Search results
Results from the WOW.Com Content Network
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 ...
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.
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]
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.
The reaction at the anode results in chlorine gas from chlorine ions: 2 Cl − → Cl 2 + 2 e −. The reaction at the cathode results in hydrogen gas and hydroxide ions: 2 H 2 O + 2 e − → H 2 + 2 OH −. Without a partition between the electrodes, the OH − ions produced at the cathode are free to diffuse throughout the electrolyte to the ...
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]
In this type of decomposition reaction, a metal chloride and oxygen gas are the products. Here, again, M represents the metal: 2 MClO 3 → 2 MCl+ 3 O 2. A common decomposition of a chlorate is in the reaction of potassium chlorate where oxygen is the product. This can be written as: 2 KClO 3 → 2 KCl + 3 O 2
The electrolysis starts with the application of an external voltage between the electrodes. This process will not occur except at extremely high voltages without an electrolyte such as sodium chloride or sulfuric acid (most used 0.1 M). [29] Bubbles from the gases will be seen near both electrodes.