This is the problem

Question

Given the Daniel Cell:   Ag| Ag¹⁺ ||Zn²⁺ |Zn

Find: a. Standard Potential of the cell. Write in the half- cell reactions

     b. Using the Nernst equation, solve the potential of the cell . If the concentrations of the ions in solutions are:

       [Ag⁺] = 1.0x10^-3 M and [Zn²⁺] = 1.0x10^-4 M

Answer 1

Ag | Ag⁺ || Zn²⁺ | Zn THIS IS NOT A DANIELL CELL. This cell will not operate spontaneously.

Reduction @ cathode: Zn²⁺ + 2e- ==> Zn Eº = -0.76

Oxidation @ anode: Ag ==> Ag⁺ + e- Eº = 0.80 V

This is a Daniell cell:

(a) Zn | Zn²⁺ || Cu²⁺ | Cu

Reduction @ cathode: Cu²⁺ + 2e- ==> Cu(s) Eº = 0.34 V

Oxidation @ anode: Zn ==> Zn²⁺ + 2e- Eº = -0.76 V

Overall reaction: Cu²⁺ + Zn ==> Cu + Zn²⁺ Eºcell = 1.1 V (0.34 + 0.76)

(b) Nernst equation @ STP even though the temperature isn't given, we'll assume standard temperature

Ecell = Eºcell - 0.0592/n log Q

Ecell = 1.1 - (0,0296)(log 1x10-4 / 1x10-3) = 1.1 - (0.0296)(-1)

Ecell = 1.07 V