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tat-ca = CH2=CH2 | Chemical Equation Balancer

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CH2=CH2

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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.

C2H2 + CH3COCH3 → CHCC(CH3)2OH C2H2 + HCl → C2H3Cl 2Cu + O2 → 2CuO 2F2 + Si → SiF4 (NH2)2CO + H2O → (NH4)2CO3 BaO + CO2 → BaCO3 Br2 + H2 → 2HBr 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.

2KMnO4 → MnO2 + O2 + K2MnO4 C2H6 → C2H4 + H2 2CH4 → C2H2 + 2H2 H2CO3 → H2O + CO2 C4H10 → CH3CH=CHCH3 + H2 2AlCl3 → 2Al + 3Cl2 5O2 + C4H6Cl2 → 2H2O + 2HCl + 4CO2 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.

CrCl3 + LiAlH4 → AlCl3 + H2 + CrCl2 + LiCl 2Al + 3H2SO4 → Al2(SO4)3 + 3H2 2KOH + Na2Cr2O7 → H2O + Na2CrO4 + K2CrO4 2O2 + SiF4 → SiO2 + F2O 2NaH + Fe3O4 → 3Fe + 4NaOH 2H2O + 2NH3 + CuCl2 → Cu(OH)2 + 2NH4Cl 6Li + N2 → 2Li3N 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).

2Cl2 + CH2Cl2 → HCl + CHCl3 FeCl2 + Zn → Fe + ZnCl2 Cu(NO3)2 + Zn → Cu + Zn(NO3)2 Al(OH)3 + NaOH → 2H2O + NaAlO2 H2SO4 + Mg → H2 + MgSO4 H2O + Mg → H2 + MgO C6H6 + HONO2 → H2O + C6H5NO2 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.

H2S + 2LiOH → 2H2O + Li2S H2S + CuSO4 → CuS + H2SO4 (NH4)2SO4 + Ba(NO3)2 → 2NH4NO3 + BaSO4 Fe2(SO4)3 + 6NaOH → 3Na2SO4 + 2Fe(OH)3 BaCl2 + K2SO4 → 2KCl + BaSO4 H2SO4 + Mg(OH)2 → 2H2O + MgSO4 2KOH + Mn2O7 → H2O + 2KMnO4 View All Double-replacement reaction
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Equations with CH2=CH2 as product

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