No redox reaction between Br₂ and Cl⁻

Steps:

• Recall standard electrode potentials: E°(Cl₂/Cl⁻) = +1.36 V > E°(Br₂/Br⁻) = +1.07 V.
• Determine oxidizing strength: Cl₂ is stronger oxidant than Br₂, so Br₂ cannot oxidize Cl⁻ to Cl₂.
• Check for displacement: No reaction as Br₂ is weaker halogen, cannot displace Cl⁻ from NaCl(aq).
• Conclude: Mixture remains unchanged, no electron transfer.

Why C is correct:

• Redox requires electron transfer; here, electrode potentials show no spontaneous reaction per Nernst equation.

Why the others are wrong:

• A: Cl⁻ cannot oxidize Br₂ as Cl⁻ is weaker reducing agent.
• B: Br₂ cannot oxidize Cl⁻ due to lower reduction potential.
• D: Na⁺ is spectator ion, not involved in redox.

Final answer: C