Question

A solution of cuso4 was kept in an iron pot after few days the iron pot was found to have a number of holes in it explain the reason in terms of reactivity write the equation to the reaction involved

Answer 1

A solution of copper sulphate $\sf{(CuSO_4)}$ was kept in iron $\sf{(Fe)}$ soltion.

The following reaction takes place :

$\sf{Fe\:+\:CuSO_4\:\rightarrow\:FeSO_4\:+\:Cu}$

As Fe is more reactive than Cu (according to reactivity series) so, it displaces Cu from CuSO4 and react with Fe to give FeSO4 and Cu.

Here.. more reactive metal displaces less reactive metal from it's salt solution. So, it is knwon as Displacement reaction.

Now, again coming back to the question.

Iron is more reactive than copper due to this it displaces copper from it's solution. After that reaction (which is shown above) iron becomes ferrous sulphate.

Since, iron is consumed holes appear on the pot.

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What is reactivity series?

=> Series of metals in the decreasing order is knwon as Reactivity series.

K = Potassium

Na = Sodium

Ca = Calcium

Mg = Magnesium

Al = Aluminum

Zn = Zinc

Fe = Iron

Pb = Lead

H = Hydrogen

Cu = Copper

Hg = Mercury

Ag = Silver

Au = Gold

(Reactivity decreases down the group. Means, Potassium is most reactive metal and Gold is least reactive. )

Answer 2

Answer:

Explanation:

A solution of CuSO₄ was kept in an iron pot , and after few days no: of holes were seen in the pot.

Iron(Fe) being more reactive than copper , displaced copper from its solution.

Hence, Iron became ferrous sulphate after this reaction , and due to this holes were produced in the pot.

Here is the reaction that takes place :-

Fe + CuSO₄ ------> FeSO₄ + Cu

( In the reactivity series of metals, Iron is placed above copper, hence Iron is more reactive than copper)