Question

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Answer 1

ANSWER...

THE COLOR OF IRON NAIL CHANGES WHEN COPPER SULPHATE IS ADDED ON IT DUE TO THE PROCESS OF CHEMICAL REACTION. DISPLACEMENT REACTION TAKES PLACE IN THIS PROCESS. THE IRON NAIL DISPLACES COPPER FROM ITS AQUEOUS SOLUTION.

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Answer 2

Question:

Explain the following process/events:

Put two to three iron nails in the blue solution of copper sulphate and after 15 to 20 minutes the color of the solution turns green.

Answer:

If we put two to three iron nails in the blue solution of copper sulphate solution, then after sometime the color of the solution turns green. This is because iron displaces copper from its salt solution and therefore iron sulphate is formed which is green in color, and copper is deposited on the iron nails.

How iron displaces copper from its salt solution?

Iron displaces copper from its salt solution because iron is more reactive than copper, and therefore a displacement reaction takes place between the two. The end products of this displacement reaction are copper (reddish-brown) on the iron nails and iron sulphate solution (green in color).

Chemical equation:

Fe (iron) + $CuSO_{4}$ (blue) ⇒ $FeSO_{4}$ (green) + Cu (reddish-brown deposit on iron nails).

What are displacement reactions?

Displacement reactions are those reactions in which a more reactive metal displaces a less reactive metal from its salt solution.

☆NOTE:

Fe (iron) + $CuSO_{4}$ (blue) ⇒ $FeSO_{4}$ (green) + Cu (reddish-brown deposit on iron nails).

But,

$FeSO_{4}$ (green) + Cu ⇒ No displacement reaction.

This is because here we have salt solution of iron. So, in this case copper can't displace iron from its salt solution as it is less reactive than iron.