Redox Processes in the Reaction

Steps:

• Oxidation state of Fe changes from +2 in Fe²⁺ to +3 in Fe³⁺, indicating oxidation (loss of electron).
• Oxidation state of Cl changes from 0 in Cl₂ to -1 in 2Cl⁻, indicating reduction (gain of electrons).
• Fe²⁺ loses an electron to Cl₂, so Fe²⁺ is the reducing agent and Cl₂ is the oxidizing agent.
• Chlorine undergoes reduction caused by iron(II) ions.

Why A is correct:

• Reduction defined as gain of electrons; Cl₂ accepts an electron from Fe²⁺, reduced by the iron(II) reducing agent.

Why the others are wrong:

• B: Reducing agent is oxidized (loses electrons); Cl₂ is reduced, so it's the oxidizing agent.
• C: Fe²⁺ is oxidized, but the statement reverses roles—Cl₂ oxidizes Fe²⁺, not vice versa.
• D: Oxidizing agent is reduced (gains electrons); Fe²⁺ is oxidized, so it's the reducing agent.

Final answer: A