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,

Question

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,

Quizplus · Accepted Answer

The greater the reduction potential, the stronger the oxidizing agent; and the smaller the reduction potential, the stronger the reducing agent. From the given reduction potentials, we can see that I₂(s) has a higher reduction potential (+0.54 V) than Ni²⁺(aq) (-0.26 V), which means that I₂(s) is a stronger oxidizing agent than Ni²⁺(aq). Similarly, I^-(aq) has a lower reduction potential (-0.54 V) than Ni(s) (-0.26 V), which means that Ni(s) is a stronger reducing agent than I^-(aq).

Consider the Following Standard Reduction Potentials