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The haloform reaction, using chlorine and sodium hydroxide, is also able to generate alkyl halides from methyl ketones, and related compounds. Chloroform was formerly produced thus. [citation needed] Chlorine adds to the multiple bonds on alkenes and alkynes as well, giving di- or tetra-chloro compounds. [citation needed]
The process has a high energy consumption, for example around 2,500 kWh (9,000 MJ) of electricity per tonne of sodium hydroxide produced. Because the process yields equivalent amounts of chlorine and sodium hydroxide (two moles of sodium hydroxide per mole of chlorine), it is necessary to find a use for these products in the same proportion ...
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.
Sodium hypochlorite solutions combined with acid evolve chlorine gas, particularly strongly at pH < 2, by the reactions: HOCl(aq) + Cl − + H + ⇌ Cl 2 (aq) + H 2 O Cl 2 (aq) ⇌ Cl 2 (g) At pH > 8, the chlorine is practically all in the form of hypochlorite anions (OCl −). The solutions are fairly stable at pH 11–12.
Non condensible gases and remaining chlorine gas are vented off as part of the pressure control of the liquefaction systems. These gases are routed to a gas scrubber, producing sodium hypochlorite, or used in the production of hydrochloric acid (by combustion with hydrogen) or ethylene dichloride (by reaction with ethylene).
Example of a reduction–oxidation reaction between sodium and chlorine, with the OIL RIG mnemonic [1] Tetracyanoquinodimethane is an organic electron-acceptor. Electron acceptors participate in electron-transfer reactions. In this context, the oxidizing agent is called an electron acceptor and the reducing agent is called an electron donor.
In the reaction, sodium metal goes from an oxidation state of 0 (a pure element) to +1: in other words, the sodium lost one electron and is said to have been oxidized. On the other hand, the chlorine gas goes from an oxidation of 0 (also a pure element) to −1: the chlorine gains one electron and is said to have been reduced.
Chloride can be oxidized but not reduced. The first oxidation, as employed in the chlor-alkali process, is conversion to chlorine gas. Chlorine can be further oxidized to other oxides and oxyanions including hypochlorite (ClO −, the active ingredient in chlorine bleach), chlorine dioxide (ClO 2), chlorate (ClO − 3), and perchlorate (ClO − 4).