? = [C6H7O2(OH)3]n | Chemical Equation Balancer

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short form C6H10NO5


Atomic_weight (g/mol) 176.1473

Density of solid (kg/m3) 1500

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.

H2O + ZnO → Zn(OH)2 5Cl2 + 2P → 2PCl5 H2O + N2O5 → 2HNO3 C2H2 + HCN → C2H3CN O2 + Se → SeO2 H2 + S → H2S 3Mg + 2P → Mg3P2 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.

C4H10 → CH3CH=CHCH3 + H2 NH4Cl → HCl + NH3 (NH4)2CO3 → H2O + 2NH3 + CO2 C6H12O6 → 2C2H5OH + 2CO2 3HClO3 → H2O + 2ClO2 + HClO4 CH4 → C + 2H2 Ag2S → 2Ag + S 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.

3Cl2 + CS2 → CCl4 + S2Cl2 Cl2 + 2KBr → Br2 + 2KCl H2O + 2NaOH + P2O5 → 2NaH2PO4 2Cu(NO3)2 → 2CuO + 4NO2 + O2 BaCl2 + K2CrO4 → KCl + BaCrO4 4Cl2 + 4H2O + H2S → H2SO4 + 8HCl NH4NO3 → 9H2O + 2HNO3 + 4N2 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 + 2NaI → I2 + 2NaBr H2SO4 + BaO2 → H2O2 + BaSO4 Cl2 + 2NaBr → Br2 + 2NaCl Fe + CuSO4 → Cu + FeSO4 3HNO3 + C6H5CH3 → 3H2O + C6H2CH3(NO2)3 2Al + 3CuCl2 → 2AlCl3 + 3Cu CH3Cl + Cl2 → HCl + CH2Cl2 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.

Na2SO4 + Pb(NO3)2 → 2NaNO3 + PbSO4 H2SO4 + Na2SO3 → H2O + Na2SO4 + SO2 AgNO3 + KCl → AgCl + KNO3 Fe2(CO3)3 + 3H2O → 3CO2 + 2Fe(OH)3 Al(OH)3 + 3HCl → AlCl3 + 3H2O H2SO4 + Na2SO3 → H2O + Na2SO4 + SO2 3H2SO4 + 2Al(NO3)3 → Al2(SO4)3 + 6HNO3 View All Double-replacement reaction

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