Use the following standard reduction potentials to determine which species is the strongest oxidizing agent.
Fe²⁺(aq) + 2 e^- ? Fe(s) ; E° = -0.41 V
Pt²⁺(aq) + 2 e^- ? Pt(s) ; E° = 1.18 V
Cr₂O₇^2-(aq) + 14 H⁺(aq) + 6 e^- ? 2 Cr³⁺(aq) + 7 H₂O( $\ell$ ) ; E° = 1.33 V

Question

Use the following standard reduction potentials to determine which species is the strongest oxidizing agent.
Fe²⁺(aq) + 2 e^- ? Fe(s) ; E° = -0.41 V
Pt²⁺(aq) + 2 e^- ? Pt(s) ; E° = 1.18 V
Cr₂O₇^2-(aq) + 14 H⁺(aq) + 6 e^- ? 2 Cr³⁺(aq) + 7 H₂O(

\ell

) ; E° = 1.33 V

Quizplus · Accepted Answer

The Answer of Use the following standard reduction potentials to determine which species is the strongest oxidizing agent. Fe²⁺(aq) + 2 e^- ? Fe(s); E° = -0.41 V Pt²⁺(aq) + 2 e^- ? Pt(s); E° = 1.18 V Cr₂O₇^2-(aq) + 14 H⁺(aq) + 6 e^- ? 2 Cr³⁺(aq) + 7 H₂O( $\ell$ ); E° = 1.33 V

Use the Following Standard Reduction Potentials to Determine Which Species ℓ\ellℓ

Use the Following Standard Reduction Potentials to Determine Which Species $\ell$