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  2. Half-cell - Wikipedia

    en.wikipedia.org/wiki/Half-cell

    In electrochemistry, a half-cell is a structure that contains a conductive electrode and a surrounding conductive electrolyte separated by a naturally occurring Helmholtz double layer. Chemical reactions within this layer momentarily pump electric charges between the electrode and the electrolyte, resulting in a potential difference between the ...

  3. Copper–copper (II) sulfate electrode - Wikipedia

    en.wikipedia.org/wiki/Coppercopper(II)_sulfate...

    The copper rod protrudes out of the tube. A voltmeter negative lead is connected to the copper rod. The potential of a coppercopper sulfate electrode is +0.314 volt with respect to the standard hydrogen electrode. [citation needed] Coppercopper(II) sulfate electrode is also used as one of the half cells in the galvanic Daniel-Jakobi cell.

  4. Galvanic cell - Wikipedia

    en.wikipedia.org/wiki/Galvanic_cell

    A galvanic cell consists of two half-cells, such that the electrode of one half-cell is composed of metal A, and the electrode of the other half-cell is composed of metal B; the redox reactions for the two separate half-cells are thus: A n + + n e − ⇌ A B m + + m e − ⇌ B. The overall balanced reaction is:

  5. Electrochemical cell - Wikipedia

    en.wikipedia.org/wiki/Electrochemical_cell

    Galvanic cells consists of two half-cells. Each half-cell consists of an electrode and an electrolyte (both half-cells may use the same or different electrolytes). [citation needed] The chemical reactions in the cell involve the electrolyte, electrodes, and/or an external substance (fuel cells may use hydrogen gas as a reactant).

  6. Reference electrode - Wikipedia

    en.wikipedia.org/wiki/Reference_electrode

    To focus on the reaction at the working electrode, the reference electrode is standardized with constant (buffered or saturated) concentrations of each participant of the redox reaction. [1] There are many ways reference electrodes are used. The simplest is when the reference electrode is used as a half-cell to build an electrochemical cell.

  7. Cell notation - Wikipedia

    en.wikipedia.org/wiki/Cell_notation

    In electrochemistry, cell notation or cell representation is a shorthand method of expressing a reaction in an electrochemical cell.. In cell notation, the two half-cells are described by writing the formula of each individual chemical species involved in the redox reaction across the cell, with all other common ions and inert substances being ignored.

  8. Standard electrode potential - Wikipedia

    en.wikipedia.org/wiki/Standard_electrode_potential

    Bipolar electrochemistry scheme. In electrochemistry, standard electrode potential, or , is a measure of the reducing power of any element or compound.The IUPAC "Gold Book" defines it as; "the value of the standard emf (electromotive force) of a cell in which molecular hydrogen under standard pressure is oxidized to solvated protons at the left-hand electrode".

  9. Auxiliary electrode - Wikipedia

    en.wikipedia.org/wiki/Auxiliary_electrode

    The auxiliary electrode often has a surface area much larger than that of the working electrode to ensure that the half-reaction occurring at the auxiliary electrode can occur fast enough so as not to limit the process at the working electrode. When a three-electrode cell is used to perform electroanalytical chemistry, the auxiliary electrode ...