Aqueous solutions of zinc sulphate and iron sulphate were taken in test tubes I and II by four students A, B, C, and D. Metal pieces of iron and zinc were dropped in the two solutions, and observations made after several hours were recorded in the form of a table as given below:
| Student Solution | Metal | Solution | Colour change Deposit/coating of solution | Deposit/coating obtained |
|---|
| A | Fe | ZnSO4 | Turned green | Silvery grey deposit |
| Zn | FeSO4 | No change | No change |
| B | Fe | ZnSO4 | No change | Black deposit |
| Zn | FeSO4 | Colour faded | Grey coating |
| C | Fe | ZnSO4 | No change | No change |
| Zn | FeSO4 | Turned colourless | Black deposit |
| D | Fe | ZnSO4 | No change | Grey deposit |
| Zn | ZnSO4 | No change | Black deposit |
Which student has given the correct report?
- A
- D
- A
- C
"
Correct Answer: (d) C
Explanation: Fe is less reactive than zinc.
$Fe(s) + ZnSO_4(aq) \rightarrow no \ reaction$
Zn is more reactive than Fe, so it displaces iron as follows:
$Zn(s) + FeSO_4(aq) (green) \rightarrow ZnSO_4(aq) (colourless) + Fe(s) (black \ deposit)$
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