Electrochemical Cells Quiz
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Questions and Answers

Which type of cell uses a spontaneous redox reaction to generate electrical energy?

  • Concentration cell
  • Galvanic cell (correct)
  • Electrolytic cell
  • Fuel cell
  • What is the equation used to calculate the electromotive force (emf) of a galvanic cell?

  • Gibbs-Helmholtz equation
  • Hess's law
  • Nernst equation (correct)
  • Faraday's law
  • What is the standard potential of a cell?

  • The potential difference of the cell at maximum power
  • The potential difference of the cell at equilibrium
  • The potential difference of the cell under standard conditions (correct)
  • The potential difference of the cell at infinite dilution
  • What is the molar conductivity (✆m) of an ionic solution?

    <p>The conductivity of the solution divided by the molar concentration of the electrolyte</p> Signup and view all the answers

    What does Kohlrausch's law state?

    <p>The molar conductivity of an electrolytic solution is constant at all concentrations</p> Signup and view all the answers

    Study Notes

    Galvanic Cells

    • A galvanic cell, also known as a voltaic cell, uses a spontaneous redox reaction to generate electrical energy.
    • The cell consists of two half-cells, each containing an electrode and an electrolyte, connected by an electrically conducting wire and a salt bridge.

    Electromotive Force (EMF)

    • The electromotive force (EMF) of a galvanic cell is calculated using the Nernst equation: Ecell = E°cell - (RT/nF) ln(Q).
    • EMF is the maximum potential difference developed between the two electrodes of a galvanic cell.

    Standard Potential

    • The standard potential of a cell is the potential difference developed under standard conditions, i.e., at 25°C, 1 atm, and 1 M concentration of reactants.

    Molar Conductivity

    • Molar conductivity (Λm) is the conductivity of an ionic solution per unit concentration of the electrolyte.
    • It is calculated as the conductivity of the solution (κ) divided by the concentration of the electrolyte (c): Λm = κ / c.

    Kohlrausch's Law

    • Kohlrausch's law states that the molar conductivity of an ionic solution at infinite dilution (Λm°) is the sum of the molar conductivity of the individual ions.
    • The law allows for the calculation of the molar conductivity of an ionic solution at infinite dilution from the conductivity of the individual ions.

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    Description

    Test your knowledge on electrochemical cells, Nernst equation, standard potential, and Gibbs energy with this quiz. Gain a deeper understanding of how to differentiate between galvanic and electrolytic cells and calculate the emf of a galvanic cell using the Nernst equation. Explore the relationship between standard potential, Gibbs energy, and equilibrium constant. Challenge yourself on concepts related to resistance in electrochemical cells.

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