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? = BaO2.8H2O | Chemical Equation Balancer

? = Barium peroxide octahydrate

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BaO2.8H2O

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Bari peroxit octahidrat


Barium peroxide octahydrate


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.

4Al + 3O2 → 2Al2O3 Br2 + H2 → 2HBr Cl2 + H2 → 2HCl O2 + Si → SiO2 O2 + Se → SeO2 Cl2 + Mg → MgCl2 CuO + H2O → Cu(OH)2 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.

2HgO → 2Hg + O2 C2H5Cl → C2H4 + HCl 3HClO3 → H2O + 2ClO2 + HClO4 2H2O + CaCl2 → Ca(OH)2 + Cl2 + 2H2 C4H10 → C2H4 + C2H6 H2CO3 → H2O + CO2 C4H10 → CH4 + C3H6 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.

10HNO3 + 8Na → 3H2O + 8NaNO3 + NH4NO3 Ag + 2HNO3 → AgNO3 + H2O + NO2 4FeCO3 + O2 → 2Fe2O3 + 4CO2 C + SiO2 → Si + CO2 2Al + 6HCl → 2AlCl3 + 3H2 H2SO4 + 2HI → 2H2O + I2 + SO2 2HClO4 → H2O + Cl2O7 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 2HNO3 + Ni → H2 + Ni(NO3)2 2Al + 6HBr → 3H2 + 2AlBr3 Cl2 + 2NaBr → Br2 + 2NaCl 2C + SiO2 → 2CO + Si Zn + CuSO4 → Cu + ZnSO4 4Al + 3SiO2 → 2Al2O3 + 3Si 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 + H2SO4 → 2H2O + CaSO4 3Ag2SO4 + 2FeCl3 → 6AgCl + Fe2(SO4)3 HCl + [Zn(NH3)4]Cl2 → NH4Cl + ZnCl2 Al2O3 + 2KOH → H2O + 2KAlO2 H2SO4 + Ba(ClO2)2 → HClO3 + BaSO4 Ca(OH)2 + 2HCl → 2H2O + CaCl2 Na2CO3 + CaCl2 → CaCO3 + 2NaCl View All Double-replacement reaction
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Barium peroxide octahydrate

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