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? = H2MnO4 | Chemical Equation Balancer

? = Manganic acid

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H2MnO4



Manganic acid


Manganic acid



Atomic_weight (g/mol) 120.9515

Combination reaction

Also known as a synthesis reaction. One kind of frequently occurring combination reaction is the reaction of an element with oxygen to form an oxide. Under certain conditions, metals and nonmetals both react readily with oxygen. Once ignited, magnesium reacts rapidly and dramatically, reacting with oxygen from the air to create a fine magnesium oxide powder.

O2 + S → SO2 Na2O + SO2 → Na2SO3 H2SO4 + 2NH3 → (NH4)2SO4 C2H2 + C2H5OH + CO → C2H3COOC2H5 HCl + NH3 → NH4Cl 2Mg + O2 → 2MgO 2Al + 3Br2 → 2AlBr3 View All Combination reaction
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Decomposition reaction

Many decomposition reactions involve heat , light, or electricity to input energy. Binary compounds are compounds which consist of only two elements. The simplest sort of reaction to decomposition is when a binary compound breaks down into its elements. Mercury (II) oxide, a red solid, decomposes to form mercury and oxygen gas when heated. Also, a reaction is regarded as a decomposition reaction even if one or more of the products are still a compound. A metal carbonate breaks down to form a metal oxide and carbon dioxide gas. Calcium carbonate for example decomposes into calcium oxide and carbon dioxide.

2AgNO3 → 2Ag + 2NO2 + O2 4Al(NO3)3 → 2Al2O3 + 12NO2 + 3O2 2Fe(OH)3 → Fe2O3 + 3H2O CaCl2 → Ca + Cl2 Fe2(SO4)3 → Fe2O3 + 3SO3 2H2O2 → 2H2O + O2 2CuO → 2Cu + O2 View All Decomposition reaction
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Oxidation-reduction reaction

An oxidation-reduction (redox) reaction is a type of chemical reaction that involves a transfer of electrons between two species. An oxidation-reduction reaction is any chemical reaction in which the oxidation number of a molecule, atom, or ion changes by gaining or losing an electron. Redox reactions are common and vital to some of the basic functions of life, including photosynthesis, respiration, combustion, and corrosion or rusting.

2Al + 3Zn(NO3)2 → 3Zn + 2Al(NO3)3 CO + 3Fe2O3 → CO2 + 2Fe3O4 2KI → I2 + 2K Fe + 2H2SO4 → 2H2O + SO2 + FeSO4 KNO3 + 7KOH + 4Zn → 2H2O + NH3 + 4K2ZnO2 HI + 2HNO3 → H2O + 2NO + HIO3 2Fe + 6H2SO4 → Fe2(SO4)3 + 6H2O + 3SO2 View All Oxidation-reduction reaction
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Single-replacement reaction

A + BC → AC + B Element A is a metal in this general reaction and replaces element B, a metal in the compound as well. If the replacement element is a non-metal, it must replace another non-metal in a compound, and it becomes the general equation. Many metals easily react with acids, and one of the reaction products when they do so is hydrogen gas. Zinc reacts to the aqueous zinc chloride and hydrogen with hydrochloride acid (see figure below).

Cu(NO3)2 + Fe → Cu + Fe(NO3)2 Br2 + 2AgI → 2AgBr + I2 H2O + Mg → H2 + MgO H2SO4 + Mg → H2 + MgSO4 Fe + CuSO4 → Cu + FeSO4 NH3 + (CH3CO)2O → CH3COOH + CH3CONH2 Fe + 2HCl → FeCl2 + H2 View All Single-replacement reaction
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Double-replacement reaction

AB + CD → AD + CB A and C are positive charged cations in this reaction, while B and D are negative charged anions. Double-replacement reactions typically occur in aqueous solution between the compounds. To cause a reaction, one of the products is usually a solid precipitate, a gas, or a molecular compound like water. A precipitate forms in a double-replacement reaction when the cations from one reactant combine to form an insoluble ionic compound with the anions from the other reactant. The following reaction occurs when aqueous solutions of potassium iodide and lead ( II) nitrate are blended.

4NH3 + Zn(OH)2 → [Zn(NH3)4](OH)2 (NH4)2CO3 + H2SO4 → (NH4)2SO4 + H2O + CO2 2K3PO4 + 3CaCl2 → Ca3(PO4)2 + 6KCl H2O + KCl + CO2 → KHCO3 + HClO H2SO4 + Ba(ClO2)2 → HClO3 + BaSO4 H2SO4 + 2KHS → H2S + K2SO4 + H2NNHCO2CH2CH3 HCl + NaF → NaCl + HF View All Double-replacement reaction
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Manganic acid

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