Question

Which one of the following reactions is not feasible?

• A. \( Cl_2(g) + 2KBr(aq) \longrightarrow 2KCl(aq) + Br_2(l) \)
• B. \( Cl_2(g) + 2KI(aq) \longrightarrow 2KCl(aq) + I_2(s) \)
• C. \( Br_2(l) + 2KI(aq) \longrightarrow 2KBr(aq) + I_2(s) \)
• D. \( I_2(s) + 2KBr(aq) \longrightarrow 2KI(aq) + Br_2(l) \)

Hint:

For displacement reactions involving halogens, higher halogens oxidize lower ones, but lower halogens cannot oxidize higher ones.

Answer 1

The Correct Option is D

Step 1: Understanding Feasibility Feasibility depends on oxidation strength: - Chlorine is the strongest oxidizing agent, capable of replacing bromine and iodine. - Bromine is weaker, but can replace iodine. - Iodine is the weakest and cannot oxidize bromide ions. Step 2: Evaluating the Reactions - (A) \( Cl_2 + 2KBr \rightarrow 2KCl + Br_2 \): - Feasible (Chlorine displaces bromine). - (B) \( Cl_2 + 2KI \rightarrow 2KCl + I_2 \): - Feasible (Chlorine displaces iodine). - (C) \( Br_2 + 2KI \rightarrow 2KBr + I_2 \): - Feasible (Bromine displaces iodine). - (D) \( I_2 + 2KBr \rightarrow 2KI + Br_2 \): - Not feasible (Iodine cannot displace bromine). Conclusion Thus, the correct answer is: \[ I_2(s) + 2KBr(aq) \longrightarrow 2KI(aq) + Br_2(l) \]