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.

O2 + S → SO2 H2SO4 + NH3 → NH4HSO4 C2H2 + HCl → C2H3Cl 5O2 + 4P → 2P2O5 2H + NH2OH → NH4OH 2H2 + O2 → 2H2O 2Mg + Si → Mg2Si 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.

2C2H5OH → H2O + C2H5OC2H5 MgCO3 → MgO + CO2 C4H10 → CH3CH=CHCH3 + H2 (NH4)2Cr2O7 → 4H2O + N2 + Cr2O3 2KClO3 → 2KCl + 3O2 C4H10 → C2H4 + C2H6 2H2O + CaCl2 → Ca(OH)2 + Cl2 + 2H2 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.

3CO + Fe2O3 → 2Fe + 3CO2 CO + Na2O2 → Na2CO3 4CH4 + 2Cl2 + O2 → 4CH3Cl + 2H2O 2P2O5 + 3HBr → 3HPO3 + POBr3 2F2 + Si → SiF4 Li + 2S → Li2S 2HNO3 + Ni → H2 + Ni(NO3)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).

CH3Br + KCN → KBr + CH3CN 2HNO3 + Ni → H2 + Ni(NO3)2 2H2O + 2Na → H2 + 2NaOH Fe + 2HCl → FeCl2 + H2 2Na + C6H5Br + CH3Br → C6H5CH3 + 2NaBr C6H5NH3Cl + NaOH → C6H5NH2 + H2O + NaCl 2AgNO3 + Cu → 2Ag + Cu(NO3)2 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.

4NH3 + Zn(OH)2 → [Zn(NH3)4](OH)2 NaOH + NaHS → H2O + Na2S Ca(NO3)2 + 2NaF → CaF2 + 2NaNO3 H2S + LiOH → H2O + LiSH 3Cu(OH)2 + 2Fe(NO3)3 → 3Cu(NO3)2 + 2Fe(OH)3 AlCl3 + 3H2O + 3NH3 → Al(OH)3 + 3NH4Cl FeCl2 + 2NaOH → 2NaCl + Fe(OH)2 View All Double-replacement reaction

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