The standard reduction potentials for the following half-reactions are listed 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
From these, identify the most powerful oxidizing agent an

Question

The standard reduction potentials for the following half-reactions are listed 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
From these, identify the most powerful oxidizing agent and the most powerful reducing agent, respectively.

Accepted Answer

F2 and I−. F2 has the highest reduction potential (+2.85 V) so it is the strongest oxidising agent, and I- (from the lowest-E couple) is the strongest reducing agent. The pair is F2 and I-, not Cl2 and Br-.

Solution

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