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? = CH2=CH2 | Chemical Equation Balancer

? = Elayl; Ethene; Ethylene; Olefiant gas; Acetene; Eco-Sprout-Guard-EP

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CH2=CH2

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Elayl; Ethene; Ethylene; Olefiant gas; Acetene; Eco-Sprout-Guard-EP


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.

H2 + I2 => 2HI 3Cl2 + 2P => 2PCl3 2CO + O2 => 2CO2 H2 + S => H2S 2Al + 3Br2 => 2AlBr3 2H + NH2OH => NH4OH CH3COCH3 + HCN => (CH3)2C(OH)CN 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.

2CuO => 2Cu + O2 C2H6 => C2H4 + H2 2HI => H2 + I2 CaCO3 => CaO + CO2 2AgNO3 => 2Ag + 2NO2 + O2 2KMnO4 => MnO2 + O2 + K2MnO4 Cu(OH)2 => CuO + H2O 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.

H4P2O7 => H2O + 2HPO3 2Al + 2NH3 => 2AlN + 3H2 H2 + 2K => 2KH Cl2 + 2NaOH => H2O + NaCl + NaClO HClO => HCl + O2 2Al + 3Fe(NO3)2 => 3Fe + Al(NO3)3 CH4 + O2 => H2O + HCHO 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 NaOH + C2H5Cl => C2H5OH + NaCl 2Na + 2NH3 => H2 + 2NaNH2 C2H5OH + CH3COOH => H2O + CH3COOC2H5 H2SO4 + Mg => H2 + MgSO4 3Cl2 + 2NH3 => 6HCl + N2 2Al + 6HBr => 3H2 + 2AlBr3 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.

3Ag2SO4 + 2FeCl3 => 6AgCl + Fe2(SO4)3 Al(OH)3 + 3HCl => AlCl3 + 3H2O K2CO3 + 2NaHSO4 => H2O + Na2SO4 + K2SO4 + CO2 Ca(OH)2 + 2NH4Cl => 2H2O + 2NH3 + CaCl2 Ca(OH)2 + 2HNO3 => Ca(NO3)2 + 2H2O 2H2O + SiCl4 => 4H2O + SiO2 2NaOH + ZnSO4 => Na2SO4 + Zn(OH)2 View All Double-replacement reaction
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Equations with CH2=CH2 as product

Elayl; Ethene; Ethylene; Olefiant gas; Acetene; Eco-Sprout-Guard-EP

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