Question

1. What are displacement reactions? Explain these
with reference to iron and copper sulphate
solution​

Answer 1

Answer:

Displacement reactions are the one in which one element displaces (replaces) other element from its solution (in case of CuSO4)

Let's consider this eg:

Fe + CuSO4 ------> FeSO4 + Cu

in the above reaction, Iron displaces copper from its copper sulphate solution to form Ferrous sulphate.

Why does Iron displace copper? Why not the reverse?

Iron metal is more reactive than copper. Therefore, it can displace copper from copper sulphate (CuSO4) solution. Cu is less reactive than iron, therefore, cannot replace iron from iron sulphate (FeSO4).

Answer 2

$\huge\underline\mathfrak\purple{ANSWER}$

$\large\mathbb\blue{DISPLACEMENT\:REACTION}$

Displacement reaction: It is a chemical change in which a more active element displaces a less active element from its salt solution. (any compound)

AB + C —> AC + B

Element C displaces, element B from the compound AB.

CuSO4 + Zn —> ZnSO4 + Cu

Explanation; Take a solution of copper sulphate in a beaker, add a few pieces of zinc and stir with a glass rod. The blue colour of the solution gradually fades, and soon the solution becomes colourless. At the same time, reddish brown particles of copper settle down in the beaker. Here, zinc displaces copper from its compound copper sulphate.

From the above example, it can be noticed that in metals, zinc is more active(reactive) than copper.

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