Question

Can copper sulphate(${\mathrm{CuSO}}_4$) solution be stored in an iron container?

• A. No, because copper is more reactive than iron
• B. No, because iron is more reactive than copper, therefore reaction takes place
• C. Yes, because copper is less reactive than copper
• D. Yes, because copper is more reactive than iron

Answer 1

The correct option is B

No, because iron is more reactive than copper, therefore reaction takes place

No, we can not store copper sulphate solution in an iron container because iron is more reactive than copper, therefore reaction will take place.

Reactivity depends upon the oxidation potential of the elements which have been recorded with respect to Hydrogen.

The reactivity series is as follows:

Potassium(K)

Sodium(Na)

Calcium(Ca)

Magnesium(Mg)

Aluminium (Al)

Carbon(C)

Zinc(Zn)

Iron(Fe)

Tin(Sn)

Lead(Pb)

Hydrogen(H)

Copper(Cu)

Silver(Ag)

Gold(Au)

This is the decreasing order of reactivity of different elements so the element which is present below the other element can not displace it from its salt solution but an element present above can displace the lower element from its salt solution.

As we can see iron(Fe) is above the copper(Cu) in the reactivity series so iron will displace copper from its solution. The reaction will be as follows:

$\mathrm{Fe}\left(\mathrm{s}\right)+{\mathrm{CuSO}}_4\left(\mathrm{aq}\right)\to {\mathrm{FeSO}}_4\left(\mathrm{aq}\right)+\mathrm{Cu}\left(\mathrm{s}\right)$

This is the reason why we can not store copper sulphate in an iron container.