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? = MgBr | Chemical Equation Balancer

? = Magnesium bromide; Magnesium dibromide; Dibromomagnesium; Bromomagnesium bromide

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MgBr

short form BrMg



Magie bromua


Magnesium bromide; Magnesium dibromide; Dibromomagnesium; Bromomagnesium bromide



Atomic_weight (g/mol) 104.2090

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.

H2O + N2O5 → 2HNO3 BaO + H2O → Ba(OH)2 C2H2 + 2HCHO → HOCH2CCCH2OH Ca3(PO4)2 + H3PO4 → 3CaHPO4 CaO + H2O → Ca(OH)2 HCl + NH3 → NH4Cl 3Cl2 + 2P → 2PCl3 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.

3HClO3 → H2O + 2ClO2 + HClO4 2Fe(OH)3 → Fe2O3 + 3H2O 2HI → H2 + I2 C2H5Cl → C2H4 + HCl NH4Cl → HCl + NH3 2KClO3 → 2KCl + 3O2 Na2S2O7 → Na2SO4 + SO3 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.

Cl2 + H2S → 2HCl + S 2SO2 + Zn → ZnS2O4 5KClO3 + 6P → 5KCl + 3P2O5 3Br2 + 8NaOH + 2NaCrO2 → 8H2O + 2Na2CrO4 + 6NaBr 2Cl2 + Si → SiCl4 CO + 3Fe2O3 → CO2 + 2Fe3O4 2Fe(NO3)2 → 2FeO + 4NO2 + O2 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).

2Na + 2NH3 → H2 + 2NaNH2 C2H5OH + HBr → H2O + C2H5Br Mg + ZnCl2 → Zn + MgCl2 CH4 + Cl2 → CH3Cl + HCl CH3Br + KCN → KBr + CH3CN C2H2 + 2[Ag(NH3)2]OH → H2O + NH3 + C2Ag2 Cu(NO3)2 + Fe → Cu + Fe(NO3)2 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.

Ca(OH)2 + 2CH3COOH → (CH3COO)2Ca + 2H2O NaOH + HAlO2.H2O → 2H2O + NaAlO2 NaOH + NaHSO3 → H2O + Na2SO3 H2SO4 + K2O → H2O + K2SO4 Cu(NO3)2 + Na2SO4 H2S + Li2O → H2O + Li2S 3NaOH + Fe(NO3)3 → 3NaNO3 + Fe(OH)3 View All Double-replacement reaction
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Equations with MgBr as product

Magnesium bromide; Magnesium dibromide; Dibromomagnesium; Bromomagnesium bromide

View all equations with MgBr as product
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