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# Cell Notation

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Sections
Standard Reduction Potentials
Intro to Electrochemical Cells
Galvanic Cell
Electrolytic Cell
Cell Potential: Standard
Cell Potential: The Nernst Equation
Cell Potential and Gibbs Free Energy
Cell Potential and Equilibrium
Cell Potential: G and K
Cell Notation
Electroplating

Cell or Line Notation is a quick, simple method to describe an electrochemical cell without having to draw it out in detail.

###### Cell Notation Setup

Concept #1: A Cell Notation is comprised of phase and physical boundaries.

Example #1: Consider an electrochemical cell where the following reaction takes place:

3 Sn2+ (aq) + 2 Al (s)  →  3 Sn (s) + 2 Al3+ (aq)

What is the cell notation for this cell?

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

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

Practice: 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

Practice: 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