1712-64-7 Usage
Description
Isopropyl nitrate is a colorless liquid with a pleasant odor, characterized by its density being greater than water and insolubility in water. It has a flash point ranging from 32 to 73°F and is known to spontaneously decompose and explode when exposed to fire or heat for extended periods. Additionally, it produces toxic oxides of nitrogen during combustion.
Uses
Used in Diesel Industry:
Isopropyl nitrate is used as a diesel cetane improver, enhancing the combustion efficiency and reducing emissions in diesel engines.
Used in Explosives Research:
Isopropyl nitrate serves as a monopropellant with a large detonation length scale, making it a suitable substitute for nitromethane in studying homogenous liquid explosives. This application allows for increased diagnostic resolution in explosive research.
Used in Chemical Synthesis:
Isopropyl nitrate is utilized in the synthesis of 1,2-dimethoxy-4-(nitromethyl)benzene, a nitro alkane derivative. Isopropyl nitrate can be further converted to the corresponding carboxylic acid in a continuous flow reactor using the Nef oxidation method, contributing to the production of various chemical products.
Air & Water Reactions
Highly flammable. Insoluble in water.
Reactivity Profile
Organonitrates, such as Isopropyl nitrate , range from slight to strong oxidizing agents. If mixed with reducing agents, including hydrides, sulfides and nitrides, they may begin a vigorous reaction that culminates in a detonation. Nitroalkanes are milder oxidizing agents, but still react violently with reducing agents at higher temperature and pressures. Nitroalkanes react with inorganic bases to form explosive salts. The presence of metal oxides increases the thermal sensitivity of nitroalkanes. Nitroalkanes with more than one nitro group are generally explosive. Contact with either strong oxidizers or with combustibles may cause fires and explosions.
Hazard
Oxidizing material, fire risk in contact with
organic materials.
Health Hazard
May cause toxic effects if inhaled or absorbed through skin. Inhalation or contact with material may irritate or burn skin and eyes. Fire will produce irritating, corrosive and/or toxic gases. Vapors may cause dizziness or suffocation. Runoff from fire control or dilution water may cause pollution.
Fire Hazard
HIGHLY FLAMMABLE: Will be easily ignited by heat, sparks or flames. Vapors may form explosive mixtures with air. Vapors may travel to source of ignition and flash back. Most vapors are heavier than air. They will spread along ground and collect in low or confined areas (sewers, basements, tanks). Vapor explosion hazard indoors, outdoors or in sewers. Runoff to sewer may create fire or explosion hazard. Containers may explode when heated. Many liquids are lighter than water.
Check Digit Verification of cas no
The CAS Registry Mumber 1712-64-7 includes 7 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 4 digits, 1,7,1 and 2 respectively; the second part has 2 digits, 6 and 4 respectively.
Calculate Digit Verification of CAS Registry Number 1712-64:
(6*1)+(5*7)+(4*1)+(3*2)+(2*6)+(1*4)=67
67 % 10 = 7
So 1712-64-7 is a valid CAS Registry Number.
InChI:InChI=1/C3H7NO3/c1-3(2)7-4(5)6/h3H,1-2H3
1712-64-7Relevant articles and documents
Kinetics of the C3H7O2 + NO reaction: Temperature dependence of the overall rate constant and the i-C3H7ONO2 branching channel
Chow, Jessica M.,Miller, Angela M.,Elrod, Matthew J.
, p. 3040 - 3047 (2003)
The temperature dependence of the overall rate constant for the C3H7O2 + NO reaction and the rate constant for the minor branching-channel resulting in the production of i-C3H7ONO2 have been measured using the turbulent flow technique with high-pressure chemical ionization mass spectrometry for the detection of reactants and products. The temperature dependence of the overall rate constant for the C3H7O2 + NO reaction was investigated between 298 and 213 K at 100 Torr pressure, and the data were fit by the following Arrhenius expression (with 2 standard deviation error limits indicated): 43-0.9+1.0 x 10-12 exp[(268 ± 56)/T] cm3 molecule-1 s-1. This expression agrees well with previous isomer-specific measurements of the n-C3H7ONO2 and i-C3O2 + NO rate constants made at lower pressures. The temperature dependence of the rate constant for the minor reaction channel i-C3H7O2 + NO → i-C3H7ONO2 was investigated between 298 and 213 K at 100 Torr pressure. The following Arrhenius expression was determined for the minor channel: 4.9-2.9+5.3 × 10-16 exp[(1380 ± 230)/T] cm3 molecule-3 s-1. The Arrhenius expressions for the overall rate and the i-C3H7ONO2 producing channel indicate a branching ratio of about 0.006 at 298 K and 0.020 at 213 K at 100 Torr pressure, which is in good agreement with the predictions of a recently revised empirical model for alkyl nitrate branching ratios.
Nitration of alcohols by nitryl fluoride
Fedorov,Eremenko
, p. 1022 - 1023 (1997)
A general method for the preparation of nitrates by treatment of alcohols with nitryl fluoride (FNO2) in MeCN in the presence of KF has been developed.
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Steinberger et al.
, p. 4748 (1955)
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Rates of Reaction between the Nitrate Radical and Some Aliphatic Alcohols
Langer, Sarka,Ljungstroem, Evert
, p. 405 - 410 (1995)
Rate coefficients for the gas-phase reaction of NO3 with methanol, ethanol and propan-2-ol have been determined.Absolute rates were measured at temperatures between 258 and 367 K using the fast flow-discharge technique.The measured rate coefficients (in units of 1E-15 cm3 molecule-1 s-1) at 295 K are: 0.132+/-0.024, 1.37+/-0.10 and 3.13+/-0.64 for methanol, ethanol and propan-2-ol, respectively.The temperature dependence of the rate coefficients can be expressed as Arrhenius equations: kmethanol = (1.06+/-0.51) E-12exp, kethanol = (6.99+/-1.21)E-13 exp and kpropan-2-ol = (1.54+/-0.75)E-12 exp (in units cm3 molecule-1 s-1).An attempted product study, using N2O5 as the NO3 source, failed since the alcohols react with N2O5, producing alkyl nitrates.The estimated upper limit for rate coefficients for reaction of N2O5 with methanol, ethanol and propan-2-ol at 296 K in the gas phase were (2.0+/-1.0)E-19, (3.9+/-2.0)E-19 and (4.8+/-2.5)E-19 cm3 molecule-1 s-1, respectively.The error limits correspond to the 95percent-confidence interval.