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.

5Cl2 + 2P → 2PCl5 2Al + 3I2 → 2AlI3 Na2O + SO2 → Na2SO3 NaOH + CO2 → NaHCO3 H2 + S → H2S C2H2 + HCN → C2H3CN O2 + Si → SiO2 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.

2Al(OH)3 → Al2O3 + 3H2O C2H6 → C2H4 + H2 4Al(NO3)3 → 2Al2O3 + 12NO2 + 3O2 2Fe(OH)3 → Fe2O3 + 3H2O 2Ag2O → 4Ag + O2 C4H10 → CH3CH=CHCH3 + H2 2CuO → 2Cu + 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.

2Al + 3Cu(NO3)2 → 3Cu + 2Al(NO3)3 2AgNO3 + ZnCl2 → 2AgCl + Zn(NO3)2 4NaOH → 2H2O + 4Na + O2 3H2S + 2HNO3 → 4H2O + 2NO + 2S 8Al + 30HNO3 → 9H2O + 3NH4NO3 + 8Al(NO3)3 CaC2 + N2 → C + CaCN2 2Ag + O3 → Ag2O + O2 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).

Br2 + CH4 → CH3Br + HBr C6H5Cl + 2NaOH → C6H5ONa + H2O + NaCl Br2 + C2H6 → C2H5Br + HBr 4Al + 3SiO2 → 2Al2O3 + 3Si 2HNO3 + Ni → H2 + Ni(NO3)2 H2SO4 + BaO2 → H2O2 + BaSO4 CH4 + Cl2 → CH3Cl + HCl 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.

Na2HPO4 + NaOH → H2O + Na3PO4 3Ba(NO3)2 + 2K3PO4 → 6KNO3 + Ba3(PO4)2 2HNO3 + K2CO3 → H2O + 2KNO3 + CO2 (CH3COO)2Ca + H2SO4 → 2CH3COOH + CaSO4 Cr + 2HCl → H2 + CrCl2 HCl + [Zn(NH3)4]Cl2 → NH4Cl + ZnCl2 2HCl + Mg(OH)2 → 2H2O + MgCl2 View All Double-replacement reaction

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