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,
A) Ni2+(aq) is a stronger oxidizing agent than I2(s) and I-(aq) is a stronger reducing agent thanNi(s).
B) I2(s) is a stronger oxidizing agent than Ni2+(aq) and Ni(s) is a stronger reducing agent thanI-(aq).
C) Ni(s) is a stronger oxidizing agent than I-(aq) and Ni2+(aq) is a stronger reducing agent thanI2(s).
D) I-(aq) is a stronger oxidizing agent than Ni(s) and I2(s) is a stronger reducing agent thanNi2+(aq).

Answer 1

Answer:

B) ${ I }_{ 2 }$(s) is a stronger oxidizing agent than  ${ Ni }^{ 2+ }$(aq) and Ni(s) is a stronger reducing agent than  ${ I }^{ - }$ (aq).

Explanation:

Oxidation is the loss of electrons in a chemical reaction while reduction is the gaining of electrons. The given equations both show a gain of electrons in the forward reaction, however to find the strongest reducing agent we should consider their reduction potentials. The most negative reduction potential indicates a strong reducing agent. In this scenario Ni(s) is a stronger reducing agent than  ${ I }^{ - }$ (aq) since it has a reduction potential of -0,26V . The most positive reduction potential indicates a strong oxidizing  agent so ${ I }_{ 2 }$(s) is a stronger oxidizing agent than  ${ Ni }^{ 2+ }$.