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? = KOH.H2O | Chemical Equation Balancer

? = Potassium hydroxide monohydrate

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KOH.H2O

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Kali hidroxit monohidrat


Potassium hydroxide monohydrate


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.

C6H5OH + 4O2 → 3H2O + 6CO2 BaO + CO2 → BaCO3 2CO + O2 → 2CO2 2H2 + O2 → 2H2O C2H4 + H2O → C2H5OH H2 + S → H2S CaO + CO2 → CaCO3 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.

2CH4 → C2H2 + 2H2 C4H10 → C2H4 + C2H6 CaCl2 → Ca + Cl2 Cu(OH)2 → CuO + H2O (NH4)2Cr2O7 → 4H2O + N2 + Cr2O3 2Ag2O → 4Ag + O2 CH4 → C + 2H2 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.

3Cu + 8HCl + 8NaNO3 → 3Cu(NO3)2 + 4H2O + 8NaCl + NO 3Cl2 + 2Fe → 2FeCl3 2HCl + NaClO → Cl2 + H2O + NaCl Br2 + 2KI → I2 + 2KBr Al + 3Fe(NO3)3 → 3Fe(NO3)2 + Al(NO3)3 2O2 + Cu2S → 2CuO + SO2 2H2O + 5HNO3 + 3P → 5NO + 3H3PO4 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).

Mg + FeSO4 → Fe + MgSO4 Br2 + 2NaI → I2 + 2NaBr 2Ca(OH)2 + Mg(HCO3)2 → 2CaCO3 + 2H2O + Mg(OH)2 3Cl2 + 2NH3 → 6HCl + N2 CH3Br + KCN → KBr + CH3CN Cl2 + 2NaI → I2 + 2NaCl C2H2 + 2[Ag(NH3)2]OH → H2O + NH3 + C2Ag2 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.

Na3PO4 + Al(NO3)3 → NaNO3 + AlPO4 FeCl2 + Na2CO3 → FeCO3 + 2NaCl CaF2 + H2SO4 → CaSO4 + 2HF Ba(OH)2 + KHSO3 → H2O + K2SO3 + BaSO3 H2O + NaCl + NH3 + CO2 → NaHCO3 + NH4Cl 2NaOH + MgCl2 → Mg(OH)2 + 2NaCl 2NaOH + CrSO4 → Na2SO4 + Cr(OH)2 View All Double-replacement reaction
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Potassium hydroxide monohydrate

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