? = [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.

BaO + H2O → Ba(OH)2 CaO + H2O → Ca(OH)2 Br2 + H2 → 2HBr SnCl4 + Sn → 2SnCl2 C2H2 + CO + H2O → C2H3COOH 5Cl2 + 2P → 2PCl5 2H + NH2OH → NH4OH 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 2H2O + CaCl2 → Ca(OH)2 + Cl2 + 2H2 2KClO3 → 2KCl + 3O2 CaCO3 → CaO + CO2 C2H6 → C2H4 + H2 2CH4 → C2H2 + 2H2 C6H12O6 → 2C2H5OH + 2CO2 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.

3H2SO4 + 2B → 3SO2 + 2H3BO3 H2O + HPO3 → H3PO4 4Cl2 + 4H2O + H2S → H2SO4 + 8HCl (NH4)2SO4 + 2NaNO3 → 4H2O + Na2SO4 + 2N2O 2HClO4 → H2O + Cl2O7 FeCl2 + 4HNO3 → H2O + 2HCl + NO2 + Fe(NO3)3 CO + Fe3O4 → 3FeO + CO2 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).

C6H5NH3Cl + NaOH → C6H5NH2 + H2O + NaCl 2HNO3 + Ni → H2 + Ni(NO3)2 C2H2 + 2Na → H2 + Na2C2 Zn + CuSO4 → Cu + ZnSO4 C6H5Cl + 2NaOH → C6H5ONa + H2O + NaCl CH3Cl + Cl2 → HCl + CH2Cl2 2Na + C6H5Br + CH3Br → C6H5CH3 + 2NaBr 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.

Fe2O3 + 3H2SO4 → Fe2(SO4)3 + 3H2O 2H2SO4 + ZnS → 2H2S + ZnSO4 2HCl + Fe(OH)2 → FeCl2 + 2H2O CaCO3 + 2HNO3 → Ca(NO3)2 + H2O + CO2 FeO + H2SO4 → H2O + FeSO4 FeBr3 + 3Ag(NO3) → 3AgBr + Fe(NO3)3 2HCl + Na2CO3 → H2O + 2NaCl + CO2 View All Double-replacement reaction

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