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? = HONO2 | Chemical Equation Balancer

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Searching in our database with more than 5552 chemical substances

HONO2

short form HNO3



axit nitric




Atomic_weight (g/mol) 63.0128

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 5O2 + 4P → 2P2O5 HCl + NH3 → NH4Cl CaO + CO2 → CaCO3 2H + NH2OH → NH4OH C2H2 + CH3OH → CH3OCHCH2 Fe + S → FeS 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.

(NH4)2Cr2O7 → 4H2O + N2 + Cr2O3 2AgNO3 → 2Ag + 2NO2 + O2 2HI → H2 + I2 NH4Cl → HCl + NH3 C4H10 → CH3CH=CHCH3 + H2 C6H12O6 → 2C2H5OH + 2CO2 5O2 + C4H6Cl2 → 2H2O + 2HCl + 4CO2 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.

2NH4NO3 → 4H2O + 2N2 + O2 2Al + 3FeCl2 → 2AlCl3 + 3Fe 2NH3 → 3H2 + N2 3O2 → 2O3 5KClO3 + 6P → 5KCl + 3P2O5 4HCl + O2 → 2Cl2 + 2H2O NaNO2 + NH4Cl → 2H2O + N2 + NaCl 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).

Br2 + C2H6 → C2H5Br + HBr 2Na + 2NH3 → H2 + 2NaNH2 2HNO3 + Ni → H2 + Ni(NO3)2 4Al + 3SiO2 → 2Al2O3 + 3Si H2SO4 + Na2O2 → H2O2 + Na2SO4 C2H5OH + HBr → H2O + C2H5Br Fe + H2SO4 → H2 + FeSO4 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.

Fe2O3 + 3H2SO4 → Fe2(SO4)3 + 3H2O 3AgNO3 + Na3PO4 → 3NaNO3 + Ag3PO4 Cu(OH)2 + 2HNO3 → Cu(NO3)2 + 2H2O 2HCl + Mg(HCO3)2 → H2O + MgCl2 + 2CO2 4KOH + Al(NO3)3 → 2H2O + 3KNO3 + KAlO2 BaCl2 + FeSO4 → FeCl2 + BaSO4 2NaOH + NH4HSO4 → 2H2O + Na2SO4 + NH3 View All Double-replacement reaction
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