Question

identify the type of reaction for each of the following. note: phases of reactants are given. phases of products may need to be determined to identify the type of reaction.
k₂s(aq) + cacl₂(aq) → 2 kcl + cas --
cl₂(aq) + 2 nabr(aq) → 2 nacl + br₂ --
h₂so₄(aq) + 2 lioh(aq) → li₂so₄ + 2 h₂o --

Explanation:

Step1: Analyze the first reaction

In \(K_{2}S(aq)+CaCl_{2}(aq)\to 2KCl + CaS\), the cations (\(K^{+}\) and \(Ca^{2+}\)) exchange anions (\(S^{2 -}\) and \(Cl^{-}\)). This is a double - displacement reaction.

Step2: Analyze the second reaction

In \(Cl_{2}(aq)+2NaBr(aq)\to 2NaCl + Br_{2}\), \(Cl_{2}\) (a more reactive non - metal) displaces \(Br^{-}\) from \(NaBr\). This is a single - displacement reaction.

Step3: Analyze the third reaction

In \(H_{2}SO_{4}(aq)+2LiOH(aq)\to Li_{2}SO_{4}+2H_{2}O\), \(H_{2}SO_{4}\) (an acid) reacts with \(LiOH\) (a base) to form a salt (\(Li_{2}SO_{4}\)) and water (\(H_{2}O\)). This is an acid - base (neutralization) reaction.

Answer:

1. Double - displacement reaction
2. Single - displacement reaction
3. Acid - base (neutralization) reaction