Given
`E_(Ag^(+)//Ag)^(@)=0.80V`, `E_(Mg^(2+)//Mg)^(@)=-2.37V`,
`E_(Cu^(2+)//Cu)^(@)=0.79 E_(Hg^(2+)//Hg)^(@)=1.71V`
Which of the following statements is/are correct?

Options

A. `AgNO_(3)` can be stored in copper vessel
B. `CU(NO_(3))_(2)` can be stored in copper vessel magnesium vessel
C. `CUCl_(2)` can be stored in silver vessel
D. `Hg_(2)Cl_(2)` can be stored in copper vessel

Explanation

To solve the problem, we need to analyze the given standard reduction potentials and determine whether the specified compounds can be stored in the respective vessels based on the reactivity of the metals involved.

### Step-by-Step Solution:

1. **Understanding Standard Reduction Potentials**:
- The standard reduction potentials (E°) indicate the tendency of a species to gain electrons (be reduced). A higher E° value means a greater tendency to be reduced, while a lower E° value indicates a more reactive species that is likely to lose electrons (be oxidized).

2. **Given Values**:
- \( E^{\circ}_{Ag^+/Ag} = 0.80 \, V \)
- \( E^{\circ}_{Mg^{2+}/Mg} = -2.37 \, V \)
- \( E^{\circ}_{Cu^{2+}/Cu} = 0.79 \, V \)
- \( E^{\circ}_{Hg^{2+}/Hg} = 1.71 \, V \)

3. **Analyzing Each Statement**:

**Statement 1**: AgNO3 can be stored in a copper vessel.
- **Analysis**:
- Copper (Cu) has a lower reduction potential (0.79 V) than silver (Ag) (0.80 V). This means copper is more reactive and can displace silver from its compound.
- **Conclusion**: This statement is **incorrect**.

**Statement 2**: Mg(NO3)2 can be stored in a copper vessel.
- **Analysis**:
- Magnesium (Mg) has a much lower reduction potential (-2.37 V) compared to copper (0.79 V). This indicates that magnesium is more reactive than copper.
- Therefore, magnesium will not react with the copper vessel, and Mg(NO3)2 can be stored in it.
- **Conclusion**: This statement is **correct**.

**Statement 3**: CuCl2 can be stored in a silver vessel.
- **Analysis**:
- Copper (Cu) has a lower reduction potential (0.79 V) than silver (0.80 V). Thus, copper is more reactive and cannot be displaced by silver.
- Therefore, CuCl2 can be safely stored in a silver vessel.
- **Conclusion**: This statement is **correct**.

**Statement 4**: Hg2Cl2 can be stored in a copper vessel.
- **Analysis**:
- Mercury (Hg) has a higher reduction potential (1.71 V) compared to copper (0.79 V). This means that copper is more reactive and can displace mercury from its compound.
- Therefore, Hg2Cl2 cannot be stored in a copper vessel.
- **Conclusion**: This statement is **incorrect**.

4. **Final Conclusions**:
- The correct statements are:
- Statement 2: Mg(NO3)2 can be stored in a copper vessel.
- Statement 3: CuCl2 can be stored in a silver vessel.

### Summary of Correct Statements:
- **Correct Statements**: 2 and 3.