If `E^(c-)._((Ag|Ag^(o+)))=-0.8V` and `E^(c-)._((H_(2)|2H^(o+)))=0 V` , in a cell arrangement using these two electrodes, find `E^(c-)._(cell)` and find out which electrode acts as anode and which acts as cathode.

Explanation

Note that `E^(c-)._((Ag|Ag^(o+)))` and `E^(c-)._(H_(2)|2H^(o+))` are stanard oxidation potential values. Comparing the two values,
`E^(c-)._((H_(2)|2H^(o+)))gtE^(c-)._((Ag|Ag^(o+)))` or
Comparing the reduction potential values,
`E^(c-)._((Ag^(o+)|Ag))gtE^(c-)._((2H^(o+)|H_(2)))`
Hence, silver electrode will act as catohde and hydrogen electrode will act as anode.
The cell representation of the cell is `:`
`Pt,H_(2)(1 atm)|H^(o+)(1.0M)||Ag^(o+)(1.0M)|Ag(s)`
`E^(c-)._(cell)=(E^(c)._(reduction))_(cathode)-(E^(c-)._(reduction))_(anode)`
`=0.8-0=0.8V`