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

Cl2 and Br−. The most powerful oxidizing agent is Cl2 because it has the highest standard reduction potential, indicating it can easily gain electrons. Conversely, the most powerful reducing agent is Br−, as it has the lowest reduction potential, meaning it is more likely to lose electrons.

Solution

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