Use the following standard reduction potentials to determine which species is the best oxidizing agent. O₂(g) + 4 H⁺(aq) + 4 e^- → 2 H₂O( )
E° = +1.229 V
Hg₂²⁺(aq) + 2 e^- → 2 Hg( )
E° = +0.789 V
I₂(s) + 2 e^- → 2 I^-(aq)
E° = +0.535 V

Question

Use the following standard reduction potentials to determine which species is the best oxidizing agent. O₂(g) + 4 H⁺(aq) + 4 e^- → 2 H₂O(

)
E° = +1.229 V
Hg₂²⁺(aq) + 2 e^- → 2 Hg(

)
E° = +0.789 V
I₂(s) + 2 e^- → 2 I^-(aq)
E° = +0.535 V

Quizplus · Accepted Answer

The species with the highest E° value is the best oxidizing agent. Therefore, the best choice is O₂(g) with an E° value of +1.229 V.

Use the Following Standard Reduction Potentials to Determine Which Species