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For more information, please see full course syllabus of Chemistry
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Lecture Comments (2)

0 answers

Post by Amir Bahri on August 22, 2013

Dear Professor Goldwhite

I've got a question about the standard electrode potential. I wonder if we can use the same method as explained here to measure the potental of different alloys of steel with ferent composition.


0 answers

Post by Billy Jay on April 6, 2011

Electric Charge is 1.6x10^-19 C (not 1.9X10^-19 C). Pretty significant difference on exams, so thought I'd clarify.

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Electrochemical Cells, Half-Cell Potentials

  • Some half-reactions can be made into half-cell electrodes

  • Joining half-cells gives galvanic or electrochemical cells; chemical reactions give electric current

  • Need a salt-bridge to conduct ions and balance charges

  • Zero of half-cell potentials is standard hydrogen electrode, SHE

  • Convention is half-cell potentials are for reduction half reactions

  • Table of half-cell potentials is electrochemical series; shows good oxidizing and reducing agents

  • E0 = 0.0592VlogK/n n=no. of electrons transferred

  • Nernst equation for non-standard conditions: E = E0 – 0.0592VlogQ/n; Q = reaction quotient

  • pH meter shows use of Nernst equation

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Electrochemical Cells, Half-Cell Potentials

Lecture Slides are screen-captured images of important points in the lecture. Students can download and print out these lecture slide images to do practice problems as well as take notes while watching the lecture.

  • Intro 0:00
  • Electricity from Chemical Reactions 0:29
    • Galvani Volta: Current Electricity
    • Voltaic Pile (Battery)
    • Potato Clock
  • Daniell Cell 5:56
    • Oxidation of Zinc, Reduction of Copper
    • Spontaneous Overall Reaction
    • Anode and Cathode
  • Current Electricity Fundamentals 11:34
    • Electric Charge: Coulomb
    • Electric Current: Ampere
    • Volt
    • Ohm's Law
  • Galvanic Cell 17:41
    • Salt Bridge
  • Cell Potential and Work 20:56
    • Joules
    • Coulombs
  • Hydrogen Electrode 22:53
    • Breakdown
  • Half-Cell Potentials 29:24
    • Example: Zinc and Standard Hydrogen Electrode (SHE)
  • Electrochemical Series 35:04
    • Example: Aluminum Reducing Iron Ion
  • Nernst Equation 41:46
    • Faraday
    • Example: Concentration Cell (Copper Ions)
  • Nernst Equation: pH Meter 52:24
    • Example: Potential and pH
  • Nernst Equation: Ion Concentrations 56:11
  • Additional Example 1
  • Additional Example 2