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reportBalance = 2357 | Chemical Equation Balancer

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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.

2H2 + O2 → 2H2O 2Mg + O2 → 2MgO O2 + Si → SiO2 Na2O + SO2 → Na2SO3 C + CO2 → 2CO BaO + CO2 → BaCO3 C2H2 + CH3COCH3 → CHCC(CH3)2OH 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.

2Al(OH)3 → Al2O3 + 3H2O 4Al(NO3)3 → 2Al2O3 + 12NO2 + 3O2 Fe2(SO4)3 → Fe2O3 + 3SO3 2H3PO4 → H2O + H4P2O7 2HCl → Cl2 + H2 H2CO3 → H2O + CO2 CaCO3 → CaO + 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.

2Al + 4H2SO4 → Al2(SO4)3 + 4H2O + S 2HCl + KClO → Cl2 + H2O + KCl 2NaOH + 4NO → H2O + 2NaNO2 + N2O 2KOH + CO2 → H2O + K2CO3 4NaOH + 6NO → 2H2O + N2 + 4NaNO2 3Cl2 + 6FeSO4 → 2Fe2(SO4)3 + 2FeCl3 C + 4HNO3 → 2H2O + 4NO2 + CO2 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 C2H5OH + CH3COOH → H2O + CH3COOC2H5 3Ca + 2H3PO4 → Ca3(PO4)2 + 3H2 C + ZnO → CO + Zn Fe + CuCl2 → Cu + FeCl2 Cl2 + C6H5CH3 → HCl + C6H5CH2Cl Mg + ZnCl2 → Zn + MgCl2 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.

Na3PO4 + Al(NO3)3 → NaNO3 + AlPO4 8HCl + Ba(AlO2)2 → 2AlCl3 + BaCl2 + 4H2O CH3Cl + NaOH → CH3OH + NaCl CaCO3 + 2HCl → H2O + CO2 + CaCl2 CaO + 2HNO3 → Ca(NO3)2 + H2O Al2O3 + 6HNO3 → 3H2O + 2Al(NO3)3 2AgNO3 + CuCl2 → 2AgCl + Cu(NO3)2 View All Double-replacement reaction
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