To determine the type of chemical reaction for the equation [tex]\(2 \text{KClO}_3 \rightarrow 2 \text{KCl} + 3 \text{O}_2\)[/tex], we need to analyze the process and the nature of the reactants and products.
1. Identify the reactants and products:
- The reactant is [tex]\( \text{KClO}_3 \)[/tex] (potassium chlorate).
- The products are [tex]\( \text{KCl} \)[/tex] (potassium chloride) and [tex]\( \text{O}_2 \)[/tex] (oxygen gas).
2. Understand the reaction process:
- [tex]\( \text{KClO}_3 \)[/tex] decomposes into [tex]\( \text{KCl} \)[/tex] and [tex]\( \text{O}_2 \)[/tex].
- This means one compound ([tex]\(\text{KClO}_3\)[/tex]) breaks down into two or more simpler substances ([tex]\(\text{KCl}\)[/tex] and [tex]\( \text{O}_2 \)[/tex]).
3. Classify the reaction type:
- In a synthesis reaction, two or more simpler substances combine to form a more complex compound. This is not the case here.
- In a decomposition reaction, a single compound breaks down into two or more simpler substances, which fits our reaction.
- In a single replacement reaction, an element in a compound is replaced by another element. This is not happening here.
- In a double replacement reaction, ions in two compounds exchange places to form two new compounds. This is not happening here.
Given the analysis, the reaction is best described as a decomposition reaction because the compound [tex]\( \text{KClO}_3 \)[/tex] is breaking down into the simpler substances [tex]\( \text{KCl} \)[/tex] and [tex]\( \text{O}_2 \)[/tex].
Final answer: decomposition.
