Galvanic Cells Overview
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Questions and Answers

In the Daniell cell, which half-cell undergoes reduction?

  • Copper half-cell (correct)
  • Both half-cells simultaneously
  • Neither half-cell undergoes reduction
  • Zinc half-cell
  • What is the primary purpose of a galvanic cell?

  • To absorb electrical energy from its surroundings
  • To convert the chemical energy of a spontaneous redox reaction into electrical energy (correct)
  • To store chemical energy for later use
  • To convert the chemical energy of a non-spontaneous reaction into heat
  • What role does the salt bridge play in a galvanic cell?

  • It enhances the electrical output of the cell by increasing surface area
  • It supplies additional electrons to the oxidation half-cell
  • It connects the two half-cells electrically without allowing ion migration
  • It allows for the migration of ions between half-cells to maintain charge balance (correct)
  • Which statement accurately describes standard electrode potential?

    <p>It is the potential difference observed when all species in a half-cell have equal concentrations</p> Signup and view all the answers

    What defines the anode in a galvanic cell?

    <p>It is the half-cell that donates electrons</p> Signup and view all the answers

    Which of the following is true regarding the flow of electrons in a galvanic cell?

    <p>Electrons flow from the anode to the cathode</p> Signup and view all the answers

    What happens at the electrode-electrolyte interface in a galvanic cell?

    <p>There is a competition between metal ions depositing and metal atoms ionizing</p> Signup and view all the answers

    Which combination accurately represents the components of a galvanic cell?

    <p>Half-cells, salt bridge, and an external circuit</p> Signup and view all the answers

    What characteristic does the cathode have in a galvanic cell?

    <p>It has a positive potential with respect to the solution</p> Signup and view all the answers

    What defines the flow of current in a galvanic cell?

    <p>It flows in the opposite direction to electron flow</p> Signup and view all the answers

    Study Notes

    Overview of Galvanic Cells

    • Galvanic cells convert chemical energy from spontaneous redox reactions into electrical energy.
    • Gibbs energy from the redox reaction is transformed into electrical work for powering devices like motors or heaters.

    Daniell Cell Example

    • A primary example of a galvanic cell is the Daniell cell, which operates on the reaction:
      • Zn(s) + Cu2+(aq) -> Zn2+(aq) + Cu(s)
    • The overall cell reaction comprises two half-reactions:
      • Reduction: Cu2+ + 2e- -> Cu(s)
      • Oxidation: Zn(s) -> Zn2+ + 2e-

    Half-Cells and Electrode Functions

    • The two half-reactions occur in separate parts of the cell known as half-cells or redox couples.
    • The copper electrode is designated as the reduction half-cell, while the zinc electrode is termed the oxidation half-cell.
    • Each half-cell consists of a metallic electrode submerged in an electrolyte solution.

    Cell Connections

    • Half-cells are connected externally by a metallic wire, a voltmeter, and a switch.
    • Internally, the half-cells connect via a salt bridge, facilitating ionic movement.

    Charge Separation and Electrode Potential

    • At the electrode-electrolyte interface, ions from the solution can deposit on the electrode, causing a positive charge.
    • Conversely, metal atoms from the electrode may enter the solution as ions, leading to a negative charge at the electrode.
    • This charge separation results in an electrode potential, which is the potential difference between the electrode and the electrolyte.
    • When all species in a half-cell reach unity concentration, the electrode potential is termed standard electrode potential.

    Anode and Cathode Definitions

    • The half-cell where oxidation occurs is known as the anode, exhibiting a negative potential relative to the solution.
    • Conversely, the half-cell where reduction occurs is the cathode, having a positive potential relative to the solution.
    • A potential difference induces the flow of electrons from the anode (negative electrode) to the cathode (positive electrode).
    • The flow of current, however, moves in the opposite direction to electron flow, following conventional current direction.

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    Description

    This quiz focuses on the fundamental principles of galvanic cells, which are electrochemical devices that convert chemical energy into electrical energy. It explores how the Gibbs energy from spontaneous redox reactions can be harnessed for practical applications, such as powering electrical devices. The Daniell cell is one example discussed in detail.

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