Carbonate Decomposition
Aim: To investigate the decomposition of a carbonate.
Equipment:
· Copper Carbonate (CuCO3)
· Limewater
· Bunsen Burner
· Matches
· Test tubes
· Clamp and stand
· Hydrochloric Acid
· Electronic Scales
Method:
1. Weighed Copper Carbonate by taring empty test tube.
2. Placed some Copper Carbonate in a test tube fitted with gas delivery tube
and stopper.
3. Clamped the test tube to the stand at a slight angle.
4. Half filled another test tube with limewater and placed the other end of gas
delivery tube into it.
5. Using a small blue flame gently heated the carbonate. Observed what
happened.
6. Removed gas tube from limewater before turning off the Bunsen burner.
7. Allowed to cool
8. Weighed the remaining Copper Carbonate.
9. Added approximately 5ml of Hydrochloric Acid to the solid residue (Copper
Oxide) from the decomposition reaction.
10. Transferred a small amount of original Copper Carbonate to new test tube
and added same amount of Hydrochloric Acid to that. Recorded observations.
Results: Observations from Decomposition: The limewater turned milky.
Observations from HCl & Copper Oxide: Small bubbles. Hardly a reaction.
Observations from HCl & Copper Carbonate: Bubbles & fizzing. Small amount
of heat generated. Turned milky green in colour. Reacted immeadiately.
Conclusion: The limewater proved that Carbon Dioxide was produced as a result of thedecomposition reaction.
The Copper Oxide test showed that theoretically there should be no reaction with HCl. Copper Carbonate, however, theoretically, should react.
Evaluation: Overall, the experiment was a success except for the fact that the HCl shouldn'thave reacted with the Copper Oxide but did. This is probably due to the fact there
was some Copper Carbonate still stuck to the side of the test tube and the HCl
reacted with that.
The process of extracting copper of copper carbonate
The concentrated ore is heated strongly with silicon dioxide (silica) and air or oxygen in a furnace or series of furnaces.
The copper(II) ions in the chalcopyrite are reduced to copper(I) sulphide (which is reduced further to copper metal in the final stage).
The iron in the chalcopyrite ends up converted into an iron(II) silicate slag which is removed.
Most of the sulphur in the chalcopyrite turns into sulphur dioxide gas. This is used to make sulphuric acid via the Contact Process.
An overall equation for this series of steps is:
The copper(I) sulphide produced is converted to copper with a final blast of air.
Strongly heating Copper carbonate makes it decompose into black Copper(II) oxide (CuO) and Carbon dioxide. When this black powder is reacted with reducing agents like hydrogen or Carbon monoxide it is reduced to elementary copper.
CuO + H2 ----> Cu + H2O
CuO + CO ----> Cu + CO2
It can also be reacted with concentrated Phenol to yield copper.
C6H5OH + CuO ----> CO2 + H2O + Cu
You don't. Copper ore CONTAINS copper oxide.
Copper sulfate(sulphate) can be made by adding Copper Oxide to a beaker full of sulfuric acid. Water is also created as well.
Copper can be found by mining it from various countries. It is a natural mineral so it does not need to be made.
You heat the copper carbonate to create copper oxide but I'm not sure what temperature you have to heat it to.
Because it is easier. The molecular formula of copper carbonate is CuCO3. When it decomposes it loses a CO2 molecule. If it became Copper 1 oxide(Cu2O then it would have to combine with another molecule(releasing O). Instead it becames copper2 oxide(CuO) because that is an easier transition.
CuCO3 + Heat --> CuO + O2 Green Copper Carbonate when heated will form Copper Oxide and Oxygen
This compound is the copper(II) oxide, CuO.
Magnesium + copper oxide --> magnesium oxide + copper
These two compunds form Calcium Hydroxide and Copper oxide
They form magnesium oxide, copper oxide etc. and will form carbon dioxide as a byproduct.
Here are the equations for the thermal decomposition of copper carbonate (notice that a metal oxide is formed, just as it was with calcium carbonate): Copper carbonate → copper oxide + carbon dioxide CuCO3 → CuO + CO2
Because it is easier. The molecular formula of copper carbonate is CuCO3. When it decomposes it loses a CO2 molecule. If it became Copper 1 oxide(Cu2O then it would have to combine with another molecule(releasing O). Instead it becames copper2 oxide(CuO) because that is an easier transition.
CuCO3 + Heat --> CuO + O2 Green Copper Carbonate when heated will form Copper Oxide and Oxygen
Carbonate by itself is an ion that does not contain copper and therefore could not produce copper if heated. However, because carbonate is a negatively charged ion, no substantial number of carbonate ions can exist stably except in association with an equal number of positively charged cations to neutralize the electrical charge of the carbonate ions. If these cations are cations of copper, then copper oxide can be produced by heating the copper carbonate salt.
This compound is the copper(II) oxide, CuO.
Because it undergoes thermal decomposition. If you give heat to Copper (II) carbonate, it will decompose to form Copper (II) oxide. Instead of saying green copper carbonate, I guess it is safer and better to say copper (II) carbonate.
You get copper (I) oxide which is red and copper (II) oxide that is black. Copper (II) oxide is more stable. In moist air it also forms copper hydroxide and copper carbonate giving the known green color.
Magnesium + copper oxide --> magnesium oxide + copper
Copper Carbonate when heated decomposes to give copper oxide and carbon dioxide.
Copper carbonate is a chemical substance, also called Cupric carbonate. The molecular formula is CuCO3. Copper carbonate decomposes at high temperatures, giving off carbon dioxide and leaving copper(II) oxide.
These two compunds form Calcium Hydroxide and Copper oxide