Which one of the following chemical reactions is not feasible?
- A.Fe + CuSO4 → FeSO4 + Cu
- B.Zn + CuSO4 → ZnSO4 + Cu
- C.Cu + PbCl2 → CuCl2 + Pb
- D.Mg + CuSO4 → MgSO4 + Cu
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Explanation
The correct answer is C, Cu + PbCl2 → CuCl2 + Pb. Copper is less reactive than lead, so it cannot push lead out of its compound.
In a displacement reaction, a more reactive metal takes the place of a less reactive metal in its salt solution. The reactivity series, from more to less reactive, runs: potassium, sodium, calcium, magnesium, aluminium, zinc, iron, lead, hydrogen, copper, mercury, silver, gold. Magnesium, zinc and iron are all above copper, so each of them displaces copper from copper sulphate; the blue solution fades and reddish-brown copper is deposited. Copper, however, lies below lead, so it has no power to displace lead from lead chloride.
A is wrong: iron is more reactive than copper, so this reaction takes place, the classic iron nail in copper sulphate experiment.
B is wrong: zinc is above copper in the series and readily displaces it.
D is wrong: magnesium is far more reactive than copper and displaces it easily.
Exam tip: a metal displaces only those below it in the reactivity series: K, Na, Ca, Mg, Al, Zn, Fe, Pb, H, Cu, Hg, Ag, Au.