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C4H9F = tat-ca | Chemical Equation Balancer

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C4H9F



1-florobutan




Atomic_weight (g/mol) 76.1127

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.

Na2O + SO2 => Na2SO3 O2 + S => SO2 NaOH + CO2 => NaHCO3 2Mg + O2 => 2MgO C2H4 + H2O => C2H5OH 2P + 5S => P2S5 3H2O + P2O5 => 2H3PO4 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.

Na2S2O7 => Na2SO4 + SO3 HNO3 + HBr => Br2 + H2O + NO2 C2H5OH => C2H4 + H2O 2H2O + CaCl2 => Ca(OH)2 + Cl2 + 2H2 C2H6 => C2H4 + H2 CaCO3 => CaO + CO2 2KMnO4 => MnO2 + O2 + K2MnO4 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.

2SO2 + Zn => ZnS2O4 AgNO3 + Fe(NO3)2 => Ag + Fe(NO3)3 3x - 2yO2 + 4FexOy => 2xFe2O3 H2 + 2K => 2KH 3Cl2 + 2P => 2PCl3 4C + MgSO4 => 4CO + MgS 8HNO3 + 6KI => 4H2O + 3I2 + 6KNO3 + 2NO 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).

CH3CH2CH2OH + C2H5COOH => H2O + C2H5COOCH2CH2CH3 Fe + H2SO4 => H2 + FeSO4 Br2 + 2NaI => I2 + 2NaBr 2AlCl3 + 3Mg => 2Al + 3MgCl2 Fe + CuSO4 => Cu + FeSO4 2AgNO3 + Cu => 2Ag + Cu(NO3)2 Cl2 + CHCl3 => HCl + CCl4 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.

C6H5ONa + H2O + CO2 => C6H5OH + NaHCO3 Cu(OH)2 + 2HNO3 => Cu(NO3)2 + 2H2O NaOH + H3PO4 => H2O + NaH2PO4 2HCl + Na2HPO4 => 2NaCl + H3PO4 NaOH + NH4NO3 => H2O + NaNO3 + NH3 Al2(SO4)3 + 3Ca(OH)2 => 2Al(OH)3 + 3Ca(SO4) KNO3 + NaCl => View All Double-replacement reaction
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