The E values at 298 corresponding to the following two reduction electrode processes are i) Cu+/Cu = +0.52V ii) Cu2+/Cu = 0.16 V Formulate the galvanic cell for their combination. what will be the cell potential? Calculate the del r G for the cell reaction.(E=96500 C/mol) Share with your friends Share 12 Vartika Jain answered this Dear Student, Since anode electrode has less value of E°(reduction), so the galvanic cell obtained by the combination of anode and cathode will be :Cu+/Cu2+ ∥ Cu+/Cu(s)Since E°(reduction) value, +0.52>+0.16 V, so we haveCu+ + e- ↔ Cu E°=+0.52 V (cathode)Cu2+ + e- ↔ Cu+ E°= +0.16 V (anode) Substracting the above two, 2Cu+ ↔ Cu + Cu2+ E°=0.52-0.16=0.36 VSince the reaction os a one electron change, n=1∆G°=-nFE° =-1×96500×0.36 =-34540 J =-34.74 kJ 27 View Full Answer Prashant answered this zimnd 9