Given the half reactions and Eo values below,Fe + 2e- FeE° = -0.45 VH2O2 + 2H + 2e → 2H2OE° = +1.78 V2H* + 2e → H2E° = 0.00 V4H +NO3 + 3e→ NO + 2H20 E° = +0,96 VDetermine which species is the strongest reducing agent.OHO•FeNO

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Given the half reactions and Eo values below, Fe + 2e- Fe E° = -0.45 V H2O2 +2H + 2e → 2H2O E° = +1.78 V 2H* + 2e → H2 E° = 0.00 V 4H +NO3 + 3e → NO +2H2O E = +0.96 V Determine which species is the strongest reducing agent. O HO OH • Fe NO

Given the half reactions and Eo values below, Fe + 2e- Fe E° = -0.45 V H2O2 +2H + 2e → 2H2O E° = +1.78 V 2H* + 2e → H2 E° = 0.00 V 4H +NO3 + 3e → NO +2H2O E = +0.96 V Determine which species is the strongest reducing agent. O HO OH • Fe NO

Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

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Question

Given the half reactions and Eo values below,
Fe + 2e- Fe
E° = -0.45 V
H2O2 + 2H + 2e → 2H2O
E° = +1.78 V
2H* + 2e → H2
E° = 0.00 V
4H +NO3 + 3e
→ NO + 2H20 E° = +0,96 V
Determine which species is the strongest reducing agent.
OHO
•Fe
NO

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