Question

7. What voltage will be generated by a cell that consists of an iron electrode immersed in 0.5M FeSO4 solution and a copper electrode immersed in 1M CuSO4solution at 298 K. Given EoFe= -0.41V and EoCu=0.34V. Write the cell representation and cell reaction.

Answer 1

Cell representation

$Fe|Fe^{2+}(0.5M)||Cu^{2+}(1M)|Cu$

We know that

$E_{cell}=E^0_{cell}-\frac{0.0591}{n}log\frac{[Fe^{2+}]}{[Cu^{}2+]}$

$n=2$

$[Fe^{2+}]=0.5M$

$[Cu^{2+}]=1M\\E^0_{cell}=E^0_{cathode}-E^0_{anode}=0.34-(-.41)\ V=.75\ V$

Hence

$E_{cell}=$$0.75+0.008895=0.758895\ V$