Difference between revisions of "Calcium cyanamide"

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| OtherNames = Cyanamide calcium salt<br>Lime Nitrogen<br>Nitrolime<br>UN 1403
 
| OtherNames = Cyanamide calcium salt<br>Lime Nitrogen<br>Nitrolime<br>UN 1403
 
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| ImageFile = Calcium_cyanamide.jpg
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| ImageSize = 270
 
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| ImageCaption = Freshly made calcium cyanamide
 
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| pKb =  
 
| pKb =  
 
| Solubility = Reacts
 
| Solubility = Reacts
| SolubleOther = Insoluble in organic solvents
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| SolubleOther = Reacts with acids<br>Insoluble in organic solvents
 
| Solvent =  
 
| Solvent =  
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| VaporPressure = ~0 mmHg
 
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| Section3 = {{Chembox Structure
 
| Section3 = {{Chembox Structure
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==Properties==
 
==Properties==
 
===Chemical===
 
===Chemical===
Hydrolysis of CaCN<sub>2</sub> will yield [[cyanamide]], as well as ammonia.
+
Hydrolysis of CaCN<sub>2</sub> will yield [[cyanamide]], as well as [[ammonia]].
  
 
: CaCN<sub>2</sub> + H<sub>2</sub>O + CO<sub>2</sub> → CaCO<sub>3</sub> + H<sub>2</sub>NCN
 
: CaCN<sub>2</sub> + H<sub>2</sub>O + CO<sub>2</sub> → CaCO<sub>3</sub> + H<sub>2</sub>NCN
 
: CaCN<sub>2</sub> + 3 H<sub>2</sub>O → 2 NH<sub>3</sub> + CaCO<sub>3</sub>
 
: CaCN<sub>2</sub> + 3 H<sub>2</sub>O → 2 NH<sub>3</sub> + CaCO<sub>3</sub>
 +
 +
At high pH, cyanamide converts to [[cyanoguanidine]] (dicyandiamide).
  
 
Fusing calcium cyanamide with sodium carbonate will give sodium cyanide.
 
Fusing calcium cyanamide with sodium carbonate will give sodium cyanide.
 
: CaCN<sub>2</sub> + Na<sub>2</sub>CO<sub>3</sub> + 2C → 2 NaCN + CaO + 2 CO
 
: CaCN<sub>2</sub> + Na<sub>2</sub>CO<sub>3</sub> + 2C → 2 NaCN + CaO + 2 CO
 +
 +
Fusing calcium cyanamide with [[ammonium nitrate]] at high temperatures will give [[guanidinium nitrate]].<ref>https://cdnsciencepub.com/doi/pdf/10.1139/v58-211</ref> Although some old literature data indicates that the reaction can also be done in an aq. solution, it's been shown that the presence of water may lead to the formation of other side products.<ref>https://www.freepatentsonline.com/2431301.pdf</ref>
  
 
===Physical===
 
===Physical===
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==Availability==
 
==Availability==
Calcium cyanamide is sold as fertilizer. In some places it's hard to find.
+
Calcium cyanamide is sold as fertilizer, usually in the form of black pellets, which contain up to 50% CaCN<sub>2</sub> by mass. In some places it's hard to find, as the compounds readily hydrolyzes in the presence of moisture, and water-sensitive materials are generally not sold in most stores due to safety.
  
 
It can also be bought from chemical suppliers.
 
It can also be bought from chemical suppliers.
  
 
==Preparation==
 
==Preparation==
A common route to calcium cyanamide involves heating a mixture of [[calcium oxide]] and [[urea]] at 120-350 °C which gives calcium cyanate, followed by calcination at 7-900 °C to give calcium cyanamide.<ref>https://www.youtube.com/watch?v=S-SOjfZ_yS4</ref>
+
A common route to calcium cyanamide involves heating a mixture of [[calcium oxide]] and [[urea]] at 120-350 °C which gives calcium cyanate, followed by calcination at 7-900 °C to give calcium cyanamide.<ref>https://www.youtube.com/watch?v=S-SOjfZ_yS4</ref>
  
:3 CO(NH<sub>2</sub>)<sub>2</sub> → 3 HOCN + NH<sub>3</sub>
+
: 3 CO(NH<sub>2</sub>)<sub>2</sub> → 3 HOCN + NH<sub>3</sub>
:CaO + 2 HOCN → Ca(OCN)<sub>2</sub> + H<sub>2</sub>O
+
: CaO + 2 HOCN → Ca(OCN)<sub>2</sub> + H<sub>2</sub>O
:Ca(OCN)<sub>2</sub> → CaCN<sub>2</sub> + CO<sub>2</sub>
+
: Ca(OCN)<sub>2</sub> → CaCN<sub>2</sub> + CO<sub>2</sub>
  
Calcium cyanamide is obtained industrially by heating [[calcium carbide]] powder at 1,000 °C, usually in an electric furnace, while injecting [[nitrogen]] gas over the hot carbide, which is recirculated. The reaction takes several hours for completion.
+
Calcium cyanamide is obtained industrially by heating [[calcium carbide]] powder at 1,000 °C, usually in an electric furnace, while injecting [[nitrogen]] gas over the hot carbide, which is recirculated. The reaction takes several hours for completion. The reaction produces carbon and is the reason commercial calcium cyanamide fertilizer is usually black in color.
 +
 
 +
: CaC<sub>2</sub> + N<sub>2</sub> → Ca(CN)<sub>2</sub> → CaCN<sub>2</sub> + C
  
 
Another route involves heating calcium cyanide with nitrogen gas at 600 °C for at least one hour.<ref>Franck, H.; Heimann, H.; Angewandte Chemie; vol. 44; (1931); p. 372 - 378</ref>
 
Another route involves heating calcium cyanide with nitrogen gas at 600 °C for at least one hour.<ref>Franck, H.; Heimann, H.; Angewandte Chemie; vol. 44; (1931); p. 372 - 378</ref>
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Reacting [[ammonia]] with [[calcium carbonate]] above 600 °C is another route.<ref>Franklin; Journal of the American Chemical Society; vol. 44; (1922); p. 504</ref><ref>Patent; Caro; Frank; DE467479; Fortschr. Teerfarbenfabr. Verw. Industriezweige; vol. 16; p. 283</ref>
 
Reacting [[ammonia]] with [[calcium carbonate]] above 600 °C is another route.<ref>Franklin; Journal of the American Chemical Society; vol. 44; (1922); p. 504</ref><ref>Patent; Caro; Frank; DE467479; Fortschr. Teerfarbenfabr. Verw. Industriezweige; vol. 16; p. 283</ref>
  
Since calcium cyanamide reacts with oxygen at high temperatures, all of these routes must be done in low of oxygen environment, and an inert gas is used.
+
Since calcium cyanamide reacts with oxygen at high temperatures, all of these routes must be done in the absence of oxygen, thus an inert gas is often used.
  
 
==Projects==
 
==Projects==
 +
*Make [[cyanoguanidine]]
 
*Make [[guanidine]] compounds
 
*Make [[guanidine]] compounds
 
*Make [[sodium cyanide]]
 
*Make [[sodium cyanide]]
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===Storage===
 
===Storage===
In closed containers, away from moisture.
+
Calcium cyanamide must be kept in closed containers, away from moisture. Empty paint or instant coffee cans are good.
  
 
===Disposal===
 
===Disposal===
 
Can be dumped in the ground.
 
Can be dumped in the ground.
 +
 +
==Gallery==
 +
<gallery widths="200" position="center" columns="4" orientation="none">
 +
Silver_cyanamide.jpg|The yellow color of silver cyanamide is used to confirm the presence of the ion
 +
Calcium_cyanamide_fertilizer.jpg|Calcium cyanamide fertilizer is usually black due to carbon impurities
 +
</gallery>
  
 
==References==
 
==References==
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[[Category:Readily available chemicals]]
 
[[Category:Readily available chemicals]]
 
[[Category:Irritants]]
 
[[Category:Irritants]]
 +
[[Category:Essential reagents]]

Latest revision as of 15:17, 18 November 2023

Calcium cyanamide
Calcium cyanamide.jpg
Freshly made calcium cyanamide
Names
IUPAC name
Calcium cyanamide
Other names
Cyanamide calcium salt
Lime Nitrogen
Nitrolime
UN 1403
Properties
CaCN2
Molar mass 80.102 g/mol
Appearance White solid (Often gray or black from impurities)
Odor Odorless
Density 2.29 g/cm3
Melting point 1,340 °C (2,440 °F; 1,610 K)
Boiling point Sublimes
Reacts
Solubility Reacts with acids
Insoluble in organic solvents
Vapor pressure ~0 mmHg
Thermochemistry
-351.6 kJ/mol
Hazards
Safety data sheet Sigma-Aldrich
Flash point Non-flammable
Related compounds
Related compounds
Calcium carbide
Cyanamide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Calcium cyanamide is an inorganic compound with the formula CaCN2, widely used as fertilizer in agriculture.

Properties

Chemical

Hydrolysis of CaCN2 will yield cyanamide, as well as ammonia.

CaCN2 + H2O + CO2 → CaCO3 + H2NCN
CaCN2 + 3 H2O → 2 NH3 + CaCO3

At high pH, cyanamide converts to cyanoguanidine (dicyandiamide).

Fusing calcium cyanamide with sodium carbonate will give sodium cyanide.

CaCN2 + Na2CO3 + 2C → 2 NaCN + CaO + 2 CO

Fusing calcium cyanamide with ammonium nitrate at high temperatures will give guanidinium nitrate.[2] Although some old literature data indicates that the reaction can also be done in an aq. solution, it's been shown that the presence of water may lead to the formation of other side products.[3]

Physical

Calcium cyanamide is a white (gray or black if impure) solid, which reacts with water.

Availability

Calcium cyanamide is sold as fertilizer, usually in the form of black pellets, which contain up to 50% CaCN2 by mass. In some places it's hard to find, as the compounds readily hydrolyzes in the presence of moisture, and water-sensitive materials are generally not sold in most stores due to safety.

It can also be bought from chemical suppliers.

Preparation

A common route to calcium cyanamide involves heating a mixture of calcium oxide and urea at 120-350 °C which gives calcium cyanate, followed by calcination at 7-900 °C to give calcium cyanamide.[4]

3 CO(NH2)2 → 3 HOCN + NH3
CaO + 2 HOCN → Ca(OCN)2 + H2O
Ca(OCN)2 → CaCN2 + CO2

Calcium cyanamide is obtained industrially by heating calcium carbide powder at 1,000 °C, usually in an electric furnace, while injecting nitrogen gas over the hot carbide, which is recirculated. The reaction takes several hours for completion. The reaction produces carbon and is the reason commercial calcium cyanamide fertilizer is usually black in color.

CaC2 + N2 → Ca(CN)2 → CaCN2 + C

Another route involves heating calcium cyanide with nitrogen gas at 600 °C for at least one hour.[5]

Reducing calcium nitride with carbon at 800-900 °C in a nitrogen atmosphere will also give calcium cyanamide.[6]

Reacting ammonia with calcium carbonate above 600 °C is another route.[7][8]

Since calcium cyanamide reacts with oxygen at high temperatures, all of these routes must be done in the absence of oxygen, thus an inert gas is often used.

Projects

Handling

Safety

Calcium cyanamide is harmful and should be handled with care.

It is known to cause alcohol intolerance, before or after the consumption of alcohol.

Storage

Calcium cyanamide must be kept in closed containers, away from moisture. Empty paint or instant coffee cans are good.

Disposal

Can be dumped in the ground.

Gallery

References

  1. Franck, H. H.; Hochwald, F.; Zeitschrift fuer Elektrochemie; vol. 31; (1925); p. 581 - 590
  2. https://cdnsciencepub.com/doi/pdf/10.1139/v58-211
  3. https://www.freepatentsonline.com/2431301.pdf
  4. https://www.youtube.com/watch?v=S-SOjfZ_yS4
  5. Franck, H.; Heimann, H.; Angewandte Chemie; vol. 44; (1931); p. 372 - 378
  6. Krase, H. J.; Jee, J. Y.; Journal of the American Chemical Society; vol. 46; (1924); p. 1358 - 1366
  7. Franklin; Journal of the American Chemical Society; vol. 44; (1922); p. 504
  8. Patent; Caro; Frank; DE467479; Fortschr. Teerfarbenfabr. Verw. Industriezweige; vol. 16; p. 283

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