CH3CH=CHCH3 = C2H2 C2H6 | Chemical Equation Balancer

= ethane

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Density of solid (kg/m3) 604

Boiling Point (°C) 2.25

Melting point (°C) -122.2




Atomic_weight (g/mol) 26.0373

Density of solid (kg/m3) 1.097

Boiling Point (°C) -84

Melting point (°C) -80.8




Atomic_weight (g/mol) 30.0690

Density of solid (kg/m3) 1.3562

Boiling Point (°C) -89

Melting point (°C) -183

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.

2Na + Se → Na2Se C2H2 + CO + H2O → C2H3COOH 2Al + 3Br2 → 2AlBr3 Ca3(PO4)2 + 4H3PO4 → 3Ca(H2PO4)2 CuO + H2O → Cu(OH)2 CH3CH=CHCH3 + H2O → C4H10O H2 + S → H2S 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.

2H2O + CaCl2 → Ca(OH)2 + Cl2 + 2H2 2AlCl3 → 2Al + 3Cl2 (NH4)2CO3 → H2O + 2NH3 + CO2 2HI → H2 + I2 2CH4 → C2H2 + 2H2 Ag2S → 2Ag + S 2HCl → Cl2 + H2 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.

3Cl2 + N2 → 2NCl3 Fe(NO3)2 + Na2S → FeS + 2NaNO3 H2SO4 + K2SO3 → H2O + SO2 + K2SO4 3HCl + Fe(OH)3 → 3H2O + FeCl3 2Al + 6H2O + 2NaOH → 3H2 + 2Na[Al(OH)4] 10C + P4O10 → 10CO + P4 2FeS + 9KNO3 → Fe2O3 + 9KNO2 + 2SO3 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).

2Ca(OH)2 + Mg(HCO3)2 → 2CaCO3 + 2H2O + Mg(OH)2 Mg + ZnCl2 → Zn + MgCl2 H2SO4 + BaO2 → H2O2 + BaSO4 Cl2 + 2NaBr → Br2 + 2NaCl 2Al + 3CuCl2 → 2AlCl3 + 3Cu Cl2 + C6H5CH3 → HCl + C6H5CH2Cl 2C + SiO2 → 2CO + Si 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.

2AgNO3 + H2S → 2HNO3 + Ag2S Zn + CrSO4 → Cr + ZnSO4 6CaF2 + H2SO4 + 7SO3 + Na2B4O7 → Na2SO4 + 6CaSO4 + 4BF3 H2S + CuSO4 → CuS + H2SO4 CaF2 + H2SO4 → CaSO4 + 2HF 2(NH4)3PO4 + 3H2SO4 → 3(NH4)2SO4 + 2H3PO4 BaCl2 + H2SO4 → 2HCl + BaSO4 View All Double-replacement reaction

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