See whether the cell representation given below is in accordance with the conventation or not. If it is not, then write the correct representation and reaction of the cell. Calculate the standard EMF of the cell: `Cu|Cu^(2+)||Zn|Zn^(2+)`.
`["Given : "E_(Cu^(2+)|Cu)^(@)=+0.34V, E_(Zn^(2+)|Zn)^(@)=-0.76V]`

Explanation

For the given Cell,
`E_("cell")^(@)=E_("cathode")^(@)-E_("anode")^(@)=(-0.76-0.34)V=-1.10V`
The negative value of `E_("cell")^(@)` indicates that the cell reaction for the cell is not spontaneous. Hence, the cell representation is not correct.
Since `E_(Zn^(2+)|Zn)^(@) lt E_(Cu^(2+)|Cu)^(@)`, the cell should consists of `Zn^(2+)|Zn` half - cell as the anode and `Cu^(2+)|Cu` half - cell as the cathode, So, the correct representation of the cell will be `Zn|Zn^(2+)||Cu^(2+)|Cu`
For this cell, Anode reaction : `Zn(s)rarr Zn^(2+)(aq)+2e`
Cathode reaction : `Cu^(2+)(aq)+2e rarr Cu(s)`
and the cell reaction : `Zn(s)+Cu^(2+)(aq)rarr Zn^(2+)(aq)+Cu(s)`
The electromotive force of the cell is
`E_("cell")^(@)=E_("cathode")^(@)-E_("anode")^(@)=[0.34-(-0.76)]V=1.10V`