When a rod of copper is immersed in a solution of `ZnSO_(4)` zinc gets precipitated.

Answer

**Step-by-Step Solution:**

1. **Identify the Reaction Type**: The reaction described is a single displacement (or single replacement) reaction. In this type of reaction, a more reactive metal displaces a less reactive metal from its compound.

2. **Refer to the Reactivity Series**: The reactivity series of metals helps us determine which metal can displace another. The order from most reactive to least reactive is:
- Sodium > Potassium > Calcium > Magnesium > Aluminum > Zinc > Iron > Tin > Lead > Hydrogen > Copper > Mercury > Silver > Gold > Platinum.
From this series, we can see that zinc (Zn) is more reactive than copper (Cu).

3. **Analyze the Given Reaction**: The question states that when a copper rod is immersed in a solution of zinc sulfate (ZnSO₄), zinc gets precipitated. This implies that copper is somehow displacing zinc from the solution, which contradicts the reactivity series.

4. **Determine the Correct Displacement**: Since zinc is more reactive than copper, it cannot be displaced by copper. Instead, zinc would displace copper if the reaction were to occur. The correct reaction would be:
\[ Zn + CuSO_4 \rightarrow ZnSO_4 + Cu \]
Here, zinc displaces copper from copper sulfate (CuSO₄), resulting in the formation of zinc sulfate (ZnSO₄) and solid copper (Cu) as a precipitate.

5. **Conclusion**: The statement in the question is incorrect. Copper does not displace zinc; rather, zinc displaces copper due to its higher reactivity.

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