Consider the following standard reduction potentials: Ni²⁺(aq)+ 2 e^- → Ni(s)E° = -0.26 V I₂(s)+ 2 e^- → 2 I^-(aq)E° = +0.54 V Under standard conditions: A)Ni²⁺(aq)is a stronger oxidizing agent than I₂(s),and I^-(aq)is a stronger reducing agent than Ni(s) B)I₂(s)is a stronger oxidizing agent than Ni²⁺(aq),and Ni(s)is a stronger reducing agent than I^-(aq) C)Ni(s)is a stronger oxidizing agent than I^-(aq),and Ni²⁺(aq)is a stronger reducing agent than I₂(s) D)I^-(aq)is a stronger oxidizing agent than Ni(s),and I₂(s)is a stronger reducing agent than Ni²⁺(aq)

Question

Quizplus · Accepted Answer

The standard reduction potential is a measure of the tendency of a species to be reduced. The more positive the reduction potential, the stronger the oxidizing agent. Conversely, the more negative the reduction potential, the stronger the reducing agent. In this case, I₂(s) has a more positive reduction potential (+0.54 V) than Ni²⁺(aq) (-0.26 V), meaning that it is a stronger oxidizing agent than Ni²⁺(aq). Meanwhile, Ni(s) has a more negative reduction potential (-0.26 V) than I^-(aq) (0.00 V), meaning that it is a stronger reducing agent than I^-(aq). Therefore, option B is the best choice.

Consider the Following Standard Reduction Potentials