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Can we store copper sulphate solution in...

Can we store copper sulphate solution in iron vessel? Give suitable explanation in support of your answer
`[E°(Cu^(2+)//Cu)=+0.34V,E°(Fe^(2+)//Fe)=-0.44V]`

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Reduction potential of iron is less so iron undergoes oxidation and `Cu^(2+)` get reduced.
`Fe(s) + CuSO_(4)(aq) rarr FeSO_(4) (aq) + Cu(s)`
Hence blue colour of `CuSO_(4)` gets discharged.
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Can we store copper sulphate solution in an iron vessel ?

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Can Chlorine gas be stored in Copper Cylinder ? Given E_(Cu^(+)//Cu)^(@)= 0.34V and E_(Cl_(2)//Cl)^(@)= 1.36V

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Write the Nernst equation for the above cell, if E^@(Zn^(2+)|Zn)=-0.76V, E^@(Cu^(@+)|Cu)=+0.34V

Calculate the electrode potential at copper electrode dipped in a 0.1 M solution of copper sulphate at 298K, assuming CuSO_4 to be completely ionised. The standard electrode potential of Cu^(2+)|Cu is 0.34V at 298K.

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