20. Electrochemistry

For the following electrochemical cell

Cu(s) | Cu₂(aq, 0.0155 m) || Ag(aq, 2.50 m) | Ag(s)

What is the balanced reaction for the cell diagram below? Al(s) | Al³⁺(aq) || Cd²⁺(aq) | Cd(s)

Write the half reactions as well as the overall net ionic equation for the following line notation: 

                     Fe (s) | Fe²⁺ (aq) || Mg²⁺ (aq) | Mg (s)

What is the [Cu²⁺] for the following cell notation diagram if the cell potential is 0.4404 V?

Cu | Cu²⁺ (aq, ? M) || Ag⁺(aq, 0.50 M) | Ag

Standard Reduction Potentials

Cu²⁺ (aq) + 2 e^–  →. Cu (s)               E°_red = + 0.3394

Ag⁺ (aq) + e^–­  →  Ag (s)                    E°_red= + 0.8000

The cell notation for a redox reaction is given as the following at (T= 298 K). Calculate the cell potential for the reaction at 25ºC.

Zn (s) | Zn²⁺ (aq, 0.37 M) || Ni²⁺ (aq, 0.059 M) | Ni (s)

Standard Reduction Potentials

Zn²⁺ (aq) + 2 e^–  →. Zn (s)            E°_red = - 0.7621

Ni²⁺ (aq) + 2 e^–­  →  Ni (s)             E°_red = - 0.2300