When Zn piece is kept in `CuSO_(4)` solution, the copper get precipitated due to standard potential of zinc is

Options

A. `gtcopper`
B. `ltcopper`
C. `gt`sulphide
D. `lt`sulphate

Explanation

To solve the problem, we need to analyze the reaction that occurs when a piece of zinc (Zn) is placed in a copper sulfate (CuSO₄) solution. The key here is to understand the standard reduction potentials of zinc and copper.

### Step-by-Step Solution:

1. **Identify the Reaction**:
When zinc is placed in a copper sulfate solution, the following reaction occurs:
\[ \text{Zn} + \text{CuSO}_4 \rightarrow \text{ZnSO}_4 + \text{Cu} \]

2. **Determine Oxidation States**:
- Zinc (Zn) starts with an oxidation state of 0 and ends with +2 in ZnSO₄.
- Copper (Cu) starts with an oxidation state of +2 in CuSO₄ and ends with 0 in elemental copper (Cu).

3. **Identify Oxidation and Reduction**:
- Zinc is oxidized:
\[ \text{Zn} \rightarrow \text{Zn}^{2+} + 2e^{-} \]
- Copper is reduced:
\[ \text{Cu}^{2+} + 2e^{-} \rightarrow \text{Cu} \]

4. **Standard Reduction Potentials**:
- The standard reduction potential for zinc (Zn²⁺/Zn) is approximately -0.77 V.
- The standard reduction potential for copper (Cu²⁺/Cu) is approximately +0.34 V.

5. **Comparison of Standard Potentials**:
- Since the standard reduction potential for copper is higher than that of zinc, this indicates that copper ions (Cu²⁺) are more likely to be reduced than zinc atoms (Zn) are to be oxidized.

6. **Conclusion**:
- Because zinc can reduce copper ions to copper metal, we conclude that zinc is a stronger reducing agent than copper. Therefore, the standard potential of zinc is less than that of copper.

### Final Answer:
The standard potential of zinc is less than that of copper.