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As can be seen in the following reaction, 1,2-dichloroethane is cracked: ClCH 2 CH 2 Cl → CH 2 =CHCl + HCl. The HCl from this cracking process is recycled by oxychlorination in order to reduce the consumption of raw material HCl (or Cl 2, if direct chlorination of ethylene is chosen as main way to produce 1,2-dichloroethane). [3]
Cl 2 + H 2 → 2 HCl. As the reaction is exothermic, the installation is called an HCl oven or HCl burner. The resulting hydrogen chloride gas is absorbed in deionized water, resulting in chemically pure hydrochloric acid. This reaction can give a very pure product, e.g. for use in the food industry. The reaction can also be triggered by blue ...
The process involves intermediate formation of sodium bisulfate, an exothermic reaction that occurs at room temperature: NaCl + H 2 SO 4 → HCl + NaHSO 4. The second step of the process is endothermic, requiring energy input: NaCl + NaHSO 4 → HCl + Na 2 SO 4. Temperatures in the range 600-700 °C are required. [5]
The ion-permeable ion-exchange membrane at the center of the cell allows only the sodium ions (Na +) to pass to the second chamber where they react with the hydroxide ions to produce caustic soda (NaOH) (B in figure): [1] Na + + OH − → NaOH The overall reaction for the electrolysis of brine is thus: 2NaCl + 2 H 2 O → Cl 2 + H 2 + 2NaOH
Catalytic oxidation are processes that rely on catalysts to introduce oxygen into organic and inorganic compounds. Many applications, including the focus of this article, involve oxidation by oxygen. Such processes are conducted on a large scale for the remediation of pollutants, production of valuable chemicals, and the production of energy. [1]
In the combustion reaction, oxygen reacts with the fuel, and the point where exactly all oxygen is consumed and all fuel burned is defined as the stoichiometric point. With more oxygen (overstoichiometric combustion), some of it stays unreacted. Likewise, if the combustion is incomplete due to lack of sufficient oxygen, fuel remains unreacted.
However, oxy-fuel is a viable alternative to removing CO 2 from the flue gas from a conventional air-fired fossil fuel plant. However, an oxygen concentrator might be able to help, as it simply removes nitrogen. In industries other than power generation, oxy-fuel combustion can be competitive due to higher sensible heat availability. Oxy-fuel ...
Heat required to initiate this reaction is generated by oxidation of a small amount of iron powder mixed with the sodium chlorate, and the reaction consumes less oxygen than is produced. Barium peroxide (Ba O 2) is used to absorb the chlorine that is a minor product in the decomposition. [10] An ignitor charge is activated by pulling on the ...