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Copper at red heat (300-400°C) combines directly with chlorine gas, giving (molten) copper(II) chloride. The reaction is very exothermic. [8] [15] Cu(s) + Cl 2 (g) → CuCl 2 (l) A solution of copper(II) chloride is commercially produced by adding chlorine gas to a circulating mixture of hydrochloric acid and copper. From this solution, the ...
Simplified diagram of the Copper–Chlorine cycle. The copper–chlorine cycle (Cu–Cl cycle) is a four-step thermochemical cycle for the production of hydrogen. The Cu–Cl cycle is a hybrid process that employs both thermochemical and electrolysis steps. It has a maximum temperature requirement of about 530 degrees Celsius. [1]
The reaction takes place at about 400 to 450 °C in the presence of a variety of catalysts, including copper chloride (CuCl 2). Three companies developed commercial processes for producing chlorine based on the Deacon reaction: [1] The Kel-Chlor process developed by the M. W. Kellogg Company, which utilizes nitrosylsulfuric acid.
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.
Electrolysis is usually done in bulk using hundreds of sheets of metal connected to an electric power source. In the production of copper, these pure sheets of copper are used as starter material for the cathodes, and are then lowered into a solution such as copper sulfate with the large anodes that are cast from impure (97% pure) copper.
A low voltage DC current is applied, electrolysis happens producing sodium hypochlorite and hydrogen gas (H 2). The solution travels to a tank that separates the hydrogen gas based on its low density. [1] Only water and sodium chloride are used. The simplified chemical reaction is: NaCl + H 2 O + energy → NaOCl + H 2 [citation needed]
The most common chloralkali process involves the electrolysis of aqueous sodium chloride (a brine) in a membrane cell. A membrane, such as Nafion, Flemion or Aciplex, is used to prevent the reaction between the chlorine and hydroxide ions. Basic membrane cell used in the electrolysis of brine. At the anode (A), chloride (Cl −) is
Important examples of electrolysis are the decomposition of water into hydrogen and oxygen, and bauxite into aluminum and other chemicals. Electroplating (e.g., of copper, silver, nickel, or chromium) is done using an electrolytic cell. Electrolysis is a technique that uses a direct electric current (DC).