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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.
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.
) to chlorine gas, it releases electrons to the anode. Likewise, the cathode reduces sodium ions (Na +), which accepts electrons from the cathode and deposits them on the cathode as sodium metal. Sodium chloride that has been dissolved in water can also be electrolyzed. The anode oxidizes the chloride ions (Cl −), and produces chlorine (Cl 2 ...
Basic membrane cell used in the electrolysis of brine. At the anode (A), chloride (Cl −) is oxidized to chlorine. The ion-selective membrane (B) allows the counterion Na+ to freely flow across, but prevents anions such as hydroxide (OH −) and chloride from diffusing across. At the cathode (C), water is reduced to hydroxide and hydrogen gas ...
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
Proton exchange membrane (PEM) electrolysis is the electrolysis of water in a cell equipped with a solid polymer electrolyte (SPE) [3] that is responsible for the conduction of protons, separation of product gases, and electrical insulation of the electrodes. The PEM electrolyzer was introduced to overcome the issues of partial load, low ...
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 ...
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 ...