Examine the following half-reactions and select the weakest oxidizing agent among the species listed.
AuBr₄^-(aq) + 3e^-
Au(s) + 4Br^-(aq) ;E° = 0.854 V
Mn²⁺(aq) + 2e^-
Mn(s) ;E° = -1.185 V
K⁺(aq) + e^-
K(s) ;E° = -2.931 V
F₂O(aq) + 2H⁺(aq) + 4e^-
2F^-(aq) + H₂O(l) ;E° = 2.153 V

Question

Examine the following half-reactions and select the weakest oxidizing agent among the species listed.
AuBr₄^-(aq) + 3e^-

Examine the following half-reactions and select the weakest oxidizing agent among the species listed. AuBr<sub>4</sub><sup>-</sup>(aq) + 3e<sup>-</sup> Au(s) + 4Br<sup>-</sup>(aq) ;E° = 0.854 V Mn<sup>2+</sup>(aq) + 2e<sup>-</sup> Mn(s) ;E° = -1.185 V K<sup>+</sup>(aq) + e<sup>-</sup> K(s) ;E° = -2.931 V F<sub>2</sub>O(aq) + 2H<sup>+</sup>(aq) + 4e<sup>-</sup> 2F<sup>-</sup>(aq) + H<sub>2</sub>O(l) ;E° = 2.153 V A) AuBr<sub>4</sub><sup>-</sup>(aq) B) Mn<sup>2+</sup>(aq) C) K<sup>+</sup>(aq) D) F<sub>2</sub>O(aq) E) H<sup>+</sup>(aq)

Au(s) + 4Br^-(aq) ;E° = 0.854 V
Mn²⁺(aq) + 2e^-

Mn(s) ;E° = -1.185 V
K⁺(aq) + e^-

K(s) ;E° = -2.931 V
F₂O(aq) + 2H⁺(aq) + 4e^-

2F^-(aq) + H₂O(l) ;E° = 2.153 V

Quizplus · Accepted Answer

The weakest oxidizing agent has the smallest positive reduction potential (or largest negative oxidation potential) among the species listed. From the given half-reactions, we can see that K has the most negative E° value of -2.931 V, indicating that it has the least tendency to accept electrons and act as an oxidizing agent. Therefore, choice C, K⁺(aq), is the weakest oxidizing agent among the species listed.

Examine the Following Half-Reactions and Select the Weakest Oxidizing Agent