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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

An electrochemical cell is an instrument composed of 2 half-cells connected by a conductive wire. 

Examining an Electrochemical Cell

Concept #1: Electrochemical Cells are designed to deal with redox reactions to either harness or use their potential energy.

Concept #2: The sign of the cell potential determines if an electrochemical cell produces or consumes electricity.

Example #1: EXAMPLE: Which of the following electrochemical cells would use up the largest quantity of electricity at 25ºC?

a) Electrochemical Cell A (Eºcell = -0.75 V)

b) Electrochemical Cell B (Eºcell = +1.30 V)

c) Electrochemical Cell C (Eºcell = +0.08 V)

d) Electrochemical Cell D (Eºcell = -1.42 V)