Problem: Examine the following half-reactions and select the strongest reducing agent among the species listed.PbI2(s) + 2e– ⇌ Pb(s) + 2I–(aq)                   E° = –0.365 VCa2+(aq) + 2e– ⇌ Ca(s)                               E° = –2.868 VPt2+(aq) + 2e– ⇌ Pt(s)                                 E° = 1.18 VBr2(l) + 2e– ⇌ 2Br–(aq)                               E° = 1.066 VA) Pb(s)B) Ca(s)C) Pt(s)D) Br–(aq)E) Pt2+(aq)

FREE Expert Solution

We’re being asked to determine the strongest reducing agent among the given species. The reducing agent is the species that are being oxidized in a redox reaction. Recall the mnemonics LEO GER.

Loss Electrons → Oxidation → Reducing Agent
Gain Electrons → Reduction → Oxidizing Agent



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

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Problem Details

Examine the following half-reactions and select the strongest reducing agent among the species listed.

PbI2(s) + 2e ⇌ Pb(s) + 2I(aq)                   E° = –0.365 V

Ca2+(aq) + 2e ⇌ Ca(s)                               E° = –2.868 V

Pt2+(aq) + 2e ⇌ Pt(s)                                 E° = 1.18 V

Br2(l) + 2e ⇌ 2Br(aq)                               E° = 1.066 V

A) Pb(s)

B) Ca(s)

C) Pt(s)

D) Br(aq)

E) Pt2+(aq)

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Redox Reaction concept. You can view video lessons to learn Redox Reaction. Or if you need more Redox Reaction practice, you can also practice Redox Reaction practice problems.