Copper (II) chloride: Difference between revisions
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=====copper (II) oxide / sulfide===== | =====copper (II) oxide / sulfide===== | ||
...hydrochlorination of the copper(II) compounds begins at 190°C to form ammonium chlorocuprates, {{#Chem:(NH4)2CuCl4}} in with [[copper (II) oxide]] and {{#Chem:NH4CuCl3}} with copper (II) sulfide, which at the temperature higher than 300°C decompose affording [[copper (II) chloride|{{#Chem:CuCl2}}]]<ref>{{cite pub | |||
|publication=Russian Journal of General Chemistry | |publication=Russian Journal of General Chemistry | ||
(2) (PDF) Reaction of ammonium chloride with the copper(II) sulfide and oxide, and identification of the reaction products. Available from: https://www.researchgate.net/publication/251412801_Reaction_of_ammonium_chloride_with_the_copperII_sulfide_and_oxide_and_identification_of_the_reaction_products [accessed Jan 23 2020]. | |||
|year=2011 | |year=2011 | ||
|volume=81 | |volume=81 | ||
| Line 103: | Line 106: | ||
|doi=10.1134/S107036321107005X | |doi=10.1134/S107036321107005X | ||
}}</ref> | }}</ref> | ||
# Heat to 300°C | '''Compound I.''' A mixture of copper oxide, 6.67 g, and ammonium chloride, 17.61 g, was calcined at a temperature of 320ºC for 12 h. | ||
'''Compound II.''' Prepared similarly from 5.46 g of copper sulfide and 18.04 g of ammonium chloride at a temperature of 320ºC for 12 h | |||
# Combine 1ubm [[copper (II) oxide]] and 2.6ubm dry [[ammonium chloride]] | |||
# Heat to 300°C for 12h | |||
#: {{#Chem: 2 NH4Cl + CuO = CuCl2 + H2O + 2 NH3 }} | #: {{#Chem: 2 NH4Cl + CuO = CuCl2 + H2O + 2 NH3 }} | ||
#: {{#Chem: 2 NH4Cl + CuS = CuCl2 + H2S + 2 NH3 }} | #: {{#Chem: 2 NH4Cl + CuS = CuCl2 + H2S + 2 NH3 }} | ||
Revision as of 07:27, 10 May 2020
| Chemical formula | CuCl2 |
|---|---|
| OTP appearance | yellow-brown solid |
| Molar Mass(g/mol) | 134.45(anh) 170.48(dihydrate) |
| Density(g/cc) | 3.386 |
| Melting Point(°C) | 498 |
| Boiling Point(°C) | 993 (decomp) |
| Solubility in water(g/L) | 757 |
| Solubility in ethanol(g/L) | 530 |
| Solubility in methanol(g/L) | 680 |
| Solubility in ether(g/L) | 1.1 |
| Solubility in acetone(g/L) | 30 |
| NFPA 704 |  0
2
1
|
| Thermal Decomposition | copper (II) chloride
993°C CuCl,Cl2 |
Uses
Other
- Catalyst for the production of sulfuric acid
- Metal etchant
Natural occurrence
- Does occur naturally as the very rare minerals tolbachite and eriochalcite
Hazards
Soluble copper compounds are toxic to mammals and can be deadly to fish.
Production
Synthesis
The main routes are divided by the source and valence of the copper, and the source of the chloride ion.
| Source of chlorine ion | |||
|---|---|---|---|
| hydrochloric acid (aerated) | ammonium chloride | chlorine gas | |
| Copper (0) | |||
| copper metal | ✔ | ? | ✔ |
| Copper (I) | |||
| copper (I) chloride | ✔ | ? | ? |
| Chalcocite copper (I) sulfide |
? | ? | ? |
| Cuprite copper (I) oxide |
? | ? | ? |
| Copper (II) | |||
| Tenorite Copper (II) oxide |
✔ | ✔ | ? |
| Covellite copper (II) sulfide |
✔ | ✔ | ? |
| Malachite | ✔ | ✔ | ? |
| Azurite | ✔ | ✔ | ? |
| Copper (II) acetate | ✔ | ? | no |
| Copper (II) hydroxide | ? | ? | ? |
via hydrochloric acid
metallic copper
- Bubble air through copper metal immersed in hydrochloric acid. This will not work without the air, and even then it takes days. This may go in two separate steps, first to copper (I) chloride, and thence to copper(II) chloride, shown separately below.
- 4 Cu + 4 HCl + O2 → 4 CuCl + 2 H2O // from copper(0) to copper (I)
- 4 CuCl + 4 HCl + O2 → 4 CuCl2 + 2 H2O // from copper(I) to copper (II)
copper (I) chloride
- Bubble air through copper (I) chloride in hydrochloric acid. This will not work without the air, and even then it takes days. [1]
- 4 CuCl + 4 HCl + O2 → 4 CuCl2 + 2 H2O // from (I) to (II)
copper (II) minerals
- Combine malachite and hydrochloric acid
- Cu2CO3(OH)2 + 4 HCl → 2 CuCl2 + 3 H2O + CO2
- Combine azurite and hydrochloric acid
- Cu3(CO3)2(OH)2 + 6 HCl → 3 CuCl2 + 4 H2O + 2 CO2
via ammonium chloride
copper hydroxide
- Combine ammonium chloride and damp copper (II) hydroxide
- Mix thoroughly, allowing the compounds to react
- Heat above 40°C, driving off the ammonium hydroxide
- NB keep temperature below 200°C to prevent decomposing the copper hydroxide
- keep temperature below 350°C to prevent decomposing the ammonium chloride
- Both ammonium hydroxide and copper chloride are thermally stable.
copper carbonate / malachite / azurite
These reactions work in the presence of excess ammonium chloride
- 4 NH4Cl + Cu2CO3(OH)2 → 2 CuCl2 + 3 H2O + 4 NH3 + CO2 // 2x excess of -chloride
- 6 NH4Cl + Cu3(CO3)2(OH)2 → 3 CuCl2 + 4 H2O + 6 NH3 + 2 CO2 // UNTESTED
copper (II) oxide / sulfide
...hydrochlorination of the copper(II) compounds begins at 190°C to form ammonium chlorocuprates, (NH4)2CuCl4 in with copper (II) oxide and NH4CuCl3 with copper (II) sulfide, which at the temperature higher than 300°C decompose affording CuCl2[2] Compound I. A mixture of copper oxide, 6.67 g, and ammonium chloride, 17.61 g, was calcined at a temperature of 320ºC for 12 h. Compound II. Prepared similarly from 5.46 g of copper sulfide and 18.04 g of ammonium chloride at a temperature of 320ºC for 12 h
- Combine 1ubm copper (II) oxide and 2.6ubm dry ammonium chloride
- Heat to 300°C for 12h
- 2 NH4Cl + CuO → CuCl2 + H2O + 2 NH3
- 2 NH4Cl + CuS → CuCl2 + H2S + 2 NH3
- Cool to RT with dryer in place.
via chlorine
metallic copper
At or above red heat (~500°C), copper reacts directly with gaseous chlorine, giving molten CuCl2. The reaction is sufficiently exothermic that the reaction will continue once started.
via calcium chloride
Metathesis reaction between copper (II) sulfate with calcium chloride or barium chloride, producing copper chloride in solution and calcium sulfate as a precipitate. Obviously this is only useful after the production of both materials, so there's a bootstrapping problem.
- CuSO4 + CaCl2 → CuCl2 + CaSO4
- CuSO4 + BaCl2 → CuCl2 + BaSO4
Purification
Recrystallize from hot dilute aqueous HCl by cooling in a calcium chloride-ice bath
Testing
- Visual: Yellow-brown (anhydrous) dark green (excess chloride) or bright blue (partially hydrated) crystals
- Reacts vigorously with aluminum
- 3 CuCl2 + 2 Al → 3 Cu + 2 AlCl3
Storage
- Do not store with excess copper. This can result in decomposition to copper (I) chloride:
- Cu + CuCl2 → 2 CuCl
- Do not store in acidic conditions.
Disposal
- Combining with sodium hydroxide produces insoluble copper hydroxide, which will then absorb carbon dioxide from the air, resulting in nature-safe carbonate/hydroxide compounds equivalent to malachite and azurite
- Combining with sodium bicarbonate or sodium carbonate shortcuts the carbon dioxide absorption and produces the mineral forms of copper directly.
See Also
References
- ↑ US patent 2586579 "Method of production of cuprous oxide and copper chlorides"
Link courtesy Google - ↑ Borisov, V.A.; D’yachenko, A.N; Kraidenko, R.I. (2011) "Reaction of Ammonium Chloride with the Copper(II) Sulfide and Oxide, and Identification of the Reaction Products"
Russian Journal of General Chemistry (2) (PDF) Reaction of ammonium chloride with the copper(II) sulfide and oxide, and identification of the reaction products. Available from: https://www.researchgate.net/publication/251412801_Reaction_of_ammonium_chloride_with_the_copperII_sulfide_and_oxide_and_identification_of_the_reaction_products [accessed Jan 23 2020]. 81(7); pp1430–1433.
DOI:10.1134/S107036321107005X
link courtesy researchgate.