Problem: Consider the following standard reduction potentials:Al3+ + 3e –  → Al (s)                  E ̊red = –1.66AgBr (s) + e – → Ag (s) + Br–    E ̊red = +0.07Sn4+ + 2e – → Sn2+                  E ̊red = +0.14Fe3+ + e – → Fe2+                     E ̊red = +0.77Which of the following substances below is the strongest reducing agent?a) Fe3+b) Fe2+c) Ag (s)d) Al3+e) Al (s)

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We’re being asked which of the given species is the strongest reducing agent. Reducing agent are the species that are being oxidized in a redox reaction. Recall the mnemonics LEO GER.

Lose               Gain

Electron         Electrons

Oxidation       Reduction

The strongest reducing agent would be the element that would be easily oxidized or easily loses an electron:

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Problem Details

Consider the following standard reduction potentials:

Al3+ + 3e   → Al (s)                  E ̊red = –1.66

AgBr (s) + e  → Ag (s) + Br    E ̊red = +0.07

Sn4+ + 2e  → Sn2+                  E ̊red = +0.14

Fe3+ + e  → Fe2+                     E ̊red = +0.77

Which of the following substances below is the strongest reducing agent?

a) Fe3+

b) Fe2+

c) Ag (s)

d) Al3+

e) Al (s)

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