13. Classify each of the following reactions as a synthesis reaction, a decomposition reaction, a single-displacement reaction, a double- displacement reaction, or a combustion reaction: a. \( \mathrm{N}_{2}+3 \mathrm{H}_{2} \rightarrow 2 \mathrm{NH}_{3} \) b. \( \mathrm{Li}+2 \mathrm{H}_{2} \mathrm{O} \rightarrow 2 \mathrm{LiOH}+\mathrm{H}_{2} \) c. \( 2 \mathrm{NaNO}_{3} \rightarrow 2 \mathrm{NaNO}_{2}+\mathrm{O}_{2} \) d. \( 2 \mathrm{C}_{6} \mathrm{H}_{41}+19 \mathrm{O}_{2} \rightarrow 12 \mathrm{CO}_{2}+14 \mathrm{H}_{2} \mathrm{O} \) e. \( \mathrm{NH}_{4} \mathrm{Cl} \rightarrow \mathrm{NH}_{3}+\mathrm{HCl} \) f. \( \mathrm{BaO}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{Ba}(\mathrm{OH})_{2} \) g. \( \mathrm{AgNO}_{3}+\mathrm{NaCl} \rightarrow \mathrm{AgCl}+\mathrm{NaNO}_{3} \)

Sure, let's classify each of the given chemical reactions based on their types: ### a. \( \mathrm{N}_2 + 3 \mathrm{H}_2 \rightarrow 2 \mathrm{NH}_3 \) **Type:** **Synthesis Reaction** **Explanation:** This reaction involves two reactants (\(\mathrm{N}_2\) and \(\mathrm{H}_2\)) combining to form a single product (\(\mathrm{NH}_3\)). Synthesis reactions typically involve the combination of simpler substances to form a more complex compound. --- ### b. \( \mathrm{Li} + 2 \mathrm{H}_2\mathrm{O} \rightarrow 2 \mathrm{LiOH} + \mathrm{H}_2 \) **Type:** **Single-Displacement Reaction** **Explanation:** In this reaction, lithium (\(\mathrm{Li}\)) displaces hydrogen from water (\(\mathrm{H}_2\mathrm{O}\)) to form lithium hydroxide (\(\mathrm{LiOH}\)) and hydrogen gas (\(\mathrm{H}_2\)). Single-displacement reactions involve an element reacting with a compound, where one element replaces another in the compound. --- ### c. \( 2 \mathrm{NaNO}_3 \rightarrow 2 \mathrm{NaNO}_2 + \mathrm{O}_2 \) **Type:** **Decomposition Reaction** **Explanation:** Sodium nitrate (\(\mathrm{NaNO}_3\)) breaks down into sodium nitrite (\(\mathrm{NaNO}_2\)) and oxygen gas (\(\mathrm{O}_2\)). Decomposition reactions involve a single compound breaking down into two or more simpler substances. --- ### d. \( 2 \mathrm{C}_6\mathrm{H}_{14} + 19 \mathrm{O}_2 \rightarrow 12 \mathrm{CO}_2 + 14 \mathrm{H}_2\mathrm{O} \) **Type:** **Combustion Reaction** **Explanation:** This reaction involves a hydrocarbon (\(\mathrm{C}_6\mathrm{H}_{14}\)) reacting with oxygen (\(\mathrm{O}_2\)) to produce carbon dioxide (\(\mathrm{CO}_2\)) and water (\(\mathrm{H}_2\mathrm{O}\)). Combustion reactions typically involve organic compounds reacting with oxygen to produce carbon dioxide and water, often releasing energy in the form of heat and light. --- ### e. \( \mathrm{NH}_4\mathrm{Cl} \rightarrow \mathrm{NH}_3 + \mathrm{HCl} \) **Type:** **Decomposition Reaction** **Explanation:** Ammonium chloride (\(\mathrm{NH}_4\mathrm{Cl}\)) decomposes into ammonia (\(\mathrm{NH}_3\)) and hydrogen chloride (\(\mathrm{HCl}\)). This is a classic example of a decomposition reaction where a single compound breaks down into multiple products. --- ### f. \( \mathrm{BaO} + \mathrm{H}_2\mathrm{O} \rightarrow \mathrm{Ba(OH)}_2 \) **Type:** **Synthesis Reaction** **Explanation:** Barium oxide (\(\mathrm{BaO}\)) reacts with water (\(\mathrm{H}_2\mathrm{O}\)) to form barium hydroxide (\(\mathrm{Ba(OH)}_2\)). This is a synthesis reaction where two reactants combine to form a single, more complex product. --- ### g. \( \mathrm{AgNO}_3 + \mathrm{NaCl} \rightarrow \mathrm{AgCl} + \mathrm{NaNO}_3 \) **Type:** **Double-Displacement Reaction** **Explanation:** Silver nitrate (\(\mathrm{AgNO}_3\)) and sodium chloride (\(\mathrm{NaCl}\)) exchange their ions to form silver chloride (\(\mathrm{AgCl}\)) and sodium nitrate (\(\mathrm{NaNO}_3\)). Double-displacement reactions involve the exchange of ions between two compounds to form two new compounds. --- ### **Summary:** | **Reaction** | **Type** | |-------------------------------------------------------|----------------------------| | a. \( \mathrm{N}_2 + 3 \mathrm{H}_2 \rightarrow 2 \mathrm{NH}_3 \) | Synthesis Reaction | | b. \( \mathrm{Li} + 2 \mathrm{H}_2\mathrm{O} \rightarrow 2 \mathrm{LiOH} + \mathrm{H}_2 \) | Single-Displacement Reaction | | c. \( 2 \mathrm{NaNO}_3 \rightarrow 2 \mathrm{NaNO}_2 + \mathrm{O}_2 \) | Decomposition Reaction | | d. \( 2 \mathrm{C}_6\mathrm{H}_{14} + 19 \mathrm{O}_2 \rightarrow 12 \mathrm{CO}_2 + 14 \mathrm{H}_2\mathrm{O} \) | Combustion Reaction | | e. \( \mathrm{NH}_4\mathrm{Cl} \rightarrow \mathrm{NH}_3 + \mathrm{HCl} \) | Decomposition Reaction | | f. \( \mathrm{BaO} + \mathrm{H}_2\mathrm{O} \rightarrow \mathrm{Ba(OH)}_2 \) | Synthesis Reaction | | g. \( \mathrm{AgNO}_3 + \mathrm{NaCl} \rightarrow \mathrm{AgCl} + \mathrm{NaNO}_3 \) | Double-Displacement Reaction | If you have any further questions or need additional explanations, feel free to ask!