Can a solution of 1 M `ZnSO_(4)` be stored in a vessel made of copper ? Given that
`E_(Zn^(+2)//Zn)^(@) =-0.76V and E_(Cu^(+2)//Cu)^(@)=0.34 V`

Explanation

To determine whether a solution of 1 M ZnSO₄ can be stored in a vessel made of copper, we need to analyze the electrochemical properties of zinc and copper using their standard electrode potentials.

### Step-by-Step Solution:

1. **Identify the Half-Reactions and Standard Electrode Potentials:**
- The reduction half-reaction for zinc is:
\[
\text{Zn}^{2+} + 2e^- \rightarrow \text{Zn} \quad E^\circ = -0.76 \, \text{V}
...