General Chemistry – Electrochemistry and the Galvanic Cell
Learn the fundamentals of electrochemistry, redox reactions, and galvanic cells in this comprehensive chemistry course. Understand concepts, balance reactions, calculate cell potential, and apply the Nernst equation. Suitable for high school and college chemistry students.
What you’ll learn
- Understand All the Concepts of Electrochemistry in a First Year Chemistry Course
- Balance Oxidation-Reduction Reactions (Redox Reactions) in Acidic or Basic Solution
- Write and Balance Redox Half-Reactions
- Set Up a Galvanic Cell, Assign the Anode and Cathode, Identify the Oxidizing Agent and Reducing Agent, and Calculate the Electricity Generated
- Calculate the Cell Potential (Ecell), or Electromotive Force (emf) Using Standard Reduction Potentials
- Write the Line Notation to Describe a Galvanic Cell, or Electrochemical Cell
- Use and Apply the Nernst Equation, the Faraday Constant, and the Relationship Between Free Energy and Cell Potential
- Detailed Understanding of Concentration Cells, Batteries, and Electrolytic Cells
GENERAL CHEMISTRY – Electrochemistry, Galvanic Cells, and Overall Cell Potential. Redox, Line Notation, Nernst Equation, and Electrolysis.
LECTURE #1 – Electrochemistry and the Galvanic Cell
17-1 — Oxidation-Reduction Reactions (Redox Reactions)
– A Typical Redox Reaction
– The Oxidizing Agent and the Reducing Agent
– Redox Half-Reactions
17-2 — Redox Reactions and Electricity Generation
– Separating the Oxidizing Agent and the Reducing Agent
– Electrochemical Cells
17-2 — Galvanic Cells
– Galvanic Cell Setup
– The Anode and the Cathode (“OIL RIG”)
– The Salt Bridge
– Measuring Voltage with a Voltmeter
Runtime: 18:00
===== ===== ===== =====
LECTURE #2 – Cell Potential (Ecell), Standard Reduction Potentials, and Line Notation
17-4 — Cell Potential (Ecell)
– The Electromotive Force (emf)
– Calculating the Cell Potential
– Standard Reduction Potentials (E’cell)
17-5 — Table of Standard Reduction Potentials
17-7 — Line Notation to Describe an Electrochemical Cell
Runtime: 11:36
===== ===== ===== =====
LECTURE #3 – Galvanic Cell Practice Problems
17-10 — Inert Electrodes
– Platinum as an Inert Electrode
17-10 — Galvanic Cell Practice Problems
– Three Practice Problems
– “Completely Describe” the Following Galvanic Cells
Runtime: 15:38
===== ===== ===== =====
LECTURE #4 – The Relationship Between Free Energy and Cell Potential
17-11 — The Relationship Between Free Energy and Cell Potential
– The Faraday Constant (F)
– Spontaneous vs. Non-Spontaneous Redox Reactions
Runtime: 12:25
===== ===== ===== =====
LECTURE #5 – Concentration Cells, and the Nernst Equation
17-13 — Concentration Cells
– Direction of Electron Flow
– Designation of Anode and Cathode
17-15 — The Nernst Equation
– Non-Standard Cell Potentials
Runtime: 14:00
===== ===== ===== =====
LECTURE #6 – Galvanic Cells and the Equilibrium Constant, K
17-17 — Calculating the Equilibrium Constant (K) for a Redox Reaction
Runtime: 10:05
===== ===== ===== =====
LECTURE #7 – Batteries: the Lead Storage Battery and the Dry Cell Battery
17-18 — Batteries
– Sources of Direct Current
– The Lead Storage Battery
– The Dry Cell Battery
Runtime: 9:39
===== ===== ===== =====
LECTURE #8 – Electrolysis and the Electrolytic Cell
17-21 — Electrolysis
– Electrolytic Cells
– Reversal of Electron Flow
– Electrolytic Cells vs. Galvanic Cells
Runtime: 10:39
Who this course is for:
- 1st Year Chemistry Students Taking High School Chemistry
- 1st Year Chemistry Students Taking High School AP Chemistry
- 1st Year Chemistry Students Taking College Chemistry
- 1st Year General Chemistry Students
- 1st Year Inorganic Chemistry Students
User Reviews
Be the first to review “General Chemistry – Electrochemistry and the Galvanic Cell”
You must be logged in to post a review.
There are no reviews yet.