Electrochemistry

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About Course

This comprehensive course is designed to demystify the relationship between chemical energy and electrical energy. Students will master the principles of redox reactions, explore the mechanics of electrolytic and electrochemical cells, and learn to perform precise calculations involving Faraday’s Laws. Tailored specifically for the Nigerian curriculum (WAEC/NECO) and JAMB (UTME) standards, this course provides the conceptual clarity and problem-solving skills necessary to excel in O-Level and entry-level university chemistry.

Course Content

Module 1: Foundations of Redox Reactions
Oxidation and Reduction: Understanding redox in terms of oxygen transfer, hydrogen transfer, and electron transfer. Oxidation Numbers: Rules for assigning oxidation states and identifying oxidizing/reducing agents. Balancing Redox Equations: Half-reaction method and oxidation number method.

Module 2: Electrolysis (The Electrolytic Cell)
Components of Electrolysis: Electrolytes (strong vs. weak), electrodes (inert vs. active), and the electrolytic tank. Preferential Discharge of Ions: Factors affecting the discharge of ions (position in electrochemical series, concentration, and nature of electrodes). Practical Examples: Electrolysis of acidified water, brine, and copper(II) sulfate solution.

Module 3: Quantitative Electrochemistry (Faraday’s Laws)
Module 3: Quantitative Electrochemistry (Faraday’s Laws)Faraday’s First Law: Relationship between mass ($m$), current ($I$), and time ($t$). Formula: $m = zIt$.Faraday’s Second Law: Chemical equivalents and the Faraday constant ($96,500 text{ C mol}^{-1}$).Calculations: Determining mass deposited, volume of gases at STP, and the charge on ions.

Module 4: Electrochemical Cells (Galvanic/Voltaic)
Cell Construction: Half-cells, salt bridges, and external circuits. Standard Electrode Potential (E ∘ ): The Standard Hydrogen Electrode (SHE) and the Electrochemical Series. Cell Notation: Writing and interpreting cell diagrams (e.g., Zn (s)∣Zn(aq)2+ ∣∣Cu (aq)2+ ∣Cu (s)). Electromotive Force (e.m.f.): Calculating E cell ∘ ​ =E cathode ∘ ​ −E anode

Module 5: Industrial Applications & Corrosion
Electroplating and Purification: How electrolysis is used to coat metals and refine copper. Primary and Secondary Cells: Lead-acid accumulators, dry cells (Leclanché), and fuel cells. Corrosion of Metals: The chemistry of rusting and methods of prevention (cathodic protection, galvanizing).

Module 6: Exam Prep (WAEC/NECO/UTME Focus)

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