Question

Samples of four metals $A,B,C\text{and}D$ were taken and added to ferrous sulphate solution one by one in different beakers. Metals $A\text{and}B$ showed changes in colour, whereas metals $C\text{and}D$ did not. What do you infer from this?

• A. Metals $A\text{and}B$ are less reactive than iron.
• B. Metals $C\text{and}D$ are more reactive than iron.
• C. Metals $A\text{and}B$ are more reactive than iron.
• D. Metals $A\text{and}B$ are less reactive, whereas metals C and D are more reactive than iron

Answer 1

The correct option is C Metals $A\text{and}B$ are more reactive than iron.

The reaction in which a more reactive metal displaces a less reactive metal from its solution is known as displacement reaction.

Here, metals $A\text{and}B$ show changes in colour when added to the solution of ferrous sulphate. The possible reactions can be as follows:
$A+FeS{O}_4\to AS{O}_4+Fe$
$B+FeS{O}_4\to BS{O}_4+Fe$

Metals $C\text{and}D$ do not show any changes in colour as there is no reaction takes place because metals $C\text{and}D$ are less reactive than iron.