A decomposition reaction is a chemical reaction that breaks down a chemical compound. The reverse of a decomposition response is a combination reaction.
In each chemical reaction, the reactants are degraded and products formed. Therefore, the term decomposition reaction is usually used for reactions in which a single reactant forms multiple products. Energy effects
Many decomposition reactions are endothermic: it takes energy to allow them to expire. This can be seen by looking at the reaction mechanism of an analysis. What should be the first to start a decomposition? There is no need to wait until the reactants come together, as it is only a rearrangement of the atoms that are already within the molecule. If a decomposition reaction is exothermic, then it would be possible to proceed. The substance could spontaneously decompose, and can not be stored stable. The only rescue is the kinetics: the activation energy of the decomposition could be so high that under normal conditions no decomposition can occur. We could call the compound kinetic stable. However, the substance remains thermodynamically unstable: when such an exothermic decomposition commences accidentally or by environmental influences, the released energy is often sufficient to allow the neighboring molecules to decompose. A chain reaction takes place, which decomposes very quickly. In this case, especially when gaseous products arise, an explosion can occur. An example is the decomposition of dry picric acid: it can already start with a mechanical shock.
All thermodynamically stable chemical compounds therefore have endothermic decomposition reactions, and continuous energy must be supplied to allow them to flow. Power supply
The energy for the endothermic decomposition reaction can be applied in different ways. Depending on the type of power supply, the response gets a more specific name: Also see
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