Example Galvanic cell 8.19 Nernst equation Write the scheme of the galvanic cell in which the reaction Fe(s)+Cu2+(aq)=Fe2+(aq)+Cu(s) proceeds. Calculate cell potential (electromotive force) at temperature 298.15K if the concentrations of ions are c(Cu2+)=0.04moldm3 and c(Fe2+)=0.4 mol dm3. Assume ideal behaviour of electrolyte solutions. Data: standard reduction electrode potentials at 298.15K:E(Cu2+/Cu)=+0.337V,E(Fe2+/Fe)=0.441V. Solution: 1.Write the scheme of galvanic cell 2.Nernst equation for cathodic reaction 3.Nernst equation for anodic reaction 4.Cell potential E=Ecathode,reductionEanode,reduction 4. E=Ecathode,reductionEanoder,reduction= =ECu2|Iu,reductiono2FRTlnaCu2+1[EFe2Fe,reductiono2FRTlnaFe2+1] =ECu2|Iu,reductionoEFe2FFer,reduction2FRTlnaCu2+aFe2+=2FRTln=V Example Galvanic cell 8.19 Nernst equation Write the scheme of the galvanic cell in which the reaction Fe(s)+Cu2+(aq)=Fe2+(aq)+Cu(s) proceeds. Calculate cell potential (electromotive force) at temperature 298.15K if the concentrations of ions are c(Cu2+)=0.04moldm3 and c(Fe2+)=0.4 mol dm3. Assume ideal behaviour of electrolyte solutions. Data: standard reduction electrode potentials at 298.15K:E(Cu2+/Cu)=+0.337V,E(Fe2+/Fe)=0.441V. Solution: 1.Write the scheme of galvanic cell 2.Nernst equation for cathodic reaction 3.Nernst equation for anodic reaction 4.Cell potential E=Ecathode,reductionEanode,reduction 4. E=Ecathode,reductionEanoder,reduction= =ECu2|Iu,reductiono2FRTlnaCu2+1[EFe2Fe,reductiono2FRTlnaFe2+1] =ECu2|Iu,reductionoEFe2FFer,reduction2FRTlnaCu2+aFe2+=2FRTln=V