302-01-2 Usage
Chemical Description
Different sources of media describe the Chemical Description of 302-01-2 differently. You can refer to the following data:
1. Hydrazine is a reducing agent used for deprotection of chemical groups.
2. Hydrazine is a colorless, flammable liquid with a pungent odor that is used as a reducing agent and in the synthesis of various organic compounds.
3. Hydrazine is used in the synthesis of pyrazole 7.
Chemical Properties
Different sources of media describe the Chemical Properties of 302-01-2 differently. You can refer to the following data:
1. Hydrazine is a colorless flammable liquid with strong toxicity and instability, and combines easily in the air with water molecules to form hydrazine hydrate. It is also very important for industrial uses such as rocket fuel, photographic development, and in fuel cells.
Hydrazine is the simplest diamine in its class of compounds and may be thought of as derived from ammonia by replacement of a hydrogen atom by the – NH2 group. The hydrated hydrazine, N2H4.H2O was first prepared by Curtius in 1887. The anhydrous hydrazine as a water free base was prepared by De Bruyn for the first time. Preparation of hydrazine by the oxidation of NH3 with hypochlorite – a process that became the chief commercial method of manufacture was first demonstrated by Raschig.
2. HYDRAZINE, colorless, fuming liquid, decomposes when heated above 350 °C at atmospheric pressure into N2 and NH2, also decomposes in presence of a catalyst (e.g., platinum) into N2 and NH3. Hydrazine burns when ignited in air with a violet-colored flame. The compound is soluble in all proportions with H2O and is soluble in alcohol. Hydrazine forms a hydrate with one molecule of H2O. Upon moderate heating or in a vacuum, the hydrate yields hydrazine and H2O. Hydrazine is a base slightly weaker than NH4OH.
3. colourless oily liquid
Uses
Different sources of media describe the Uses of 302-01-2 differently. You can refer to the following data:
1. Hydrazine is mostlyed used as a blowing agent in preparing polymer foams. It is mainly used as rocket fuels, boiler water treatments, chemical reactants, medicines, and in cancer research.
2. Hydrazine is used as a high-energy rocket fuel, as a
reducing agent, and for preparing organic hydrazine derivatives.
The propellant grade of commercial hydrazine is more
than 97.7% active. It is also used as an oxygen scavenger in
boiler water. Hydrazine has also been used as an experimental
drug for treating tuberculosis and sickle cell anemia.
3. Reducing agent for many transition metals and
some nonmetals (arsenic, selenium, tellurium), as
well as uranium and plutonium; corrosion inhibitor
in boiler feedwater and reactor cooling water;
waste water treatment; electrolytic plating of metals on glas
4. Hydrazine is a highly reactive base and powerful reducing
agent. It acts as an oxygen scavenger and is highly reactive with
other chemicals. Hydrazine has a number of uses including, as
a chemical precursor to blowing agents (e.g., azodicarbonamide
and azobisisobutyronitrile), in the organic synthesis of
pharmaceuticals and pesticides (e.g., isoniazid, fluconazole,
and 3-amino-1,2,4-triazole), as a missile and rocket propellant
(e.g., used in the F-16 fighter), as a gas-forming agent in air bags
(e.g., sodium nitrite), as a corrosion inhibitor and reducing
agent in large industrial boilers, and as a fuel source in fuel
cells.
Production
The industrial production of hydrazine always applies Raschin method. In October 1981, the French company Jürgen-Coleman successfully studied the imine hydrogen peroxide oxidation method, which is a promising method of production. Raschin uses ammonia and sodium hypochlorite as raw materials, followed by chlorination and amination to obtain hydrazine: ammonia and sodium hypochlorite are sent into the reactor in 1: 3 (molar ratio) with reaction generating chloramines. Chloramine can react with anhydrous ammonia to generate hydrazine in the hydrazine reactor. We can also use urea as the raw material to have it reacted with sodium hypochlorite-sodium hydroxide solution in the presence of a potassium permanganate catalyst (see hydrazine hydrate, [7803-57-8]).
The dehydrating agent method mixes caustic soda and 50% ~ 54% hydrazine hydrate (the mass ratio is 10: 8), gradually send nitrogen to remove air and heats the alkaline temperature to 118 DEG C. After the caustic soda is completely dissolved, cool to around 60℃, apply vacuum distillation to a distillate containing hydrazine content of 90% to 94%, followed by fractional distillation to remove water, condensation to obtain 98% to 99.5% of anhydrous hydrazine.
Extraction dehydration method: hydrazine hydrate solution can subject to fractionation to distill out of water to until the water and hydrazine become azeotropic (68% hydrazine); the solution is subject to secondary fractionation; add aniline to change its boiling point and distill the aniline and water off from the water; the recovered aniline can be for recycling use; the secondary fractionation solution is further subject to three times fractionation to obtain anhydrous hydrazine.
Description
Hydrazine sulphate, hydrobromide and hydrochloride
have been reported to be occupational sensitizers,
mainly in soldering flux.
Physical properties
Colorless, mobile, fuming liquid; ammoniacal odor; density 1.0045 g/mL at25°C; refractive index 1.46044 at 22°C; solidifies at 2°C to a white crystallinesolid; boils at 113.5°C; flash point 52°C; burns with a violet flame; vapor pres-sure 14.4 torr at 25°C; critical temperature 379.85°C; critical pressure 145atm; surface tension 66.67 dyne/cm at 25°C; dielectric constant 51.7 at 25°C;viscosity 0.876 centipoise at 25°C; very soluble in water; forms an azeotropewith water at molar composition of 58.5% hydrazine: 41.5% water (71.48%:28.52% by weight), the azeotrope with water boils at 120.5°C; forms hydrazinehydrate at 1:1 molar concentration in water; soluble in alcohols and other polar solvents; pKa 8.1 at 25°C.
History
Hydrazine was isolated first as a sulfate salt by Curtius in 1887. Earlier, in1875, Fischer prepared and identified the organic derivatives of hydrazine.Raschig in 1906 prepared hydrazine by hypochlorite oxidation of ammonia.Hydrazine and its derivatives have numerous commercial applications. Itwas used initially as rocket propellant. During World War II, it was used as afuel for rocket-powered fighter planes. However, the most important applications of hydrazine and its derivatives at present are: as blowing agents; forinsect control; in pharmaceuticals; in water treatment; and in fuel cells.Hydrazine derivatives release nitrogen on decomposition, producing foamingaction in polymers to form pores or cells. A large number of hydrazine derivatives are used in agricultural applications as fungicides, herbicides, and pesticides for weed and pest control. A few hydrazide drugs, such as isoniazid [54-85-3] are used extensively for treating tuberculosis. Other applications ofhydrazine include its use in fuel cells; and in wastewater treatment forremoval of iron; iron removal from hot-water heating systems; reduction ofred iron oxide rust into magnetite; and for removal of oxygen to protectagainst corrosion. It also is used in electrolytic plating of metals on glassesand as a reducing agent. Several hydrazine derivatives are used in azo dyes;as coupling agents in color photography; and in explosives and ammunitionprimers.
Production Methods
Different sources of media describe the Production Methods of 302-01-2 differently. You can refer to the following data:
1. Although the earlier processes for the commercial production of hydrazine used urea as a raw material, modern processes employ direct ammonia oxidation. In one such process, reactions occur in two steps: NH3 + NaOCl → NH2Cl + NaOH (1) NH3 + NH2Cl + NaOH → H2N·NH2 + NaCl + H2O. (2) High-grade hypochlorite is required for Step 1. Special agents, such as gelatin, ethylenediamine tetracetic acid, glue, high alcohols, and formaldehyde, are required to inhibit undesirable side reactions that would reduce the hydrazine yield through formation of ammonium chloride and N2. In another hydrazine process, chlorine, NH3, and H2SO4, along with methylethyl ketone, are used as the charge. The products of this process include hydrazine hydrate, hydrazine sulfate, ketazine, and dialkyldiazacyclopropane. Hydrazine also is used as a start-up ingredient in the preparation of cooling water for nuclear reactors where it is desired to keep the oxygen content of the water to an absolute minimum and thus decrease corrosion. Oxygen reacts with hydrazine. H2N·NH2 + O2 → N2 + 2H2O. When no oxygen is present in the water, the hydrazine acts as a sink for dissolved oxygen that may enter later, by maintaining metal oxides at their lower oxidation states. In the laboratory, hydrazine can be prepared by converting one-half of a given amount of NH3 into chloramine, NH2Cl, by sodium hypochlorite solution in the presence of a colloid and heating. The remaining one-half of the NH3 reacts with chloramine to form hydrazine. The product is then cooled to 0 °C and H2SO4 added in amount to react with the hydrazine to form hydrazine sulfate, N2H6SO4, insoluble solid. Hydrazine hemisulfate, (N2H5)2SO4, is soluble in H2O. It can also be made by the reaction of NH3 and hydroxylamine-O-sulfonic acid.
2. Hydrazine is a colorless, fuming, oily liquid with an
ammonia-like odor. It should be stored in glass containers
in a cool, dark place.
Hydrazine is prepared commercially by the Raschig and
the urea processes. The Raschig method involves reacting
sodium hypochlorite with excess ammonia, flash boiling to
recover dilute hydrazine, and fractionating to produce the
hydrate. In the urea process, urea is oxidized with hypochlorite
to produce the hydrate. Both anhydrous hydrazine and the
hydrate are fuming, strongly basic (pKb1=5.52), colorless
liquids. Hydrazine may ignite under various circumstances
(e.g., on contact with rust) and it decomposes violently in
contact with oxidizing materials. It is usually stored under
nitrogen to reduce the flammability hazard and to maintain
purity.
Definition
Different sources of media describe the Definition of 302-01-2 differently. You can refer to the following data:
1. A colorless
liquid that can be prepared by the oxidation
of ammonia with sodium
chlorate(I) or by the gas phase reaction of
ammonia with chlorine. Hydrazine is a
weak base, forming salts (e.g. N2H4.HCl)
with strong acids. It is a powerful reducing
agent, reducing salts of the noble metals to
the metal. Anhydrous hydrazine ignites
spontaneously in oxygen and reacts violently
with oxidizing agents. The aqueous
solution, hydrazine hydrate, has been used
as a fuel for jet engines and for rockets.
2. hydrazine: A colourless liquid orwhite crystalline solid,N2H4; r.d. 1.01(liquid); m.p. 1.4°C; b.p. 113.5°C. It isvery soluble in water and soluble inethanol. Hydrazine is prepared bythe Raschig synthesis in which ammoniareacts with sodium(I) chlorate(sodium hypochlorite) to give NH2Cl,which then undergoes further reactionwith ammonia to give N2H4. Industrialproduction must be carefullycontrolled to avoid a side reactionleading to NH4Cl. The compound is aweak base giving rise to two series ofsalts, those based on N2H5+, whichare stable in water (sometimes writtenin the form N2H4.HCl rather thanN2H5+Cl-), and a less stable and extensivelyhydrolysed series based onN2H62+. Hydrazine is a powerful reducingagent and reacts violentlywith many oxidizing agents, henceits use as a rocket propellant. It reactswith aldehydes and ketones togive hydrazones.
General Description
Colorless liquid with an ammonia-like odor. A violent poison. Causes delayed eye irritation. Very corrosive, attacks glass, rubber, and cork. Corrodes molybdenum steels such as Allegheny stainless 316.
It is a strong reducing agent and a flammable liquid and vapour. Hydrazine is a useful building block in organic synthesis of pharmaceuticals and pesticides. There are many kinds of hydrazine compounds, including hydrazine, 1,1-dimethylhydrazine, and 1,2-dimethylhydrazine. Small amounts of hydrazine occur naturally in plants. Most hydrazines are manufactured for use as rocket propellants and fuels, boiler water treatments, chemical reactants, medicines, and in cancer research. Hydrazines are highly reactive and easily catch fire.
Air & Water Reactions
Fumes in air. Water soluble.
Reactivity Profile
HYDRAZINE are strongly basic and are powerful reducing agents. Note that a 64% solution corresponds to the composition hydrazine hydrate (N2H4.H2O). Spontaneous ignition can occur with hydrogen peroxide and nitric acid. Contact with metallic oxide surfaces may lead to flaming decomposition [Haz. Chem. Data (1966)]. The reaction between 2,4-dinitrochlorobenzene and hydrazine hydrate shattered the reaction flask [Wischmeyer 1967]. Spontaneous ignition occurs when nitrous oxide and hydrazine are mixed [Mellor 8, Supp. 2:214(1967)]. Potassium and sodium dichromate react explosively with hydrazine [Mellor 11:234(1946-1947)]. Hydrazine hydrate reacts with stannous chloride to give stannous dihydrazinechloride, which decomposes explosively when heated [Mellor 7:430(1946-1947)]. Explodes during distillation if traces of air are present. Affected by UV and metal ion catalysis [Merck, 11th ed., 1989].
Hazard
Severe explosion hazard when exposed to
heat or by reaction with oxidizers. Toxic by ingestion, inhalation, and skin absorption; strong irritant
to skin and eyes; a confirmed carcinogen.
Health Hazard
Hydrazine is extremely destructive to the tissues of the mucous membranes and upper
respiratory tract, eyes, and skin. Skin contact with the liquid can result in severe burns;
hydrazine is readily absorbed through the skin, leading to systemic effects, which may
include damage to the liver, kidney, nervous system, and red blood cells. Hydrazine
vapor is irritating to the nose, throat, and respiratory tract, and inhalation of high
concentrations may be fatal as a result of spasm, inflammation, chemical pneumonitis,
and pulmonary edema. Symptoms of exposure may include a burning sensation,
coughing, wheezing, laryngitis, shortness of breath, headache, nausea, and vomiting.
Hydrazine vapor is extremely irritating to the eyes and can cause temporary blindness.
Eye contact with the liquid can result in severe burns and permanent damage. Hydrazine
is not considered to have adequate warning properties.
Hydrazine is listed by IARC in Group 2B "possible human carcinogen" and is classified
as a "select carcinogen" according to the criteria of the OSHA Laboratory Standard.Chronic exposure to subacute levels of hydrazine can cause lethargy, vomiting,
tremors, itching and burning of the eyes and skin, conjunctivitis, and contact
dermatitis. Hydrazine has been found to exhibit reproductive and developmental
toxicity in animal tests.
Fire Hazard
Flammable/combustible material. May be 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.
Flammability and Explosibility
Hydrazine is a flammable liquid (NFPA rating = 3) over a very broad range of vapor
concentrations (4.7 to 100%). Hydrazine may undergo autoxidation and ignite
spontaneously when brought in contact with porous substances such as rusty
surfaces, earth, wood, or cloth. Fires should be extinguished with water spray,
carbon dioxide, or dry chemical extinguishers.
Environmental Fate
Hydrazine can be found in the environment in small quantities
and is a component of tobacco smoke. However, hydrazine is
primarily an industrial chemical that enters the environment by
emissions from its use as an aerospace fuel and from industrial
facilities that manufacture, process, and/or use this chemical.
Treatment and disposal of wastes containing hydrazine also
contribute to environmental concentrations. However, hydrazine
rapidly degrades in the environment and is rarely
encountered outside the industrial setting.
storage
work
with hydrazine should be conducted in a fume hood to prevent exposure by
inhalation, and splash goggles and impermeable gloves should be worn at all times
to prevent eye and skin contact. Hydrazine should be used only in areas free of
ignition sources. Hydrazine should be stored under nitrogen in containers placed in
secondary containers in areas separate from oxidizers and acids.
Purification Methods
Hydrazine hydrate is dried by refluxing with an equal weight of KOH pellets for 3hours, then distilled from fresh solid NaOH or BaO in a current of dry N2. Use stainless steel or copper equipment. Hydrazine and its hydrates have VERY IRRITATING and TOXIC vapours and should be used in an efficient fume cupboard. Store in a well-stoppered vessel, preferably under N2. It is a reducing agent. [Schenk in Handbook of Preparative Inorganic Chemistry (Ed. Brauer) Academic Press Vol I pp 469-472 1963.]
Toxicity evaluation
Hydrazine is strongly corrosive and therefore severely irritates
the skin, eyes, and mucous membranes. Systemic toxicity
observed after hydrazine exposure is thought to be the result of
several possible mechanisms including:
1. Corrosive actions directly with tissue.
2. The reaction of hydrazine with endogenous alpha-keto
acids such as vitamin B, (pyridoxine). The formation of
hydrazones of pyridoxine is the proposed mechanism by
which hydrazine produces the neurological effects observed
after exposure.
3. The generation of free radical intermediates, which have
been detected during the metabolism of hydrazine in vitro.
The carcinogenicity of hydrazine is believed to be a result of
the condensation of hydrazine with endogenous formaldehyde
forming a formaldehyde hydrazone, which is further metabolized
to a potent DNA methylating agent causing the formation
of methylated DNA and transcription errors.
Incompatibilities
Hydrazine is a highly reactive reducing agent that forms shock-sensitive, explosive
mixtures with many compounds. It explodes on contact with barium oxide, calcium
oxide, chromate salts, and many other substances. On contact with metal catalysts
(platinum black, Raney nickel, etc.), hydrazine decomposes to ammonia, hydrogen,
and nitrogen gases, which may ignite or explode.
Waste Disposal
In the event of a spill, remove all ignition sources, soak up the hydrazine with a spill
pillow or absorbent material, place in an appropriate container, and dispose of
properly. Evacuation and cleanup using respiratory protection may be necessary in
the event of a large spill or release in a confined area.
Disposal Excess hydrazine and waste material containing this substance should be placed in
an appropriate container, clearly labeled, and handled according to your institution's
waste disposal guidelines. For more information on disposal procedures, see
Chapter 7 of this volume.
Check Digit Verification of cas no
The CAS Registry Mumber 302-01-2 includes 6 digits separated into 3 groups by hyphens. The first part of the number,starting from the left, has 3 digits, 3,0 and 2 respectively; the second part has 2 digits, 0 and 1 respectively.
Calculate Digit Verification of CAS Registry Number 302-01:
(5*3)+(4*0)+(3*2)+(2*0)+(1*1)=22
22 % 10 = 2
So 302-01-2 is a valid CAS Registry Number.
InChI:InChI=1/H4N2/c1-2/h1-2H2
302-01-2Relevant articles and documents
Rational design of bimetallic Rh0.6Ru0.4nanoalloys for enhanced nitrogen reduction electrocatalysis under mild conditions
Zhao, Lei,Liu, Xuejing,Zhang, Shen,Zhao, Jie,Xu, Xiaolong,Du, Yu,Sun, Xu,Zhang, Nuo,Zhang, Yong,Ren, Xiang,Wei, Qin
supporting information, p. 259 - 263 (2021/01/14)
As a carbon-free reaction process, the electrocatalytic nitrogen reduction reaction (eNRR) under mild conditions has broad prospects for green and sustainable NH3 production. In this work, bimetallic RhRu nanoalloys (NAs) with cross-linked curly nanosheets were successfully prepared and exhibited exciting results in the eNRR process. Furthermore, the composition effect of RhRu NAs on eNRR activity was studied systematically, and the results showed that Rh0.6Ru0.4 NAs/CP exhibited the highest NH3 yield rate of 57.75 μg h-1 mgcat.-1 and faradaic efficiency of 3.39%. As an eNRR catalyst with great potential, Rh0.6Ru0.4 NAs extend the possibility of alloy-nanomaterials in the eNRR field and further provide an idea for the precise structure of more effective and stable electrocatalysts.
Enhancing electrocatalytic nitrogen reduction to ammonia with rare earths (La, Y, and Sc) on high-index faceted platinum alloy concave nanocubes
Chen, You-Hu,Jiang, Xin,Liao, Hong-Gang,Liu, Feng,Mao, Yu-Jie,Sheng, Tian,Sun, Shi-Gang,Wei, Lu,Ye, Jin-Yu,Zhao, Xin-Sheng
, p. 26277 - 26285 (2021/12/10)
Surface structure effect is the key subject in electrocatalysis, and consists of the structure dependence of interaction between reaction molecules and the catalyst surface in specifying the surface atomic arrangement, chemical composition and electronic structure. Herein, we develop a controllable synthesis of Pt-RE (RE = La, Y, Sc) alloy concave nanocubes (PtRENCs) with {410} high-index facets (HIFs) by an electrochemical method in a choline chloride-urea based deep eutectic solvent. The PtRENCs are used as an efficient catalyst in electrocatalytic nitrogen reduction to ammonia (NH3). Owing to the high density of low-coordinated Pt step sites (HIF structure) and the unique electronic effect of Pt-RE, the as-prepared PtRENCs exhibit an excellent electrocatalytic performance for the nitrogen reduction reaction (NRR) under ambient conditions. The NH3 yield rate and faradaic efficiency (FE) share the same trend of Pt-La (rNH3: 71.4 μg h-1 μgcat-1, FE: 35.6%) > Pt-Y (rNH3: 65.2 μg h-1 μgcat-1, FE: 26.7%) > Pt-Sc (rNH3: 48.5 μg h-1 μgcat-1, FE: 19%) > Pt (rNH3: 25.8 μg h-1 μgcat-1, FE: 10.7%). Moreover, the PtRENCs demonstrate high selectivity for N2 reduction to NH3 and high stability retaining 90% of the NH3 yield rate and FE values after 12 h continuous NRR tests. Density functional theory (DFT) calculations indicate that the rate determining step of the NRR process is the formation of N2H2? from N2 with the transfer of two proton-coupled electrons, and the upshift of the d-band center boosts the NRR activity by enhancing the bonding strength of reaction intermediates on the high-index faceted Pt-RE (RE = La, Y, Sc) alloying surface. In addition, the introduction of RE (RE = La, Y, Sc) on the Pt step surface can effectively suppress the HER process and provide appropriate sites for the NRR. This journal is
Rigid two-dimensional indium metal-organic frameworks boosting nitrogen electroreduction at all pH values
Chen, Sheng,Ding, Shan,Duan, Jingjing,Sun, Yuntong,Xia, Baokai,Yu, Licheng
supporting information, p. 20040 - 20047 (2021/09/20)
Based on an ion exchange and dissolution-recrystallization mechanism, rigid indium metal-organic framework (In-MOF) nanosheets have been synthesized under mild conditions. The collective advantages of the rigid structure and two-dimensional architecture (thickness: 1.3 nm) enable In-MOF to show great activity during nitrogen electroreduction and excellent stability over a wide pH range. At pH values ?1mg?1(or 4.94 μg h?1cm?2) and faradic efficiency ≥6.72%. At pH values ≥7, 2D In-MOF can operate efficiently with a record NH3yield of 79.20 μg h?1mg?1(or 15.94 μg h?1cm?2) and faradic efficiency of 14.98%, making it one of the most active MOF-based electrocatalysts for nitrogen electroreduction. Furthermore, the reaction mechanism of nitrogen electroreduction has been revealed using density function theory (DFT) simulations, and it follows enzymatic pathways at all pH values, with the potential determining step being *H2NNH2* → *NH2+ NH3. It is expected that the present study will offer valuable clues for the design and fabrication of low-cost and efficient all-pH nitrogen reduction electrocatalysts for industrial applications.
