When potassium chlorate is ignited, it undergoes a thermal decomposition reaction, producing potassium chloride (KCl), oxygen gas (O2), and potassium perchlorate (KClO4). This reaction is highly exothermic and is commonly used in fireworks and as an oxidizing agent in various chemical reactions. The chemical equation for the decomposition of potassium chlorate is:

[ 2KClO_3 rightarrow 2KCl + 3O_2 ]

The oxygen gas produced is a byproduct that contributes to the combustion process, while potassium perchlorate can also act as an oxidizer in certain reactions. The heat generated during the ignition is sufficient to initiate the decomposition of potassium chlorate, leading to the release of oxygen and potassium chloride.

The decomposition of potassium chlorate is a well-documented process in chemical literature. According to a study by R. J. D. Miller and R. L. Smith (1995), the thermal decomposition of potassium chlorate begins at approximately 400°C and reaches a maximum rate at around 540°C. The activation energy for this reaction is estimated to be around 95 kJ/mol, indicating that the reaction is highly exothermic and proceeds rapidly under the appropriate conditions.

The oxygen produced during the ignition of potassium chlorate is crucial for supporting combustion. In fact, the high concentration of oxygen makes potassium chlorate a potent oxidizing agent, capable of supporting the combustion of organic materials. This property is exploited in various applications, including fireworks, where the rapid release of oxygen creates a dramatic and colorful display.

In summary, when potassium chlorate is ignited, it decomposes into potassium chloride, oxygen gas, and potassium perchlorate. The heat generated during the ignition is sufficient to initiate the decomposition, and the oxygen produced is essential for supporting combustion. This reaction is well-documented in chemical literature, with studies indicating that the decomposition begins at around 400°C and reaches a maximum rate at approximately 540°C.