Electrochemical Cells and Standard Potentials
5 Questions
2 Views

Choose a study mode

Play Quiz
Study Flashcards
Spaced Repetition
Chat to lesson

Podcast

Play an AI-generated podcast conversation about this lesson

Questions and Answers

What does a positive standard electrode potential indicate about a species?

  • Hydrogen gas is a stronger oxidizing agent than the species.
  • The species cannot participate in redox reactions.
  • The reduced form is more stable than hydrogen gas. (correct)
  • The species can only act as a reducing agent.
  • How does lithium behave in terms of its standard electrode potential?

  • Lithium ion is a weak oxidizing agent. (correct)
  • Lithium ion acts as a strong oxidizing agent.
  • Lithium metal shows strong oxidizing properties in aqueous solution.
  • Lithium metal is a weak reducing agent.
  • What trend is observed in standard electrode potentials as one moves down the electrode potential table?

  • The oxidizing power of species decreases. (correct)
  • The reducing power of species decreases.
  • The potentials become less negative.
  • The oxidizing power of species increases.
  • Which statement accurately describes fluorine's standard electrode potential?

    <p>Fluorine gas is a strong oxidizing agent.</p> Signup and view all the answers

    What application utilizes standard electrode potentials for practical measurements?

    <p>Measurement of pH in solutions.</p> Signup and view all the answers

    Study Notes

    Standard Electrode Potentials

    • Standard electrode potentials provide valuable information about half-cell reduction reactions.
    • A positive potential indicates a more stable reduced form compared to hydrogen gas.
    • A negative potential indicates a more stable hydrogen gas form compared to reduced form.
    • Fluorine gas (F₂) has the highest potential, making it a strong oxidizing agent.
    • Fluoride ions (F⁻) are weak reducing agents.
    • Lithium has the lowest potential, meaning lithium ions are weak oxidizing agents and lithium metal is a strong reducing agent.
    • As you go down the table (from top to bottom), the standard electrode potential decreases.
    • This results in a decrease in oxidizing power of species on the left and an increase in reducing power on the right.

    Electrochemical Applications

    • Electrochemical cells are used to measure pH, solubility product, equilibrium constant, and other thermodynamic properties.
    • Potentiometric titrations are also based on electrochemical principles.

    Studying That Suits You

    Use AI to generate personalized quizzes and flashcards to suit your learning preferences.

    Quiz Team

    Description

    This quiz covers the concepts of standard electrode potentials and their significance in half-cell reduction reactions. It explores the relative stability of reduced and oxidized forms of various elements and the applications of electrochemical cells in measuring thermodynamic properties. Test your knowledge on these critical principles in electrochemistry!

    More Like This

    Use Quizgecko on...
    Browser
    Browser