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Transcript

Chemical Reaction

C + 2CuO => CO₂ + Cu₂

Equipment

Procedure

  • Crucible And Lid
  • Bunsen Burner
  • Tripod
  • Bench Mat
  • Pipe Clay Triangle
  • Copper Oxide
  • Carbon
  • Tin Can With Bottom Removed Or Aluminium Foil
  • 2 Teaspoons
  • An Icy-Pole Stick
  • Tongs
  • Stereomicroscope
  • Place about one teaspoon of copper oxide into the crucible.
  • Use a different teaspoon to add about a half teaspoon carbon powder to the mixture. DO NOT mix up the two teaspoons.
  • Use the icy-pole to thoroughly stir the mixture.
  • Use the carbon teaspoon to add another teaspoon of carbon to the mixture but DO NOT mix through.
  • Put a lid on the crucible and stand it in a pipe clay triangle on a tripod stand. Place the tin on the tripod so that it surrounds the crucible (see diagram).
  • Light the Bunsen Burner and heat the crucible on a hot flame with the tin can (or aluminium foil) for about 10 minutes.
  • Let the crucible cool for several minutes. Using tongs, tip the contents of the crucible onto a tin lid or other container that will not melt. Allow it to cool.

Observations

Aim

The aim of the experiment was to reduce copper oxide to its purest form by heating it up to boiling point. After this we recorded what we saw.

After the crucible had cooled I saw two different colours of powder one was black and I expected that to be the carbon and the rest of the copper oxide, and reddish brown which I expected to be the reduced copper.

Discussion

Conclusion

Before we heated the mixture we had two similar coloured powders, the carbon and the copper oxide, but after the heating there was two different colours, red/brown and black/grey. I came to realise that the red/brown was the copper. The reason carbon reduction doesn't work as well with iron is because it is less reactive than copper.

To get copper oxide first you must use oxidisation and to then turn it back to copper you use carbon reduction.

Carbon Reduction Of Copper Oxide

By Dean Smith

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