Electrochemistry Notes

Introduction

• Name: Topper Omar, Chemistry Educator
• Subject: Electrochemistry (Weightage of 9 Marks)
• Objective: Solving important questions and clarifying concepts.

Meaning of Electrochemistry

• Electro: Electricity
• Chemistry: Chemical bonds and reactions.
• Electrochemistry: Relationship between electrical and chemical energy.

Types of Electrochemical Cells

1. Galvanic Cell

   • Converts chemical energy into electrical energy.
   • Spontaneous redox reactions.
   • Anode: Negative, Cathode: Positive.

2. Electrolytic Cell

   • Non-spontaneous redox reactions.
   • Converts electrical energy into chemical energy.

Cell Notation (Cell Representation)

• Daniel Cell: Cell of zinc and copper.
  • Use of zinc sulfate and copper sulfate.
  • Flow of electrons and charge balance (neutralism ions).
  • Cell Notation: a | b || c | d
    • (a: Anode, b: Salt bridge, c: Cathode)

Electrode Potential

• Electrode Potential: Potential difference between electrode and electrolyte.
• Relationship between reduction potential and oxidation potential.
• Nernst Equation:
  • e = e° - (2.303RT/nF) log([Product]/[Reactant])

Gibbs Free Energy

• Definition of Gibbs Free Energy (ΔG).
  • ΔG = -nFE
  • Measures spontaneity.

Faraday's Laws for Electrolysis

1. Faraday's First Law:
   • m ∝ q (Directly proportional to charge).
2. Faraday's Second Law:
   • Ratio of substances liberated at two electrodes equals the ratio of their electrochemical equivalents.

Types of Batteries

1. Primary Cell: For one-time use only.
2. Secondary Cell: Can be recharged repeatedly.
3. Fuel Cell: Produces electrical energy directly from the combustion of fuel.

Homework

• Take screenshots and answer questions.

Conclusion

• Clear understanding of concepts.
• Important information for further preparation.

Note: Keep in mind all important equations and concepts for better performance in exams.