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The chloralkali process (also chlor-alkali and chlor alkali) is an industrial process for the electrolysis of sodium chloride (NaCl) solutions. It is the technology used to produce chlorine and sodium hydroxide (caustic soda), [ 1 ] which are commodity chemicals required by industry.
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.
The first type, shown on the right and left of the diagram, uses an electrolyte of sodium chloride solution, a graphite anode (A), and a mercury cathode (M). The other type of cell, shown in the center of the diagram, uses an electrolyte of sodium hydroxide solution, a mercury anode (M), and an iron cathode (D). The mercury electrode is common ...
Electrolysis of water produces hydrogen and oxygen in a ratio of 2 to 1 respectively. 2 H 2 O(l) → 2 H 2 (g) + O 2 (g) E° = +1.229 V. The energy efficiency of water electrolysis varies widely. The efficiency of an electrolyser is a measure of the enthalpy contained in the hydrogen (to undergo combustion with oxygen or some other later ...
Chlorine can be manufactured by the electrolysis of a sodium chloride solution , which is known as the Chloralkali process. The production of chlorine results in the co-products caustic soda (sodium hydroxide, NaOH) and hydrogen gas (H 2). These two products, as well as chlorine itself, are highly reactive.
In molten sodium chloride (NaCl), when a current is passed through the salt the anode oxidizes chloride ions (Cl −) 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.
Pure water has a charge carrier density similar to semiconductors [12] [page needed] since it has a low autoionization, K w = 1.0×10 −14 at room temperature and thus pure water conducts current poorly, 0.055 μS/cm. [13] Unless a large potential is applied to increase the autoionization of water, electrolysis of pure water proceeds slowly ...
Molten salts can also be electrolytes as, for example, when sodium chloride is molten, the liquid conducts electricity. In particular, ionic liquids, which are molten salts with melting points below 100 °C, [15] are a type of highly conductive non-aqueous electrolytes and thus have found more and more applications in fuel cells and batteries. [16]