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

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

Step-by-step 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+ )`.