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? = C6H11CH3 | Chemical Equation Balancer

? = methyl cyclohexane

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Searching in our database with more than 5552 chemical substances

C6H11CH3

short form C7H14



metylcyclohexane


methyl cyclohexane



Atomic_weight (g/mol) 98.1861

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.

F2 + H2 → 2HF O2 + S → SO2 2CO + O2 → 2CO2 PH3 + HClO4 → PH4ClO4 O2 + Si → SiO2 SnCl4 + Sn → 2SnCl2 2Cu + O2 → 2CuO 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.

H2CO3 → H2O + CO2 FeCl2 → Cl2 + Fe 2Ag2O → 4Ag + O2 HNO3 + HBr → Br2 + H2O + NO2 (NH4)2SO4 → H2SO4 + 2NH3 4Al(NO3)3 → 2Al2O3 + 12NO2 + 3O2 (NH4)2CO3 → H2O + 2NH3 + CO2 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.

2Al + 6HCl → 2AlCl3 + 3H2 Cu(NO3)2 + Fe → Cu + Fe(NO3)2 2H2SO4 + 2KBr + MnO2 → Br2 + 2H2O + MnSO4 + K2SO4 2H2SO4 + 2KI + 2NaNO2 → 2H2O + I2 + Na2SO4 + NO + K2SO4 3S + 2B → B2S3 2H2O + 2KMnO4 + 3MnSO4 → 2H2SO4 + 5MnO2 + K2SO4 Al + Bi2(SO4)5 → Al2(SO4)3 + Bi 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).

CH3COCl + 2C2H5NH2 → NH3 + C2H5Cl + CH3CONHC2H5 2HCl + Mg → H2 + MgCl2 Cl2 + 2NaBr → Br2 + 2NaCl 2AlCl3 + 3Mg → 2Al + 3MgCl2 NaOH + C2H5Cl → C2H5OH + NaCl Br2 + 2NaI → I2 + 2NaBr CH4 + 2Cl2 → C + 4HCl 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.

2KOH + Mn2O7 → H2O + 2KMnO4 3Ca(NO3)2 + 2Na3PO4 → Ca3(PO4)2 + 6NaNO3 SbCl5 + 5HF → 5HCl + SbF5 K2CO3 + BaS → K2S + BaCO3 Na2CO3 + Mg(HCO3)2 → MgCO3 + 2NaHCO3 BaCl2 + HNO3 Na2SO4 + Pb(NO3)2 → 2NaNO3 + PbSO4 View All Double-replacement reaction
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methyl cyclohexane

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