A cell is prepared by dipping a copper rod in 1m cuso4 solution and a nickel rod in nickel sulphate solution
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When Zn metal is dissolved in CuSO4 solution, then the following redox reaction takes place:
Zn(0)+CuSO4(II)→ZnSO4(II)+Cu(0)
This is because Zn has a higher tendemcy to get oxidised, owing to its higher oxidation potential.
The first observation is the change of colour of the solution from blue( due to CuSO4 solution) to colourless (due to ZnSO4 solution).
Also, the reduced copper metal may deposit on the base of the vessel.
When Zn metal is dissolved in CuSO4 solution, then the following redox reaction takes place:
Zn(0)+CuSO4(II)→ZnSO4(II)+Cu(0)
This is because Zn has a higher tendemcy to get oxidised, owing to its higher oxidation potential.
The first observation is the change of colour of the solution from blue( due to CuSO4 solution) to colourless (due to ZnSO4 solution).
Also, the reduced copper metal may deposit on the base of the vessel.
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