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An element–reaction–product table is used to find coefficients while balancing an equation representing a chemical reaction. Coefficients represent moles of a substance so that the number of atoms produced is equal to the number of atoms being reacted with. [1] This is the common setup: Element: all the elements that are in the reaction ...
In the first step of the catalytic cycle, H 2 O 2, or an organic peroxide, enters the active site of MnP. There the oxygen in H 2 O 2 binds to an Fe(III) ion in the heme cofactor to form an iron peroxide complex. Two electrons are transferred from Fe 3+ to peroxide, breaking the oxygen-peroxide bond to form H 2 O and a Fe(IV) oxo-porphyrin ...
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 ...
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.
Depending on the conditions in which the titration is performed, the manganese is reduced from an oxidation of +7 to +2, +4, or +6. In most cases, permanganometry is performed in a very acidic solution in which the following electrochemical reaction occurs: [3] MnO − 4 + 8 H + + 5 e − → Mn 2+ + 4 H 2 O; E° = +1.51 V [4]
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:
The standard Gibbs free energy of formation (G f °) of a compound is the change of Gibbs free energy that accompanies the formation of 1 mole of a substance in its standard state from its constituent elements in their standard states (the most stable form of the element at 1 bar of pressure and the specified temperature, usually 298.15 K or 25 °C).
Thiosulfates, e.g. Na 2 S 2 O 3 (mainly in analytical chemistry) [11] Iodides, such as potassium iodide (K I) (mainly in analytical chemistry) Hydrogen peroxide (H 2 O 2) – mostly an oxidant but can occasionally act as a reducing agent, typically in analytical chemistry [citation needed] Hydrazine (Wolff-Kishner reduction) Diisobutylaluminium ...