Classify each of the following reactions as decomposition (D), combination \( (\mathrm{C}) \), single-replacement (SR), or double- replacement \( (\mathrm{DR}): \) a. \( 2 \mathrm{KClO}_{3}(s) \xrightarrow{\Delta} 2 \mathrm{KCl}(s)+3 \mathrm{O}_{2}(g) \)

The reaction \( 2 \mathrm{KClO}_{3}(s) \xrightarrow{\Delta} 2 \mathrm{KCl}(s)+3 \mathrm{O}_{2}(g) \) is classified as a decomposition reaction (D). In this reaction, potassium chlorate (\( \mathrm{KClO}_{3} \)) breaks down into potassium chloride (\( \mathrm{KCl} \)) and oxygen gas (\( \mathrm{O}_{2} \)), which is a hallmark of decomposition processes. Decomposition reactions often require energy input, such as heat, which is indicated by the \( \Delta \) symbol (Δ) in this case. This process highlights the fascinating nature of chemical compounds breaking apart to form simpler substances, much like a magician revealing hidden treasures!