Cell Notation

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

                                          Fe (s) | Fe²⁺ (aq) || H⁺ (aq) | H₂ (g) | Pt (s)

• A. Fe (s) + 2 H+ (aq) → Fe2+ (aq) + H22 (g)
• B. Fe2+ (aq) + H22 (g) → Fe (s) + 2 H+ (aq)
• C. Fe2+ (aq) → Fe (s)
• D. H22 (g) → H22 (g)

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

• A. 0.3130 V
• B. 0.4033 V
• C. 0.5085 V
• D. 0.1199 V

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

• A. 0.87 M
• B. 1.20 M
• C. 3.32 M
• D. 0.11 M