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C4H10 = CH3CH=CHCH3 H2 | Chemical Equation Balancer

butane = hydrogen

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Searching in our database with more than 5552 chemical substances

C4H10



Butan


butane



Atomic_weight (g/mol) 58.1222


Density of solid (kg/m3) 2.48

CH3CH=CHCH3

short form



but-2-en




Density of solid (kg/m3) 604


Boiling Point (°C) 2.25


Melting point (°C) -122.2

H2



hidro


hydrogen



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.

5Cl2 + 2P → 2PCl5 C2H2 + CH3COCH3 → CHCC(CH3)2OH Ca3(PO4)2 + 4H3PO4 → 3Ca(H2PO4)2 H2O + N2O5 → 2HNO3 H2O + ZnO → Zn(OH)2 Cl2 + H2 → 2HCl BaO + P2O5 → Ba3(PO4)2 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.

2CH4 → C2H2 + 2H2 Cu(OH)2 → CuO + H2O 2NaHCO3 → H2O + Na2CO3 + CO2 2HI → H2 + I2 HNO3 + HBr → Br2 + H2O + NO2 2C2H5OH → H2O + C2H5OC2H5 CH4 → C + 2H2 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.

3H2SO4 + K2Cr2O7 + 3K2SO3 → 2H2O + 2KOH + 3K2SO4 + Cr2(SO4)3 2F2 + 2H2O → O2 + 4HF 2H2O + O2 + 4Fe(OH)2 → 4Fe(OH)3 3HNO3 + B → 3NO2 + H3BO3 C2H4 + 3O2 → 2H2O + 2CO2 3HCl + 2P2O5 → POCl3 + 3HPO3 H2 + 2K → 2KH 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).

4Cl2 + 2Fe2O3 → 4FeCl2 + 3O2 CH3Cl + CH3COOH → HCl + CH3COOCH3 C2H2 + 2Na → H2 + Na2C2 Fe + H2SO4 → H2 + FeSO4 Ag2O + C2H2 → H2O + C2Ag2 2Al + 6HCl → 2AlCl3 + 3H2 Br2 + C2H6 → C2H5Br + HBr 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.

CH3Cl + Cl2 → HCl + CH2Cl2 Ca3N2 + 3H2O → 3Ca(OH)2 + 2NH3 6H2O + Mg3N2 → 3Mg(OH)2 + 2NH3 H2SO4 + NaBr → NaHSO4 + HBr H2O + Na2CO3 + MgSO4 → Mg(OH)2 + Na2SO4 + CO2 AgNO3 + KCl → AgCl + KNO3 CaO + 2HNO3 → Ca(NO3)2 + H2O View All Double-replacement reaction
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