tat-ca = Ag(NO3) | Chemical Equation Balancer

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short form AgNO3

Bạc nitrat

Atomic_weight (g/mol) 169.8731

Density of solid (kg/m3) 4350

Boiling Point (°C) 444

Melting point (°C) 212

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.

O2 + Se → SeO2 Cl2 + H2 → 2HCl NaOH + CO2 → NaHCO3 BaO + CO2 → BaCO3 CaO + CO2 → CaCO3 2Cu + O2 → 2CuO 3O2 + 4P → 2P2O3 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.

2C2H5OH → H2O + C2H5OC2H5 C6H12O6 → 2C2H5OH + 2CO2 HNO3 + HBr → Br2 + H2O + NO2 (NH4)2SO4 → H2SO4 + 2NH3 C2H5Cl → C2H4 + HCl C4H10 → CH3CH=CHCH3 + H2 2Cu(NO3)2 → 2CuO + 4NO2 + 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.

CuS + 10HNO3 → Cu(NO3)2 + 4H2O + H2SO4 + 8NO2 H2O + Na2CO3 + CO2 → 2NaHCO3 3H2SO4 + Pb → 2H2O + SO2 + Pb(HSO4)2 FeS + Mg → Fe + MgS H2O + 2KI + O3 → I2 + 2KOH + O2 H2S + H2SO3 → H2O + 2S 6HCl + KClO3 → 3Cl2 + 3H2O + KCl 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).

2Mg + SiO2 → Si + 2MgO C + ZnO → CO + Zn CH3COCl + 2C2H5NH2 → NH3 + C2H5Cl + CH3CONHC2H5 2Cl2 + CH2Cl2 → HCl + CHCl3 2H2O + 2Na → H2 + 2NaOH Mg + FeSO4 → Fe + MgSO4 Fe + 2HCl → FeCl2 + H2 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.

Ca(NO3)2 + Na2CO3 → CaCO3 + 2NaNO3 2K3PO4 + 3CaCl2 → Ca3(PO4)2 + 6KCl CaO + H2SO4 → H2O + CaSO4 Ca(OH)2 + H2S → 2H2O + CaS 3H2O + Na3Sb → H2O2 + 3NaOH 3NaOH + Fe(NO3)3 → 3NaNO3 + Fe(OH)3 HNO3 + Ag3PO4 → AgNO3 + H3PO4 View All Double-replacement reaction

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