Difference between revisions of "Hydrazine"

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| OtherNames = Diamine<br>Diazane<br>Tetrahydridodinitrogen(N—N)
 
| OtherNames = Diamine<br>Diazane<br>Tetrahydridodinitrogen(N—N)
 
<!-- Images -->
 
<!-- Images -->
−
| ImageFile =  
+
| ImageFile = Anhydrous hydrazine in ampoule by ChemicalForce.png
−
| ImageSize =  
+
| ImageSize = 300
 
| ImageAlt =  
 
| ImageAlt =  
 
| ImageName =  
 
| ImageName =  
 +
| ImageCaption = Anhydrous hydrazine stored in a glass ampoule.
 
| ImageFile1 =  
 
| ImageFile1 =  
 
| ImageSize1 =  
 
| ImageSize1 =  
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| MeltingPt_ref =  
 
| MeltingPt_ref =  
 
| MeltingPt_notes =  
 
| MeltingPt_notes =  
 +
| Odor = Ammonia-like
 
| pKa = 8.10
 
| pKa = 8.10
 
| pKb = 5.90
 
| pKb = 5.90
 
| Solubility = Miscible
 
| Solubility = Miscible
−
| SolubleOther = soluble in [[methanol]], [[ethanol]], [[propanol]], [[isobutanol]] and amyl alcohol
+
| SolubleOther = Reacts with acids, halogens, [[hydrogen peroxide]]<br>Soluble in [[methanol]], [[ethanol]], [[propanol]], [[isobutanol]] and amyl alcohol
 
| Solvent =  
 
| Solvent =  
−
| VaporPressure =  
+
| VaporPressure = 1 kP (at 30.7 °C)
 
   }}
 
   }}
 
| Section3 = {{Chembox Structure
 
| Section3 = {{Chembox Structure
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| DeltaGf =  
 
| DeltaGf =  
 
| DeltaHc =  
 
| DeltaHc =  
−
| DeltaHf =  
+
| DeltaHf = 50.63 kJ/mol
−
| Entropy =  
+
| Entropy = 121.52 J·K<sup>−1</sup>·mol<sup>−1</sup>
 
| HeatCapacity =  
 
| HeatCapacity =  
 
   }}
 
   }}
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| AutoignitionPt = 24 to 270 °C
 
| AutoignitionPt = 24 to 270 °C
 
| ExploLimits = 1.8–99.99%
 
| ExploLimits = 1.8–99.99%
−
| ExternalMSDS =  
+
| ExternalMSDS = [https://www.docdroid.net/7gzQ9CR/hydrazine-sa.pdf.html Sigma-Aldrich]
−
| FlashPt = 52 °C
+
| FlashPt = 52 °C (125.6 °F; 325 K)
 
| LD50 = 59–60 mg/kg (oral in rats, mice)
 
| LD50 = 59–60 mg/kg (oral in rats, mice)
 
| LC50 = 260 ppm (rat, 4 hr)<br>630 ppm (rat, 1 hr)<br>570 ppm (rat, 4 hr)<br>252 ppm (mouse, 4 hr)
 
| LC50 = 260 ppm (rat, 4 hr)<br>630 ppm (rat, 1 hr)<br>570 ppm (rat, 4 hr)<br>252 ppm (mouse, 4 hr)
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| OtherFunction =  
 
| OtherFunction =  
 
| OtherFunction_label =  
 
| OtherFunction_label =  
−
| OtherCompounds = [[Ammonia]]
+
| OtherCompounds = [[Ammonia]]<br>[[Triazane]]
 
   }}
 
   }}
 
}}
 
}}
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==Properties==
 
==Properties==
 
===Chemical===
 
===Chemical===
−
Hydrazine, like ammonia, will form salts with acids. With [[sulfuric acid]], for example, forms [[hydrazine sulfate]].
+
Hydrazine, like [[ammonia]], will form salts with acids. With [[sulfuric acid]], for example, forms [[hydrazine sulfate]].
  
−
:N<sub>2</sub>H<sub>4</sub> + H<sub>2</sub>SO<sub>4</sub> → N<sub>2</sub>H<sub>5</sub>HSO<sub>4</sub>
+
: N<sub>2</sub>H<sub>4</sub> + H<sub>2</sub>SO<sub>4</sub> → N<sub>2</sub>H<sub>5</sub>HSO<sub>4</sub>
 +
 
 +
Hydrazine ignites in contact with various oxidizers, like liq. [[ozone]], liq. [[chlorine]], [[chromyl chloride]], [[dinitrogen tetroxide]]/[[nitrogen dioxide]], conc. [[hydrogen peroxide]], [[cobalt(III) fluoride]], vanadium oxytrichloride . Reaction of anhydrous hydrazine with [[osmium tetroxide]] is extremely violent, basically an explosion. Reaction with elemental [[bromine]] or [[iodine]] however, while violent, it does not lead to ignition.<ref>https://www.youtube.com/watch?v=V3HuKQvRBUE</ref>
 +
 
 +
Anhydrous hydrazine will rapidly and violently reduce [[iodine pentoxide]] to [[hydrogen iodide]]. Any elemental [[iodine]] produced is immediately reduced to HI. The reaction also produces side products like hydrogen, nitrogen, ammonia and copious amounts of ammonium iodide fumes. The reaction can sometimes be violent enough that it may cause an explosion.<ref>https://www.youtube.com/watch?v=V3HuKQvRBUE</ref>
 +
 
 +
Hydrazine reacts with [[sodium nitrite]] forming [[sodium azide]]:<ref>https://onlinelibrary.wiley.com/doi/10.1002/14356007.a13_177</ref>
 +
 
 +
: N<sub>2</sub>H<sub>4</sub> + NaNO<sub>2</sub> → NaN<sub>3</sub> + 2 H<sub>2</sub>O
  
 
===Physical===
 
===Physical===
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==Preparation==
 
==Preparation==
−
Anhydrous hydrazine can be made by reacting [[hydrazine sulfate]] with a strong base, filter the reaction product and drying the resulting condensate. Avoid distilling the resulting hydrazine and it may explode.
+
Anhydrous hydrazine can be made by reacting [[hydrazine sulfate]] with a strong base, filter the reaction product and drying the resulting condensate. Avoid distilling the resulting hydrazine at atmospheric conditions and pressure, as it may explode. Distillation can be done in an inert atmosphere, but any trace of air may lead to an explosion.
  
 
==Projects==
 
==Projects==
−
*Rocket fuel
+
*Make [[hydrazine sulfate]]
 +
*Make [[sodium azide]]
 
*Make [[hydrazoic acid]] (DANGEROUS!)
 
*Make [[hydrazoic acid]] (DANGEROUS!)
 +
*Make [[nickel hydrazine nitrate]]
 +
*Reducing agent
 +
*Rocket fuel
  
 
==Handling==
 
==Handling==
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===Storage===
 
===Storage===
−
While it can be stored in sealed or closed containers, the best way to store hydrazine is as the sulfate form. It can be easily liberated from this form with an alkali when or if needed.
+
While it can be stored in sealed or closed containers, the best and safest way to store hydrazine is in salt form, most often as the sulfate form. It can be easily liberated from this form with an alkali when or if needed.
 +
 
 +
Hydrazine will slowly leach silica from glass, so avoid storing it in glass containers. Type 304L and 347 stainless steel containers are generally used for storing hydrazine, though high density polyethylene is also suitable.<ref>http://www.hydrazine.com/~/media/Microsites/Hydrazine/Docs/SafetyHandlingTDS.ashx?la=en</ref>
  
 
===Disposal===
 
===Disposal===
−
Hydrazine can be neutralized with a diluted solution of calcium hypochlorite. Avoid using strong oxidizers, like [[hydrogen peroxide]], as this will result in a steam explosion.
+
Hydrazine can be neutralized with a diluted solution of [[calcium hypochlorite]] or another oxidizer. Avoid using strong or concentrated oxidizers, like conc. [[hydrogen peroxide]], as this will result in a steam explosion.
  
 
==References==
 
==References==
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[[Category:Inorganic compounds]]
 
[[Category:Inorganic compounds]]
 
[[Category:Nitrogen compounds]]
 
[[Category:Nitrogen compounds]]
 +
[[Category:Hydrogen compounds]]
 
[[Category:Amines]]
 
[[Category:Amines]]
 
[[Category:Bases]]
 
[[Category:Bases]]
 
[[Category:Lewis bases]]
 
[[Category:Lewis bases]]
 +
[[Category:Reducing agents]]
 +
[[Category:Materials unstable in acidic solution]]
 
[[Category:Carcinogenic]]
 
[[Category:Carcinogenic]]
 
[[Category:Foul smelling compounds]]
 
[[Category:Foul smelling compounds]]
 
[[Category:Things that can kill you very quickly]]
 
[[Category:Things that can kill you very quickly]]
 
[[Category:Things that should NOT be messed with except by professionals]]
 
[[Category:Things that should NOT be messed with except by professionals]]
 +
[[Category:Irritants]]
 +
[[Category:Liquids]]

Latest revision as of 17:29, 2 January 2023

Hydrazine
Anhydrous hydrazine in ampoule by ChemicalForce.png
Anhydrous hydrazine stored in a glass ampoule.
Names
IUPAC name
Hydrazine
Systematic IUPAC name
Hydrazine
Other names
Diamine
Diazane
Tetrahydridodinitrogen(N—N)
Properties
N2H4
Molar mass 32.0452
Appearance Clear liquid
Odor Ammonia-like
Density 1.014 g/cm3 (15 °C)
Melting point 2 °C (36 °F; 275 K)
Boiling point 114 °C (237 °F; 387 K)
Miscible
Solubility Reacts with acids, halogens, hydrogen peroxide
Soluble in methanol, ethanol, propanol, isobutanol and amyl alcohol
Vapor pressure 1 kP (at 30.7 °C)
Acidity (pKa) 8.10
Thermochemistry
121.52 J·K−1·mol−1
50.63 kJ/mol
Hazards
Safety data sheet Sigma-Aldrich
Flash point 52 °C (125.6 °F; 325 K)
Lethal dose or concentration (LD, LC):
59–60 mg/kg (oral in rats, mice)
260 ppm (rat, 4 hr)
630 ppm (rat, 1 hr)
570 ppm (rat, 4 hr)
252 ppm (mouse, 4 hr)
Related compounds
Related compounds
 Ammonia
Triazane
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Hydrazine is an inorganic compound with the chemical formula N2H4 or H2N-NH2. It is a toxic compound used as rocket fuel.

Properties

Chemical

Hydrazine, like ammonia, will form salts with acids. With sulfuric acid, for example, forms hydrazine sulfate.

N2H4 + H2SO4 → N2H5HSO4

Hydrazine ignites in contact with various oxidizers, like liq. ozone, liq. chlorine, chromyl chloride, dinitrogen tetroxide/nitrogen dioxide, conc. hydrogen peroxide, cobalt(III) fluoride, vanadium oxytrichloride . Reaction of anhydrous hydrazine with osmium tetroxide is extremely violent, basically an explosion. Reaction with elemental bromine or iodine however, while violent, it does not lead to ignition.[1]

Anhydrous hydrazine will rapidly and violently reduce iodine pentoxide to hydrogen iodide. Any elemental iodine produced is immediately reduced to HI. The reaction also produces side products like hydrogen, nitrogen, ammonia and copious amounts of ammonium iodide fumes. The reaction can sometimes be violent enough that it may cause an explosion.[2]

Hydrazine reacts with sodium nitrite forming sodium azide:[3]

N2H4 + NaNO2 → NaN3 + 2 H2O

Physical

Hydrazine is a clear fuming oily liquid, with a toxic strong ammonia like odor. It is miscible with water, and soluble in several solvents, like methanol or ethanol. Hydrazine boils at 114 °C and melts at 2 °C.

Availability

Anhydrous hydrazine is sold by chemical suppliers, though it's not easily available to the amateur chemist due to its hazards.

Preparation

Anhydrous hydrazine can be made by reacting hydrazine sulfate with a strong base, filter the reaction product and drying the resulting condensate. Avoid distilling the resulting hydrazine at atmospheric conditions and pressure, as it may explode. Distillation can be done in an inert atmosphere, but any trace of air may lead to an explosion.

Projects

Handling

Safety

Free hydrazine is extremely toxic and should only be handled with proper protection. It will slowly decompose to release nitrogen and ammonia. As a solution is less dangerous, though it's fumes are still very toxic. It may explode during its distillation in the presence of oxygen, due to its low autoignition point, so it's best to perform the distillation in an oxygen-free environment.

Due to these risks, the safest way to handle hydrazine is in the sulfate form.

Storage

While it can be stored in sealed or closed containers, the best and safest way to store hydrazine is in salt form, most often as the sulfate form. It can be easily liberated from this form with an alkali when or if needed.

Hydrazine will slowly leach silica from glass, so avoid storing it in glass containers. Type 304L and 347 stainless steel containers are generally used for storing hydrazine, though high density polyethylene is also suitable.[4]

Disposal

Hydrazine can be neutralized with a diluted solution of calcium hypochlorite or another oxidizer. Avoid using strong or concentrated oxidizers, like conc. hydrogen peroxide, as this will result in a steam explosion.

References

  1. ↑ https://www.youtube.com/watch?v=V3HuKQvRBUE
  2. ↑ https://www.youtube.com/watch?v=V3HuKQvRBUE
  3. ↑ https://onlinelibrary.wiley.com/doi/10.1002/14356007.a13_177
  4. ↑ http://www.hydrazine.com/~/media/Microsites/Hydrazine/Docs/SafetyHandlingTDS.ashx?la=en

Relevant Sciencemadness threads

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