HCl FexOy=H2O fecl2y = x-16245 | Chemical Equation Balancer

hydrogen chloride =

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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.

(NH2)2CO + H2O → (NH4)2CO3 C2H2 + C2H5OH + CO → C2H3COOC2H5 C2H2 + 2CH3CHO → HO(CH3)CHCCCH(CH3)OH 3F2 + S → SF6 2Mg + Si → Mg2Si 2H + NH2OH → NH4OH H2O + K2CO3 + CO2 → 2KHCO3 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.

2Fe(OH)3 → Fe2O3 + 3H2O MgCO3 → MgO + CO2 Hg(OH)2 → H2O + HgO C2H5OH → C2H4 + H2O 2Al(OH)3 → Al2O3 + 3H2O C4H10 → C2H4 + C2H6 2AgNO3 → 2Ag + 2NO2 + O2 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.

Fe(NO3)2 + Na2S → FeS + 2NaNO3 9H2SO4 + 6KMnO4 + 10As → 9H2O + 6MnSO4 + 3K2SO4 + 5As2O3 4CH4 + 2Cl2 + O2 → 4CH3Cl + 2H2O 2H2O + 2CuSO4 → 2Cu + 2H2SO4 + O2 Cl2 + H2O + NaHSO3 → 2HCl + NaHSO4 I2 + 2Na2S2O3 → 2NaI + Na2S4O6 10HNO3 + 3Fe(OH)2 → 8H2O + NO + 3Fe(NO3)3 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).

NH3 + (CH3CO)2O → CH3COOH + CH3CONH2 Br2 + C6H6 → C6H5Br + HBr 2Na + C6H5Br + CH3Br → C6H5CH3 + 2NaBr H2SO4 + Na2O2 → H2O2 + Na2SO4 2HCl + Mg → H2 + MgCl2 Cu(NO3)2 + Fe → Cu + Fe(NO3)2 Mg + FeSO4 → Fe + MgSO4 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.

FeCl2 + Na2S → FeS + 2NaCl Fe2(CO3)3 + 3H2O → 3CO2 + 2Fe(OH)3 Cl2 + CHCl3 → HCl + CCl4 Al2(SO4)3 + 6NaOH → 2Al(OH)3 + 3Na2SO4 FeCl2 + Na2CO3 → FeCO3 + 2NaCl CH4 + Cl2 → CH3Cl + HCl 52Al + 192HNO3 → 96H2O + 9N2 + 6NO + 6N2O + 52Al(NO3)3 View All Double-replacement reaction

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