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Mg(ClO4)2 = tat-ca | Chemical Equation Balancer

Magnesium perchlorate; Anhydrone; Dehydrite; Bishyperchloric acid magnesium salt =

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Searching in our database with more than 5552 chemical substances

Mg(ClO4)2

short form Cl2MgO8



Magie perclorat


Magnesium perchlorate; Anhydrone; Dehydrite; Bishyperchloric acid magnesium salt



Atomic_weight (g/mol) 223.2062

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.

2Cu + O2 → 2CuO 3O2 + 4P → 2P2O3 H2 + I2 → 2HI 2H + NH2OH → NH4OH C2H2 + 2CH3CHO → HO(CH3)CHCCCH(CH3)OH H2SO4 + 2NH3 → (NH4)2SO4 C2H2 + HCN → C2H3CN 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.

MgCO3 → MgO + CO2 2Al(OH)3 → Al2O3 + 3H2O 2CH4 → C2H2 + 2H2 Hg(OH)2 → H2O + HgO Fe2(SO4)3 → Fe2O3 + 3SO3 C6H12O6 → 2C2H5OH + 2CO2 3HClO3 → H2O + 2ClO2 + HClO4 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.

2H2SO4 + S → 2H2O + 3SO2 3O2 + P4 → P4O6 3CH3CHO + 4H2SO4 + K2Cr2O7 → 3CH3COOH + 4H2O + K2SO4 + Cr2(SO4)3 6Li + N2 → 2Li3N 3H2O2 + 10NaOH + 2CrCl3 → 8H2O + 6NaCl + 2Na2CrO4 6Fe(NO3)2 + 9H2SO4 → 3Fe2(SO4)3 + 4H2O + 10HNO3 + NO 14H2O2 + 12NH4OH + As2S3 → 3(NH4)2SO4 + 20H2O + 2(NH4)3AsO4 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).

Fe + 2HCl → FeCl2 + H2 Cl2 + CHCl3 → HCl + CCl4 2HCl + Zn → H2 + ZnCl2 C + ZnO → CO + Zn NH3 + (CH3CO)2O → CH3COOH + CH3CONH2 Mg + FeSO4 → Fe + MgSO4 3Cl2 + 2NH3 → 6HCl + N2 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.

2HCl + Na2S → H2S + 2NaCl CaF2 + H2SO4 → CaSO4 + 2HF (NH4)2CO3 + 2NaOH → 2H2O + Na2CO3 + 2NH3 Na2CO3 + CaCl2 → CaCO3 + 2NaCl 2KNO3 + MgCl2 → 2KCl + Mg(NO3)2 C6H5OH + 4O2 → 3H2O + 6CO2 3NaOH + Fe(NO3)3 → 3NaNO3 + Fe(OH)3 View All Double-replacement reaction
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Equations with Mg(ClO4)2 as reactant

Magnesium perchlorate; Anhydrone; Dehydrite; Bishyperchloric acid magnesium salt

View all equations with Mg(ClO4)2 as reactant
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