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  2. Half-cell - Wikipedia

    en.wikipedia.org/wiki/Half-cell

    A standard half-cell consists of a metal electrode in an aqueous solution where the concentration of the metal ions is 1 molar (1 mol/L) at 298 kelvins (25 °C). [1] In the case of the standard hydrogen electrode (SHE), a platinum electrode is used and is immersed in an acidic solution where the concentration of hydrogen ions is 1M, with ...

  3. 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:

  4. 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.

  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). 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

    A reference electrode is an electrode that has a stable and well-known electrode potential. The overall chemical reaction taking place in a cell is made up of two independent half-reactions , which describe chemical changes at the two electrodes.

  7. Electrochemistry - Wikipedia

    en.wikipedia.org/wiki/Electrochemistry

    A galvanic cell whose electrodes are zinc and copper submerged in zinc sulfate and copper sulfate, respectively, is known as a Daniell cell. [24] The half reactions in a Daniell cell are as follows: [24] Zinc electrode (anode): Zn(s) → Zn 2+ (aq) + 2 e − Copper electrode (cathode): Cu 2+ (aq) + 2 e − → Cu(s) A modern cell stand for ...

  8. Half-reaction - Wikipedia

    en.wikipedia.org/wiki/Half-reaction

    In chemistry, a half reaction (or half-cell reaction) is either the oxidation or reduction reaction component of a redox reaction. A half reaction is obtained by considering the change in oxidation states of individual substances involved in the redox reaction.

  9. Electrode - Wikipedia

    en.wikipedia.org/wiki/Electrode

    An electrode is an electrical conductor used to make contact with a nonmetallic part of a circuit (e.g. a semiconductor, an electrolyte, a vacuum or air). Electrodes are essential parts of batteries that can consist of a variety of materials (chemicals) depending on the type of battery.