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Manganese dioxide also catalyses the decomposition of hydrogen peroxide to oxygen and water: 2 H 2 O 2 → 2 H 2 O + O 2. Manganese dioxide decomposes above about 530 °C to manganese(III) oxide and oxygen. At temperatures close to 1000 °C, the mixed-valence compound Mn 3 O 4 forms. Higher temperatures give MnO, which is reduced only with ...
Manganese(VII) oxide (manganese heptoxide) is an inorganic compound with the formula Mn 2 O 7. Manganese heptoxide is a volatile liquid with an oily consistency. It is a highly reactive and powerful oxidizer that reacts explosively with nearly any organic compound. It was first described in 1860. [1] It is the acid anhydride of permanganic acid.
In enzymology, a manganese peroxidase (EC 1.11.1.13) is an enzyme that catalyzes the chemical reaction 2 Mn(II) + 2 H + + H 2 O 2 ⇌ {\displaystyle \rightleftharpoons } 2 Mn(III) + 2 H 2 O The 3 substrates of this enzyme are Mn(II) , H + , and H 2 O 2 , whereas its two products are Mn(III) and H 2 O .
Hydrogen peroxide is a chemical compound with the formula H 2 O 2.In its pure form, it is a very pale blue [5] liquid that is slightly more viscous than water.It is used as an oxidizer, bleaching agent, and antiseptic, usually as a dilute solution (3%–6% by weight) in water for consumer use and in higher concentrations for industrial use.
The chemical reaction, in which ethylene (C 2 H 4) is oxidised by potassium permanganate (KMnO 4) to carbon dioxide (CO 2), manganese oxide (MnO 2) and potassium hydroxide (KOH), in the presence of water, is presented as follows: [55] 3 C 2 H 4 + 12 KMnO 4 + 2 H 2 O → 6 CO 2 + 2 H 2 O + 12 MnO 2 + 12 KOH
The initial aqueous solution contains hydrogen peroxide, an iodate, divalent manganese (Mn 2+) as catalyst, a strong chemically unreactive acid (sulphuric acid (H 2 SO 4) or perchloric acid (HClO 4) are good), and an organic compound with an active ("enolic") hydrogen atom attached to carbon which will slowly reduce free iodine (I 2) to iodide (I −).
Manganese(III)-mediated radical reactions begin with the single-electron oxidation of a carbonyl compound to an α-oxoalkyl radical. Addition to an olefin then occurs, generating adduct radical 2 . The fate of 2 is primarily determined by reaction conditions—in the presence of copper(II) acetate, this intermediate undergoes further oxidation ...
Nitrous oxide offers the advantages of being self-pressurizing and of being relatively non-toxic, with a specific impulse intermediate between hydrogen peroxide and hydrazine. [17] Nitrous oxide generates oxygen upon decomposition, and it is possible to blend it with fuels to form a monopropellant mixture with a specific impulse up to 325 s ...