Can we use a copper vessel to store 1 M AgNO3 solution? Given that
`E_(Cu^(2+)| Cu )^(0)` = + 0.34 volt and `E_(Ag^(+)| Ag )^(0)` = 0.80 volt

Explanation

To determine whether we can use a copper vessel to store a 1 M AgNO3 solution, we need to analyze the electrochemical potentials of the two half-reactions involved: the reduction of silver ions (Ag⁺) and the reduction of copper ions (Cu²⁺).

### Step-by-Step Solution:

1. **Identify the Standard Reduction Potentials:**
- The standard reduction potential for the reaction involving silver ions is given as:
\[
E^\circ_{Ag^+/Ag} = +0.80 \, \text{V}
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