? = CH3CH=CHCH3 | Chemical Equation Balancer
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CH3CH=CHCH3
short form
but-2-en
Density of solid (kg/m3) 604
Boiling Point (°C) 2.25
Melting point (°C) -122.2
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.
PH3 + HClO4 → PH4ClO4 C2H2 + 2HCHO → HOCH2CCCH2OH O2 + S → SO2 H2 + I2 → 2HI 2H + NH2OH → NH4OH CH3CH=CHCH3 + H2O → C4H10O Cl2 + Be → BeCl2 View All Combination reactionDecomposition 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.
HNO3 + HBr → Br2 + H2O + NO2 (NH4)2SO4 → H2SO4 + 2NH3 C2H5OH → C2H4 + H2O 2Al(OH)3 → Al2O3 + 3H2O NH4Cl → HCl + NH3 2CuO → 2Cu + O2 2NaHCO3 → H2O + Na2CO3 + CO2 View All Decomposition reactionOxidation-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.
Li + 2S → Li2S 2Al + 3Cu(NO3)2 → 3Cu + 2Al(NO3)3 Zn + FeCl3 → FeCl2 + ZnCl2 NH4NO2 → 2H2O + N2 3C + Fe2O3 → 3CO + Fe 3H2S + 2HNO3 → 4H2O + 2NO + 2S 2NaOH + Zn → H2 + Na2ZnO2 View All Oxidation-reduction reactionSingle-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).
2Ca(OH)2 + Mg(HCO3)2 → 2CaCO3 + 2H2O + Mg(OH)2 4Al + 3SiO2 → 2Al2O3 + 3Si C6H5NH3Cl + NaOH → C6H5NH2 + H2O + NaCl CH4 + Cl2 → CH3Cl + HCl CH3Cl + CH3COOH → HCl + CH3COOCH3 CH4 + 2Cl2 → C + 4HCl 2Cl2 + CH2Cl2 → HCl + CHCl3 View All Single-replacement reactionDouble-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.
2H2O + 2NH3 + CuSO4 → (NH4)2SO4 + Cu(OH)2 2K3PO4 + 3CaCl2 → Ca3(PO4)2 + 6KCl 2NaOH + CrSO4 → Na2SO4 + Cr(OH)2 H2SO4 + (COONa)2 → Na2SO4 + (COOH)2 H2SO4 + Na2CO3 → H2O + Na2SO4 + CO2 3HCl + Ag3PO4 → 3AgCl + H3PO4 2HNO3 + Mg(OH)2 → 2H2O + Mg(NO3)2 View All Double-replacement reactionYou cound not find ?
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