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The exothermic (heat producing) reaction between potassium permanganate (KMnO 4), a strong oxidizing agent, and glycerol (C 3 H 5 (OH) 3), a readily oxidised organic substance, is an example of an experiment sometimes referred to as a "chemical volcano". [7] [8]
The reagent is an alkaline solution of potassium permanganate. Reaction with double or triple bonds (R 2 C=CR 2 or R−C≡C−R) causes the color to fade from purplish-pink to brown. Aldehydes and formic acid (and formates) also give a positive test. [43] The test is antiquated. Baeyer's reagent reaction
Although this is a reaction solely of the dissociated ions in solution, it is sometimes referred to as a double displacement reaction: [1] Pb(NO 3) 2 + 2 KI → 2 KNO 3 + PbI 2. At higher temperature, this substance easily re-dissolves by dissociation to its colorless ions. The actual change (net ionic equation) is thus:
Potassium permanganate will decompose into potassium manganate, manganese dioxide and oxygen gas: 2 KMnO 4 → K 2 MnO 4 + MnO 2 + O 2. This reaction is a laboratory method to prepare oxygen, but produces samples of potassium manganate contaminated with MnO 2. The former is soluble and the latter is not.
In the following redox reaction, hazardous sodium metal reacts with toxic chlorine gas to form the ionic compound sodium chloride, or common table salt: + () In the reaction, sodium metal goes from an oxidation state of 0 (a pure element) to +1: in other words, the sodium lost one electron and is said to have been oxidized.
It is desirable that the temperature of the titration mixture be greater than 60 °C to ensure that all the permanganate added reacts quickly. The kinetics of the reaction are complex, and the manganese(II) ions (Mn 2+) formed catalyze the further reaction between permanganate and oxalic acid (formed in situ by the addition of excess sulfuric ...
Potassium nitrite (distinct from potassium nitrate) is the inorganic compound with the chemical formula K N O 2.It is an ionic salt of potassium ions K + and nitrite ions NO 2 −, which forms a white or slightly yellow, hygroscopic crystalline powder that is soluble in water.
Dynamical properties of reaction networks were studied in chemistry and physics after the invention of the law of mass action.The essential steps in this study were introduction of detailed balance for the complex chemical reactions by Rudolf Wegscheider (1901), [1] development of the quantitative theory of chemical chain reactions by Nikolay Semyonov (1934), [2] development of kinetics of ...