HCl FexOy=H2O fecl2y = x-16245 | Chemical Equation Balancer
hydrogen chloride =
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HCl
short form ClH
axit clohidric
hydrogen chloride
Atomic_weight (g/mol) 36.4609
Density of solid (kg/m3) 1180
Boiling Point (°C) 110
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.
C2H2 + CH3COCH3 => CHCC(CH3)2OH CuO + H2O => Cu(OH)2 Fe + S => FeS H2O + N2O5 => 2HNO3 PH3 + HClO4 => PH4ClO4 2Na + Se => Na2Se 2Al + 3I2 => 2AlI3 View All Combination reactionDecomposition 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.
C4H10 => CH4 + C3H6 2CuO => 2Cu + O2 3HClO3 => H2O + 2ClO2 + HClO4 2KClO3 => 2KCl + 3O2 2AgNO3 => 2Ag + 2NO2 + O2 2Cu(NO3)2 => 2CuO + 4NO2 + O2 C4H10 => C2H4 + C2H6 View All Decomposition reactionOxidation-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.
H2SO4 + SO2 + 2NaClO3 => 2ClO2 + 2NaHSO4 C + Fe(CrO2)2 => Cr + Fe + 2CO2 2Cl2 + 2Ba(OH)2 => BaCl2 + 2H2O + Ba(ClO)2 2FeS + 9KNO3 => Fe2O3 + 9KNO2 + 2SO3 3Fe + 4H2O => 4H2 + Fe3O4 NH4Cl => HCl + NH3 3H2SO4 + 2Fe(OH)3 => Fe2(SO4)3 + 6H2O View All Oxidation-reduction reactionSingle-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).
2Na + 2NH3 => H2 + 2NaNH2 C6H5Cl + KOH => C6H5OH + KCl 3Cl2 + 2NH3 => 6HCl + N2 3HNO3 + C6H5CH3 => 3H2O + C6H2CH3(NO2)3 4Cl2 + 2Fe2O3 => 4FeCl2 + 3O2 CH3CH2CH2OH + C2H5COOH => H2O + C2H5COOCH2CH2CH3 H2SO4 + Mg => H2 + MgSO4 View All Single-replacement reactionDouble-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.
Mg + 2KHSO4 => H2 + K2SO4 + MgSO4 NaOH + NaHSO4 => H2O + Na2SO4 Ca(OH)2 + H2S => 2H2O + CaS H2S + KOH => H2O + KSH NaOH + NaHSO3 => H2O + Na2SO3 Ba(NO3)2 + CuSO4 => Cu(NO3)2 + BaSO4 K2CO3 + SiO2 => CO2 + K2SiO3 View All Double-replacement reactionYou cound not find ?
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Equations with HCl as reactant
hydrogen chloride
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