Construct a cell using given electrodes at `298K` and also calculate its standart `EMF`.
Given ` :` `E^(c-)._(Zn|Zn^(2+))=0.76V`
`E^(c-)._(Cu^(2+)|Cu)=0.34V`

Explanation

Note that `E^(c-)._(Zn|Zn^(2+))` is the standard oxidation potential valuse while that of `E^(c-)._(Cu^(2+)|Cu)` is standard reduction potential value.
Therfore, `E^(c-).-(Zn^(2+)|Zn)(` standard reductio potential `)` value is `-0.76v`. Comparing the two standard reduction potential values.
`:. E^(c-)._((Cu^(2+)|Cu))gtE^(c-)._((Zn^(2+)|Zn))`
Hence, copper electrode will act as cathode and Zinc electrode will act as anode. The cell representation of the cell is `:`
`Zn(s)|Zn^(2+)(1.0M)||Cu^(2+)(1.0M)|Cu(s)`
`E^(c-)._(cell)=(E^(c-)._(reduction))_(cathode)-(E^(c-)._(reduction ))_(anode)`
`=0.34-(-0.76)=1.1V`