Question

complete the balanced molecular chemical equation for the reaction below.
k₂so₄(aq) + fecl₃(aq) →
if no reaction occurs, write nr after the reaction arrow. be sure to include the proper phases for all species within the reaction.

Explanation:

Step1: Predict products

When \(K_2SO_4(aq)\) reacts with \(FeCl_3(aq)\), the potential products are \(Fe_2(SO_4)_3\) and \(KCl\) by double - displacement (exchange of cations and anions). The general form of double - displacement reaction is \(AB + CD
ightarrow AD+CB\), where \(A = K^+\), \(B=SO_4^{2 -}\), \(C = Fe^{3+}\), \(D = Cl^-\).

Step2: Check solubility

According to solubility rules:

• Salts containing \(K^+\) (Group 1 cations) and \(Cl^-\) are soluble. So \(KCl\) is soluble (\(KCl(aq)\)).
• For \(Fe_2(SO_4)_3\), sulfates (\(SO_4^{2 -}\)) are generally soluble, and there is no rule that makes \(Fe_2(SO_4)_3\) insoluble. So \(Fe_2(SO_4)_3(aq)\) is formed.

Since all products (\(Fe_2(SO_4)_3(aq)\) and \(KCl(aq)\)) are soluble (aqueous), no precipitate, gas or weak - electrolyte (like water in acid - base reactions) is formed.

Answer:

\(K_2SO_4(aq)+FeCl_3(aq)
ightarrow NR\)