Can a solution of 1 M copper sulphate be stored in a vessel made of nickel metal? Given that
`E_(Ni^(+2)//Ni)^(@)=0.25 " volt and "E_(Cu^(+2)//Cu)^(@)=+0.34" volt"`.

Explanation

To determine whether a solution of 1 M copper sulfate can be stored in a vessel made of nickel metal, we need to analyze the electrochemical properties of nickel and copper based on their standard reduction potentials.

### Step 1: Understand the Standard Reduction Potentials
The standard reduction potentials provided are:
- \( E^{\circ}_{Ni^{2+}/Ni} = 0.25 \, \text{V} \)
- \( E^{\circ}_{Cu^{2+}/Cu} = +0.34 \, \text{V} \)

### Step 2: Compare the Reduction Potentials
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