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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
Redox Reaction
Balancing Redox Reaction
The Nernst Equation
Faraday's Constant
Galvanic Cell
Batteries and Electricity
Additional Guides
Nernst Equation (IGNORE)

Batteries act as spontaneous electrochemical cells that help to generate electricity. 

Dry-Cell Batteries

These types of batteries get their names from the fact that they contain very little water. 

Concept #1: Dry-Cell Batteries & Alkaline Battery

The overall reaction within a typical dry-cell battery is  

Zn (s) + 2 MnO2 (s) + 2 NH4+ (aq) → Zn2+ (aq) + Mn2O3 (s) + 2 NH3 (g) + H2O (l)

These types of batteries get their names from the fact that they operate within a basic medium.

The overall reaction within a typical alkaline battery is  

Zn (s) + 2 MnO2 (s) + 2 H2O (l) → Zn(OH)2 (s) + 2 MnO(OH) (s)