CH3CH2CH2CH2OH = CH3CH=CHCH3 H2O | Chemical Equation Balancer

butan-1-ol = water

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short form C4H10O



Atomic_weight (g/mol) 74.1216


short form


Density of solid (kg/m3) 604

Boiling Point (°C) 2.25

Melting point (°C) -122.2




Atomic_weight (g/mol) 18.01528 ± 0.00044

Density of solid (kg/m3) 1

Boiling Point (°C) 100

Melting point (°C) 4

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.

CH3CH=CHCH3 + H2O → C4H10O O2 + S → SO2 2H2 + O2 → 2H2O 2F2 + Si → SiF4 CaO + H2O → Ca(OH)2 3Cl2 + 2P → 2PCl3 Fe + 2Fe(NO3)3 → 3Fe(NO3)2 View All Combination reaction

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.

C2H5OH → C2H4 + H2O 2CuO → 2Cu + O2 2NaHCO3 → H2O + Na2CO3 + CO2 CaCl2 → Ca + Cl2 2KClO3 → 2KCl + 3O2 C2H5Cl → C2H4 + HCl 2HgO → 2Hg + O2 View All Decomposition reaction

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.

6Fe2O3 → O2 + 4Fe3O4 Na2SO3 + S → Na2S2O3 H2SO4 + 2HBr → Br2 + 2H2O + SO2 8H2SO4 + 2KMnO4 + 10NaBr → 5Br2 + 8H2O + 2MnSO4 + 5Na2SO4 + K2SO4 2HNO3 + S → H2SO4 + 2NO 2C + SiO2 → 2CO + Si CaC2 + 2H2O → C2H2 + Ca(OH)2 View All Oxidation-reduction reaction

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).

Zn + CuSO4 → Cu + ZnSO4 Br2 + C6H6 → C6H5Br + HBr 2Al + 6HCl → 2AlCl3 + 3H2 3Cl2 + 6Fe(NO3)2 → 4Fe(NO3)3 + 2FeCl3 CH3Br + KCN → KBr + CH3CN Cu(NO3)2 + Fe → Cu + Fe(NO3)2 Cl2 + 2NaI → I2 + 2NaCl View All Single-replacement reaction

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.

HCl + NaBr → NaCl + HBr NaOH + SO2 → NaHSO3 3Ba(NO3)2 + Fe2(SO4)3 → 2Fe(NO3)3 + 3BaSO4 H2S + CsOH → H2O + Cs2S 2KNO3 + MgCl2 → 2KCl + Mg(NO3)2 H2S + Li2O → H2O + Li2S ZnCl2 + Ba(OH)2 → BaCl2 + Zn(OH)2 View All Double-replacement reaction

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