C4H10 = CH3CH=CHCH3 H2 | Chemical Equation Balancer

butane = hydrogen

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Atomic_weight (g/mol) 58.1222

Density of solid (kg/m3) 2.48


short form


Density of solid (kg/m3) 604

Boiling Point (°C) 2.25

Melting point (°C) -122.2




Atomic_weight (g/mol) 2.01588 ± 0.00014

Density of solid (kg/m3) 70

Boiling Point (°C) -252

Melting point (°C) -259

Electron negativity 2

First Ionisation Energy 1312

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.

2Al + 3Br2 → 2AlBr3 C2H2 + CH3OH → CH3OCHCH2 2CO + O2 → 2CO2 BaO + CO2 → BaCO3 Fe + S → FeS C2H4 + H2O → C2H5OH 3O2 + 4P → 2P2O3 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.

2HCl → Cl2 + H2 NH4Cl → HCl + NH3 2Ag2O → 4Ag + O2 C4H10 → CH4 + C3H6 C4H10 → CH3CH=CHCH3 + H2 CH4 → C + 2H2 Ag2S → 2Ag + S 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.

K2Cr2O7 + 2NaOH → H2O + Na2CrO4 + K2CrO4 FeCO3 → FeO + CO2 2H2O + 2KMnO4 + 3MnSO4 → 2H2SO4 + 5MnO2 + K2SO4 4NaH + B(OCH3)3 → NaBH4 + 3NaOCH3 2HCl + Ni → H2 + NiCl2 4H2 + Fe3O4 → 3Fe + 4H2O 2Al + 4H2SO4 → Al2(SO4)3 + 4H2O + S 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).

H2O + Mg → H2 + MgO Mg + FeSO4 → Fe + MgSO4 H2SO4 + Na2O2 → H2O2 + Na2SO4 Cl2 + 2NaBr → Br2 + 2NaCl C6H5NH3Cl + NaOH → C6H5NH2 + H2O + NaCl Br2 + C2H6 → C2H5Br + HBr 4Al + 3SiO2 → 2Al2O3 + 3Si 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.

FeS + 2HCl → FeCl2 + H2S Ba(NO3)2 + K2SO4 → 2KNO3 + BaSO4 2AgNO3 + H2S → 2HNO3 + Ag2S H2O + KH → H2 + KOH Ca(OH)2 + SO2 → H2O + CaSO3 FeCl2 + 2NaOH → 2NaCl + Fe(OH)2 3H2SO4 + 2Fe(NO3)3 → Fe2(SO4)3 + 6HNO3 View All Double-replacement reaction

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