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Ch.18 - ElectrochemistryWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch.17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds
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

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