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  2. Electrolysis - Wikipedia

    en.wikipedia.org/wiki/Electrolysis

    Direct electrolysis of seawater follows known processes, forming an electrolysis cell in which the seawater acts as the electrolyte to allow for the reaction at the anode, 2 Cl − (aq) → Cl 2 (g) + 2e − and the reaction at the cathode, 2 H 2 O(l) + 2 e − → H 2 (g) + 2OH − (aq).

  3. Castner–Kellner process - Wikipedia

    en.wikipedia.org/wiki/Castner–Kellner_process

    The reaction at anode (A) is: 2 Cl − → Cl 2 + 2 e −. The chlorine gas that results vents at the top of the outside cells where it is collected as a byproduct of the process. The reaction at the mercury cathode in the outer cells is Na + + e − → Na (amalgam) The sodium metal formed by this reaction dissolves in the mercury to form an ...

  4. Electrolysis of water - Wikipedia

    en.wikipedia.org/wiki/Electrolysis_of_water

    Electrolysis in pure water consumes/reduces H + cations at the cathode and consumes/oxidizes hydroxide (OH −) anions at the anode. This can be verified by adding a pH indicator to the water: Water near the cathode is basic while water near the anode is acidic.

  5. Solid oxide electrolyzer cell - Wikipedia

    en.wikipedia.org/wiki/Solid_oxide_electrolyzer_cell

    The net cell reaction yields hydrogen and oxygen gases. The reactions for one mole of water are shown below, with oxidation of oxide ions occurring at the anode and reduction of water occurring at the cathode. Anode: 2 O 2− → O 2 + 4 e −. Cathode: H 2 O + 2 e − → H 2 + O 2−. Net Reaction: 2 H 2 O → 2 H 2 + O 2

  6. Electro-oxidation - Wikipedia

    en.wikipedia.org/wiki/Electro-oxidation

    Simple scheme of the apparatus for electro-oxidation process. The set-up for performing an electro-oxidation treatment consists of an electrochemical cell.An external electric potential difference (aka voltage) is applied to the electrodes, resulting in the formation of reactive species, namely hydroxyl radicals, in the proximity of the electrode surface. [11]

  7. Auxiliary electrode - Wikipedia

    en.wikipedia.org/wiki/Auxiliary_electrode

    The auxiliary electrode functions as a cathode whenever the working electrode is operating as an anode and vice versa. 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 ...

  8. Electrolytic cell - Wikipedia

    en.wikipedia.org/wiki/Electrolytic_cell

    Electrolytic cells are often used to decompose chemical compounds, in a process called electrolysis—with electro meaning electricity [5] and the Greek word lysis means to break up. Important examples of electrolysis are the decomposition of water into hydrogen and oxygen , and bauxite into aluminum and other chemicals.

  9. Downs cell - Wikipedia

    en.wikipedia.org/wiki/Downs_cell

    The Downs cell uses a carbon anode and an iron cathode.The electrolyte is sodium chloride that has been heated to the liquid state. Although solid sodium chloride is a poor conductor of electricity, when molten the sodium and chloride ions are mobilized, which become charge carriers and allow conduction of electric current.