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H2SO4 HNO3 = NO2 HSO4��� H3O | Chemical Equation Balancer

nitric acid =

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Searching in our database with more than 5552 chemical substances

H2SO4

short form H2O4S



axit sulfuric


sulfuric acid



Atomic_weight (g/mol) 98.0785


Density of solid (kg/m3) 1840


Boiling Point (°C) 338


Melting point (°C) 10

HNO3



axit nitric


nitric acid



Atomic_weight (g/mol) 63.0128


Density of solid (kg/m3) 1510


Boiling Point (°C) 83


Melting point (°C) -42

NO2



nitơ dioxit


nitrogen dioxide



Atomic_weight (g/mol) 46.00550 ± 0.00080


Density of solid (kg/m3) 1880


Boiling Point (°C) 21

H3O+



Hydronium ion




Atomic_weight (g/mol) 19.02322 ± 0.00051

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.

CaO + CO2 → CaCO3 C6H5OH + 4O2 → 3H2O + 6CO2 2Mg + O2 → 2MgO 4Al + 3O2 → 2Al2O3 H2SO4 + 2NH3 → (NH4)2SO4 C2H2 + CO + H2O → C2H3COOH Cl2 + Be → BeCl2 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.

C2H6 → C2H4 + H2 2HgO → 2Hg + O2 2KClO3 → 2KCl + 3O2 2HI → H2 + I2 2AlCl3 → 2Al + 3Cl2 Ag2S → 2Ag + S Cu(OH)2 → CuO + H2O 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.

2H2SO4 + MnO2 + 2FeSO4 → Fe2(SO4)3 + 2H2O + MnSO4 9Cl2 + 12AlBr3 → 4Al3 + 18ClBr2 H2SO4 + C12H22O11 → 12C + H2SO4.11H2O CH4 + 2O2 → 2H2O + CO2 H2O + K2O → 2KOH 2Al + 3CuCl2 → 2AlCl3 + 3Cu 2H2O + 2NH3 + CuCl2 → Cu(OH)2 + 2NH4Cl 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 H2O + CH3COCl → CH3COOH + HCl CH3Br + KCN → KBr + CH3CN 2Cl2 + CH2Cl2 → HCl + CHCl3 Cu(NO3)2 + Zn → Cu + Zn(NO3)2 C6H5NH3Cl + NaOH → C6H5NH2 + H2O + NaCl 2HCl + Mg → H2 + MgCl2 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.

3C2H5OH + PCl3 → H3PO3 + 3C2H5Cl Mg + 2KHSO4 → H2 + K2SO4 + MgSO4 3Cu(OH)2 + 2Fe(NO3)3 → 3Cu(NO3)2 + 2Fe(OH)3 H2O + KCl + CO2 → KHCO3 + HClO 2HNO3 + K2CO3 → H2O + 2KNO3 + CO2 K2S + ZnSO4 → ZnS + K2SO4 H2S + KOH → H2O + KSH View All Double-replacement reaction
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