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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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Can we store copper sulphate solution in an iron vessel ?

Can a nickel spoon be used to stir a solution of copper sulphate ? Support your answer with reason. [E^(@)(Ni^(2+)//Ni)= -0.25V,E^(@)(Cu^(2+)//Cu)=+0.34V]

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

Can a zinc spoon be used to stir a solution of copper sulphate? Support your answer with reason E_(Zn^(2+)|Zn)^@=-0.76V , E_(Cu^(2+)|Cu)^@=+0.34V

Calculate DeltaG^(@) for the following cell: Fe|Fe^(2+)||Cu^(2+)|Cu . Given that: E^(@)(Cu^(2+)//Cu)=+0*34V,E^(@)(Fe^(2+)//Fe)=-0*44V.

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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