Assignment 1: Electrochemistry
1. Given that the E0 Ag+/Ag= 0.804 V and E0Cu2+/Cu= 0.34 V Predict whether silver solution
can be stored in a copper vessel or not. Justify your answer.
2. For the following half-cell reactions, E0 values are
Mn2+ +2H2O (l) →MnO2(s) +4H+(aq)+2e; E0= -1.23V
MnO4-(aq)+4H+(aq) +3e→ MnO2(s)+2H2O(l) ; E0=+1.70V
Calculate the E0 Cell value and predict the spontaneity of the reaction.
3. Given that the E0(Cu2+/Cu)=+0.34V, E0(Zn2+/Zn) = -0.76V. Whether the copper sulphate
solution can be stored in a vessel made up of Zinc. Justify your answer.
4. What is the free energy change and equilibrium constant for the following reaction at
250C.
2Ag+ (aq)+Fe(s) →2Ag(s) +Fe2+(aq)
5. Represent the cell in which the following reactions take place
Mg(s)+2Ag+(0.001M) →Mg2+(0.130M)+2Ag(s)
Calculate the Ecell value if E0cell =3.17 V