5.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, I2(s) is a stronger oxidizing agent than Ni2+(aq), and Ni(s) is a stronger reducing agent than I-(aq). Ni(s) is a stronger oxidizing agent than I-(aq), and Ni2+(aq) is a stronger reducing agent than I2(s). Ni2+(aq) is a stronger oxidizing agent than I2(s), and I-(aq) is a stronger reducing agent than Ni(s). I-(aq) is a stronger oxidizing agent than Ni(s), and I2(s) is a stronger reducing agent than Ni2+(aq).
5.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, I2(s) is a stronger oxidizing agent than Ni2+(aq), and Ni(s) is a stronger reducing agent than I-(aq). Ni(s) is a stronger oxidizing agent than I-(aq), and Ni2+(aq) is a stronger reducing agent than I2(s). Ni2+(aq) is a stronger oxidizing agent than I2(s), and I-(aq) is a stronger reducing agent than Ni(s). I-(aq) is a stronger oxidizing agent than Ni(s), and I2(s) is a stronger reducing agent than Ni2+(aq).
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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5.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,
I2(s) is a stronger oxidizing agent than Ni2+(aq), and Ni(s) is a stronger reducing agent than I-(aq). |
Ni(s) is a stronger oxidizing agent than I-(aq), and Ni2+(aq) is a stronger reducing agent than I2(s). |
Ni2+(aq) is a stronger oxidizing agent than I2(s), and I-(aq) is a stronger reducing agent than Ni(s). |
I-(aq) is a stronger oxidizing agent than Ni(s), and I2(s) is a stronger reducing agent than Ni2+(aq). |
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