temperature. The radicals were generated by laser photolysis from the appropriate alkyl nitrite and characterized by laser-induced fluorescence. For the reactions with O2, the ethoxy radical reacted somewhat slower than recently recommended. The values obtained for i- and n-propoxy had been combined with the measurements from a recent study at lower temperatures, allowing a more reliable determination of the Arrhenius parameters.

LIF spectra of n-propoxy and i-propoxy radicals and kinetics of their reactions with O2 and NO2

Fluorescence excitation spectra of CH3CF2CH2O (n-propoxy) and (CH3)2CHO (i-propoxy) radicals were obtained using a combined laser photolysis/laser-induced fluorescence (LIF) technique and the kinetics of reactions of these radicals with (1) O2 as a function of temperature and with (2) NO2 as a function of pressure have been determined. Propoxy radicals were produced by excimer laser photolysis of the appropriate propyl nitrites at γ=351 nm. The spectra of the (A?←X?) transitions show progressions of the CO-stretching vibration in the electronically excited states with spacings of the bands of (560±10)cm-1 for i-propoxy and (580±10)cm-1 for n-propoxy. Fluorescence spectra taken after excitation in the (4,0) band at λ=340.1 nm (i-propoxy) and in the (1,0) band at λ=342.4 nm (n-propoxy) show progressions of the CO-stretching vibration in the electronic ground state of (900±60) cm-1 for i-propoxy and (1000±50) cm-1 for n-propoxy. The Arrhenius expressions for the ractions of n-propoxy and i-propoxy with O2 have been determined to be k1 (n) = (1.4±0.6)×10-14 exp (-(0.9±0.5) kJ mol-1/RT) cm3 s-1 and kt (i) = (1.0±0.3)×10-14 exp (-(1.8±0.4) kJ mol-1/RT) cm3 s-1 in the range 218-313 K. The rate coefficients for the reactions of NO2 with n-propoxy and i-propoxy at T=296 K were found to be independent of total pressure with k2(n)=(3.6±0.4)×10-14 cm3 s-1 (6.7-53 mbar) and k2(i)=(3.3±0.3)×10-11 cm3 s-1 (6.7-106 mbar). WILEY-VCH Verlag GmbH, 1998.

Reaction of alcohol with NO2 on a Cleaned Glass Surface

Formation of alkyl nitrite from alcohol and NO2 was very fast on a Pyrex glass surface cleaned with chromic acid mixture.The reaction was practically zero order with respect to NO2.The rate constant was (1.7 +/- 0.08)*10E-18 cm3*molecule-1*s-1 for methyl nitrile formation and the apparent activation energy was -53.5 kJ*mol-1.