InterviewSolution
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InterviewSolution
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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. |
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Answer» 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` |
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