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A decomposition reaction is a type of chemical reaction in which a single compound breaks down into two or more simpler compounds. These types of reactions involve the breakdown of chemical bonds in the compound, resulting in the formation of new compounds.

An example of a decomposition reaction is the breakdown of hydrogen peroxide (H2O2) into water (H2O) and oxygen (O2). In this reaction, hydrogen peroxide, acting as a single compound, decomposes into two simpler compounds, water and oxygen gas. The chemical equation for this reaction is: \[ 2H_2O_2 \rightarrow 2H_2O + O_2 \]

Decomposition reactions can also be classified in other ways based on the types of products formed or the conditions under which the reaction occurs. Some common types of decomposition reactions include: 1. Thermal decomposition: The reaction occurs when heat is applied to the compound, causing it to break down. An example is the decomposition of calcium carbonate (\(CaCO_3\)) into calcium oxide (\(CaO\)) and carbon dioxide (\(CO_2\)) when heated. 2. Photodecomposition: The reaction occurs when the compound is exposed to light energy, which breaks its chemical bonds. An example is the decomposition of silver chloride (\(AgCl\)) into silver (\(Ag\)) and chlorine (\(Cl_2\)) when exposed to sunlight. 3. Electrolytic decomposition: The reaction occurs when an electric current is passed through the compound, causing it to break down. An example is the electrolysis of water (H2O) into hydrogen (H2) and oxygen (O2) gases. In conclusion, decomposition reactions are those in which a single compound breaks down into two or more simpler compounds. They can be further classified based on the types of products formed or the conditions that trigger the reaction, such as heat, light, or electricity.