Satement 1 A solution of `FeSO_(4)` can be stored in a copper vessel
Statement 2 `E^(0) "of" Cu < E^(0)` of Fe

Options

A. Statement 1 is true statement 2 is true , statement 2 is a corrrect explanation for statement 1
B. Statement 1 is true statement 2 is true statement 2 is not a correct explanation for statement 1
C. Statement 1 is true statement 2 is false
D. Statement 1 is false statement 2 is true

Explanation

To analyze the statements provided in the question, we will evaluate each statement based on the principles of redox reactions and electrochemistry.

### Step-by-Step Solution:

1. **Understanding Statement 1**:
- The statement claims that a solution of `FeSO4` can be stored in a copper vessel.
- To determine if this is true, we need to consider the reactivity of iron (Fe) and copper (Cu).

2. **Reactivity Series**:
- In the reactivity series, metals are arranged in order of decreasing reactivity.
- Iron is more reactive than copper. This means that iron can displace copper from its compounds, but not vice versa.

3. **Conclusion for Statement 1**:
- Since iron is more reactive than copper, a copper vessel will not react with `FeSO4`. Therefore, it is safe to store `FeSO4` in a copper vessel.
- **Statement 1 is true**.

4. **Understanding Statement 2**:
- The statement claims that the standard reduction potential (E°) of copper is less than that of iron.
- The standard reduction potential for copper (Cu²⁺ + 2e⁻ → Cu) is +0.34 V, while for iron (Fe²⁺ + 2e⁻ → Fe) it is -0.44 V.

5. **Comparison of Standard Reduction Potentials**:
- Since +0.34 V (Cu) is greater than -0.44 V (Fe), this means that copper has a higher reduction potential than iron.
- **Statement 2 is false**.

6. **Final Conclusion**:
- Statement 1 is true: A solution of `FeSO4` can be stored in a copper vessel.
- Statement 2 is false: The E° of copper is greater than that of iron, not less.

### Summary:
- Statement 1: True
- Statement 2: False