galvanic cell

(noun)

Electrochemical cell that derives electrical energy from spontaneous redox reaction taking place within the cell.

Related Terms

  • oxidizing agent
  • electrode potential
  • Gibbs free energy

Examples of galvanic cell in the following topics:

  • Free Energy and Cell Potential

    • In a galvanic cell, where a spontaneous redox reaction drives the cell to produce an electric potential, the change in Gibbs free energy must be negative.
    • The basis for an electrochemical cell, such as the galvanic cell, is always a redox reaction that can be broken down into two half-reactions: oxidation occurs at the anode, where there is a loss of electrons, and reduction occurs at the cathode, where there is a gain of electrons.
    • In a galvanic cell, where a spontaneous redox reaction drives the cell to produce an electric potential, the change in Gibbs free energy must be negative.
    • If E°cell > 0, then the process is spontaneous (galvanic cell)
    • A demonstration electrochemical cell setup resembling the Daniell cell.
  • Electrochemical Cell Notation

    • Cell notation is shorthand that expresses a certain reaction in an electrochemical cell.
    • Cell notations are a shorthand description of voltaic or galvanic (spontaneous) cells.
    • The anode half-cell is described first; the cathode half-cell follows.
    • Using these rules, the notation for the cell we put together is:
    • A typical arrangement of half-cells linked to form a galvanic cell.
  • Standard Reduction Potentials

    • In this galvanic cell, zinc reduces copper cations.
  • Equilibrium Constant and Cell Potential

    • It can also be used to determine the total voltage, or electromotive force, for a full electrochemical cell.
    • The standard cell potential for the reaction is then +0.34 V - (-0.76 V) = +1.10 V.
    • The cell equilibrium constant, K, can be derived from the Nernst equation:
    • Schematic of a galvanic cell for the reaction between Zn and Cu.
    • Calculate the equilibrium constant, K, for a galvanic cell using the Nernst equation
  • The Nernst Equation

    • In electrochemistry, the Nernst equation can be used to determine the reduction potential of an electrochemical cell.
    • In electrochemistry, the Nernst equation can be used, in conjunction with other information, to determine the reduction potential of a half-cell in an electrochemical cell.
    • Find the cell potential of a galvanic cell based on the following reduction half-reactions where [Ni2+] = 0.030 M and [Pb2+] = 0.300 M.
    • First, find the electromotive force for the standard cell, which assumes concentrations of 1 M.
    • The added half-reactions with the adjusted E0 cell are:
  • Electrolytic Cells

    • Electrolysis uses electrical energy to induce a chemical reaction, which then takes place in an electrolytic cell.
    • Electrolysis can sometimes be thought of as running a non-spontaneous galvanic cell.
    • A cell used in elementary chemical experiments to produce gas as a reaction product and to measure its volume.
  • Concentration of Cells

    • The standard potential of an electrochemical cell requires standard conditions for all of the reactants.
    • When reactant concentrations differ from standard conditions, the cell potential will deviate from the standard potential.
    • The change in Gibbs free energy for an electrochemical cell can be related to the cell potential.
    • Under standard conditions, the output of this pair of half-cells is well known.
    • Discuss the implications of the Nernst equation on the electrochemical potential of a cell
  • Voltaic Cells

    • A voltaic cell is a device that produces an electric current from energy released by a spontaneous redox reaction in two half-cells.
    • This kind of cell includes the galvanic, or voltaic, cell, named after Luigi Galvani and Alessandro Volta.
    • In a typical voltaic cell, the redox pair is copper and zinc, represented in the following half-cell reactions:
    • Each half-cell is connected by a salt bridge, which allows for the free transport of ionic species between the two cells.
    • The cell consists of two half-cells connected via a salt bridge or permeable membrane.
  • Predicting the Products of Electrolysis

    • Electrolysis is very important commercially as a stage in the separation of elements from naturally occurring sources, such as ores, using an electrolytic cell.
    • You may have noticed that this is the opposite of a galvanic cell, where the anode is negative and the cathode is positive.
  • Different Types of Currents

    • Direct current is produced by sources such as batteries, thermocouples, solar cells, and commutator-type electric machines of the dynamo type.
    • A term formerly used for direct current was galvanic current.
Subjects
  • Accounting
  • Algebra
  • Art History
  • Biology
  • Business
  • Calculus
  • Chemistry
  • Communications
  • Economics
  • Finance
  • Management
  • Marketing
  • Microbiology
  • Physics
  • Physiology
  • Political Science
  • Psychology
  • Sociology
  • Statistics
  • U.S. History
  • World History
  • Writing

Except where noted, content and user contributions on this site are licensed under CC BY-SA 4.0 with attribution required.