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tat-ca = H2MnO4 | Chemical Equation Balancer

= Manganic acid

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Searching in our database with more than 5552 chemical substances

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.

C6H5OH + 4O2 → 3H2O + 6CO2 Cl2 + Be → BeCl2 2H + NH2OH → NH4OH BaO + H2O → Ba(OH)2 C2H2 + 2CH3CHO → HO(CH3)CHCCCH(CH3)OH Na2O + SO2 → Na2SO3 C2H2 + CO + H2O → C2H3COOH 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.

CH4 → C + 2H2 C4H10 → C2H4 + C2H6 C4H10 → CH3CH=CHCH3 + H2 C2H5OH → C2H4 + H2O (NH4)2SO4 → H2SO4 + 2NH3 CaCO3 → CaO + CO2 MgCO3 → MgO + CO2 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.

MgCl2 → Cl2 + Mg H2 + C6H5COCH3 → C6H5CH(CH3)OH O2 + S → SO2 2Al + 3CuO → Al2O3 + 3Cu 2Fe + 6H2SO4 → Fe2(SO4)3 + 6H2O + 3SO2 2Na + 2NH3 → H2 + 2NaNH2 K2Cr2O7 + 2NaOH → H2O + Na2CrO4 + K2CrO4 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).

H2O + Mg → H2 + MgO NH3 + (CH3CO)2O → CH3COOH + CH3CONH2 2Mg + SiO2 → Si + 2MgO Fe + H2SO4 → H2 + FeSO4 H2SO4 + Na2O2 → H2O2 + Na2SO4 CH3Br + KCN → KBr + CH3CN 2AlCl3 + 3Mg → 2Al + 3MgCl2 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.

Ba(OH)2 + CuCl2 → BaCl2 + Cu(OH)2 2Ca3(PO4)2 + 6SiO2 → 2P2O5 + 6CaSiO3 H2O + KCl + CO2 → KHCO3 + HClO 2NaOH + H2SiO3 → 2H2O + Na2SiO3 Al2O3 + Na2SO4 H2O + NaCl + NH3 → NaHCO3 + NH4Cl 3Ba(NO3)2 + Fe2(SO4)3 → 2Fe(NO3)3 + 3BaSO4 View All Double-replacement reaction
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Manganic acid

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