The positive value of the standard electrode potential of `Cu^(2+)// Cu` indicates that ……………
1) This redox couple is a strongest reducing agent than the `H^(+)//H_(2)` couple.
2) This redox couple is a stronger oxidising agent than `H^(+)//H_(2)`
3) Cu cannot displace `H_(2)` from acid.
4) Cu cannot displaced `H_(2)` from acid.

Options

A. 2 & 4
B. Only 2
C. 3 & 4
D. 1 7 4

Answer

To solve the question regarding the standard electrode potential of the redox couple `Cu^(2+)//Cu`, we need to analyze the implications of a positive standard electrode potential.

### Step-by-Step Solution:

1. **Understanding Standard Electrode Potential**:
- The standard electrode potential (E°) indicates the tendency of a species to be reduced. A positive E° value means that the species has a strong tendency to gain electrons and undergo reduction.

2. **Analyzing the Redox Couple**:
- For the redox couple `Cu^(2+)//Cu`, the half-reaction can be written as:
\[ Cu^{2+} + 2e^- \rightarrow Cu \]
- Since the standard electrode potential for this reaction is positive, it indicates that `Cu^(2+)` is a good oxidizing agent.

3. **Comparison with Hydrogen Electrode**:
- The standard hydrogen electrode (SHE) has a potential of 0 V:
\[ 2H^+ + 2e^- \rightarrow H_2 \]
- Since the E° for `Cu^(2+)//Cu` is positive, it implies that `Cu^(2+)` has a greater tendency to be reduced compared to `H^+`, making it a stronger oxidizing agent than the hydrogen ion.

4. **Evaluating the Statements**:
- **Statement 1**: "This redox couple is a stronger reducing agent than the `H^(+)//H_(2)` couple." - This is incorrect because `Cu^(2+)` is an oxidizing agent, not a reducing agent.
- **Statement 2**: "This redox couple is a stronger oxidizing agent than `H^(+)//H_(2)`." - This is correct because of the positive E° value.
- **Statement 3**: "Cu cannot displace `H_(2)` from acid." - This is incorrect because if `Cu` is placed in an acid, it will not displace hydrogen due to its higher reduction potential.
- **Statement 4**: "Cu cannot displace `H_(2)` from acid." - This is correct as it reiterates the same idea as statement 3.

5. **Conclusion**:
- The correct statements are 2 and 4. Therefore, the answer to the question is that the positive value of the standard electrode potential of `Cu^(2+)//Cu` indicates that it is a stronger oxidizing agent than `H^(+)//H_(2)` and that `Cu` cannot displace `H_(2)` from acid.

### Final Answer:
The correct options are:
2) This redox couple is a stronger oxidizing agent than `H^(+)//H_(2)`.
4) Cu cannot displace `H_(2)` from acid.