Represent symbolically the galvanic cells in which the following reaction occurs. Calculate the standard electromotive forces of the cells :
(1) `Fe+CuSO_(4)rarr FeSO_(4)+Cu`
Given : `E_(Fe^(2+)|Fe)^(@)=-0.44V, E_(Sn^(2+)|Zn)^(@)=-0.14V`,
`E_(Cu^(2+)|Cu)^(@)=0.34V, E_(Zn^(2+)|Zn)^(@)=-0.76V`,
`E_(H^(+)|(1)/(2)H_(2))^(@)=0.00V`.

Explanation

In the reaction, Fe is oxidised to `Fe^(2+) (FeSO_(4))` and `Cu^(2+)` is reduced to Cu.
As reduction occurs at the cathode, `Cu|CuSO_(4)` will be the cathode and `Fe|FeSO_(4)` will be the anode.
According to convention, the anode is written on the left hand side, and the cathode on the right hand side.
The symbolic presentation of the cell is
`Fe|Fe^(2+)||Cu^(2+)|Cu, or Fe|FeSO_(4)(aq)||CuSO_(4)(aq)|Cu`.
For the cell `E_("cell")^(2)=E_("cathode")^(@)-E_("anode")^(@)`
`=[(+0.34)-(-0.44)]V=0.78V`