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 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

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]

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

Calculate the EMF of the cell, containing nickel and copper electrodes. Given E^@(NI^(2+)|NI)=-0.25V and 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

Calculate the emf of cell, Al|Al^(3+)||Cu^(2+)|Cu Given : E^(@) (Al^(3)|Al) = - 1.66V and E^(@) (Cu^(2+)|Cu) = + 0.34 V

A copper silver cell is set up. The copper ion concentration is 0.10 M. the concentration of silver ion is not known. The cell potential when measured was 0.422V. Determine the concentration of silver ions in the cell. Given: E_(Ag^+|Ag)=+0.80V , E_(Cu^(2+)|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.