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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 ...
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 .
Lead(II,IV) oxide – Pb 3 O 4; Lead(IV) oxide – PbO 2; Lead(IV) sulfide – PbS 2; Lead hydrogen arsenate – PbHAsO 4; Lead styphnate – C 6 HN 3 O 8 Pb; Lead tetrachloride – PbCl 4; Lead tetrafluoride – PbF 4; Lead tetroxide – Pb 3 O 4 [205] Lead titanate – PbTiO 3; Lead zirconate titanate – Pb[Ti x Zr 1−x]O 3 (e.g., x = 0.52 ...
Manganese oxide is any of a variety of manganese oxides and hydroxides. [1] These include Manganese(II) oxide, MnO; Manganese(II,III) oxide, Mn 3 O 4; Manganese(III) oxide, Mn 2 O 3; Manganese dioxide, MnO 2; Manganese(VI) oxide, MnO 3; Manganese(VII) oxide, Mn 2 O 7; Other manganese oxides include Mn 5 O 8, Mn 7 O 12 and Mn 7 O 13.
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.
Manganese(II) sulfate usually refers to the inorganic compound with the formula MnSO 4 ·H 2 O. This pale pink deliquescent solid is a commercially significant manganese(II) salt. Approximately 260,000 tonnes of manganese(II) sulfate were produced worldwide in 2005.
Manganese(IV) oxide was used in the original type of dry cell battery as an electron acceptor from zinc, and is the blackish material in carbon–zinc type flashlight cells. The manganese dioxide is reduced to the manganese oxide-hydroxide MnO(OH) during discharging, preventing the formation of hydrogen at the anode of the battery. [82]
Many industrial peroxides are produced using hydrogen peroxide. Reactions with aldehydes and ketones yield a series of compounds depending on conditions. Specific reactions include addition of hydrogen peroxide across the C=O double bond: R 2 C=O + H 2 O 2 → R 2 C(OH)OOH. In some cases, these hydroperoxides convert to give cyclic diperoxides: