Q. Standard reduction potentials of the half reactions are given below: F₂(g) + 2e⁻ → 2F⁻(aq); E° = +2.85 V Cl₂(g) + 2e⁻ → 2Cl⁻(aq); E° = +1.36 V Br₂(l) + 2e⁻ → 2Br⁻(aq); E° = +1.06 V I₂(s) + 2e⁻ → 2I⁻(aq); E° = +0.53 V The strongest oxidising and reducing agents respectively are
A) F₂ and I⁻
B) Br₂ and Cl⁻
C) Cl₂ and Br⁻
D) Cl₂ and I₂
Explanation
[Solution from source] The highest reduction potential (F₂, +2.85 V) marks the strongest oxidising agent. The lowest reduction potential (I₂/I⁻, +0.53 V) means I⁻ is most easily oxidised, so I⁻ is the strongest reducing agent; I₂ itself is an oxidant, not a reductant. Answer (1).
Reviewed by Dr. Abubacker
Physics Educator & NEET/JEE Specialist
Ph.D. in Physics with 19+ years of teaching experience.