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Chemical decomposition, or chemical breakdown, is the process or effect of simplifying a single chemical entity (normal molecule, reaction intermediate, etc.) into two or more fragments. [1] Chemical decomposition is usually regarded and defined as the exact opposite of chemical synthesis .
Classically, these reactions result in the precipitation of one product. In older literature, the term double decomposition is common. The term double decomposition is more specifically used when at least one of the substances does not dissolve in the solvent , as the ligand or ion exchange takes place in the solid state of the reactant.
Azides decompose with nitrite compounds such as sodium nitrite. Each elementary redox reaction is also a comproportionation reaction because two different N-species (N − 3 and NO − 2) converge to a same one (respectively N 2, N 2 O and NO) and is favored when the solution is acidified.
The reaction is used to make quick lime, which is an industrially important product. Another example of thermal decomposition is 2Pb(NO 3 ) 2 → 2PbO + O 2 + 4NO 2 . Some oxides , especially of weakly electropositive metals decompose when heated to high enough temperature.
Comment: there are two versions of this decomposition: complex and real. Decomposition (complex version): A = Q S Z ∗ {\displaystyle A=QSZ^{*}} and B = Q T Z ∗ {\displaystyle B=QTZ^{*}} where Q and Z are unitary matrices , the * superscript represents conjugate transpose , and S and T are upper triangular matrices.
The divide-and-conquer paradigm is often used to find an optimal solution of a problem. Its basic idea is to decompose a given problem into two or more similar, but simpler, subproblems, to solve them in turn, and to compose their solutions to solve the given problem. Problems of sufficient simplicity are solved directly.
1. Add to Grains. Turn yesterday’s soup into today’s healthy bowl. Start with a base of grains like rice, farro, or quinoa. Add roasted veggies and a protein.
The reaction can be demonstrated by starting with solutions of potassium cyanate and ammonium chloride which are mixed, heated and cooled again. An additional proof of the chemical transformation is obtained by adding a solution of oxalic acid which forms urea oxalate as a white precipitate. [3]