Author Question: Consider the following standard reduction potentials: Ni2+(aq) + 2 e- Ni(s) E = -0.26 V I2(s) + 2 e- ... (Read 66 times)

HCHenry · **on:** Jul 8, 2021

Question 1

Consider the following reaction:

2 Al(s) + 3 Ni²⁺(aq) → 2 Al³⁺(aq) + 3 Ni(s) E° = 1.410 V

What would be the cell potential at 25 °C as calculated from the Nernst equation if [Ni²⁺] = 0.020 M, [Al³⁺] = 3.60 M?
◦ 1.388 volts
◦ 1.034 volts
◦ 1.471 volts
◦ 1.349 volts
◦ 1.410 volts

Question 2

Consider the following standard reduction potentials:

Ni^²+(aq) + 2 e^-→ Ni(s) E° = -0.26 V
I₂(s) + 2 e^-→ 2 I^-(aq) E° = +0.54 V

Under standard conditions:
◦ Ni^²+(aq) is a stronger oxidizing agent than I₂(s), and I^-(aq) is a stronger reducing agent than Ni(s)
◦ I₂(s) is a stronger oxidizing agent than Ni^²+(aq), and Ni(s) is a stronger reducing agent than I^-(aq)
◦ Ni(s) is a stronger oxidizing agent than I^-(aq), and Ni^²+(aq) is a stronger reducing agent than I₂(s)
◦ I^-(aq) is a stronger oxidizing agent than Ni(s), and I₂(s) is a stronger reducing agent than Ni^²+(aq)

dudman123 · **Reply #1 on:** Jul 8, 2021

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