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This reaction is exploited in the industrial production of sodium chlorate. An alternative decomposition of hypochlorite produces oxygen instead: 2 OCl − → 2 Cl − + O 2. In hot sodium hypochlorite solutions, this reaction competes with chlorate formation, yielding sodium chloride and oxygen gas: [25] 2 NaOCl(aq) → 2 NaCl(aq) + O 2 (g)
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 ...
Hypochlorous acid is an inorganic compound with the chemical formula Cl O H, also written as HClO, HOCl, or ClHO. [2] [3] Its structure is H−O−Cl.It is an acid that forms when chlorine dissolves in water, and itself partially dissociates, forming a hypochlorite anion, ClO −.
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]
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]
For example, sodium hydroxide, NaOH, is a strong base. NaOH(aq) → Na + (aq) + OH − (aq) Therefore, when a strong acid reacts with a strong base the neutralization reaction can be written as H + + OH − → H 2 O. For example, in the reaction between hydrochloric acid and sodium hydroxide the sodium and chloride ions, Na + and Cl − take ...
Alcohol oxidation is a collection of oxidation reactions in organic chemistry that convert alcohols to aldehydes, ketones, carboxylic acids, and esters. The reaction mainly applies to primary and secondary alcohols. Secondary alcohols form ketones, while primary alcohols form aldehydes or carboxylic acids. [1] A variety of oxidants can be used.
Hypochlorite salts formed by the reaction between chlorine and alkali and alkaline earth metal hydroxides. The reaction is performed at close to room temperature to suppress the formation of chlorates. This process is widely used for the industrial production of sodium hypochlorite (NaClO) and calcium hypochlorite (Ca(ClO) 2).