Aufelio J S Page3


Tools :

- two beaker
- One zinc and iron blade
- a copper sulphate

necessary protective Equipment

- protective goggles
- a blouse (closed attention!)
- work under ventilated hood (because of sulphate vapours)

necessary material (solution or products)

A solution of copper sulfate is necessary , moreover, we can possibly realize this experience by dry voice, ie take a ribbon of magnesium and make it burn by the beak bunsen

estimated time

the estimated time is about half an hour or forty five minutes, this includes the preparation time (longer than the reaction!)

The purpose of the experiment

An oxidant is a chemical species that can gain one or more electrons during a reaction in which it shrinks.

A reducer is a chemical species that can lose one or more electrons during a reaction in which it oxidizes.

An oxydorination reaction is characterized by a transfer of electrons from a reducer from one redox torque to an oxidant from another torque. the desired purpose of this experiment is to model the transfer of electrons from one species to another and to visualize the oxidation of a species (here zinc or iron)

possible risks and dangers

there are several risks, the first is biological, the solution after experience must be emptied in a can suitable for the pH of this solution and not be emptied at the evier, then there is the physical risk, this solution is corrosive and the oxydoreduction forms vapors so the manipulation must be done under ventilated hood and this solution should not be inhaled.


1) bring the beaker and rinse it with distilled water, then fill it half of the copper sulphate solution
2) dip the zinc blade and wait for the appearance of orange residue (copper) on the blade
3) observe the result and repeat the same protocol with an iron blade
4) remove the blades with prtecaution and empty the becher in the appropriate can.
5) make the record take into account the reaction équations


the first beaker is a formation of a copper deposit
the second beaker , this is the end of the reaction the zinc atom replaced the copper atom in the solution whose equation is as follows:

A conclusion

finally, we can conclude that here the redox reaction has taken place, because on the zinc slide, the copper deposit is present

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