Given the following two half-reactions, write the overall reaction in the direction in which it is product-favored, and calculate the standard cell potential.Pb2*(aq) + 2 e- -→ Pb(s)E° = -0.126 VFe3*(aq) + e¯ →Fe2*(s)E° = +0.771 VPb2*(aq) + 2 Fe²*(s) → Pb(s) + 2 Fe³*(aq);= +0.897 VcellPb2*(aq) + Fe²*(s) → Pb(s) + Fe³*(aq); E,cell= +0.645 VPb(s) + 2 Fe³*(aq) → Pb²*(aq) + 2 Fe²*(s); F°cell= +1.416 VPb(s) + 2 Fe*(aq) → Pb²*(aq) + 2 Fe²*(s); E.'cell= +0.897 VPb(s) + Fe³*(aq) → Pb²*(aq) + Fe²*(s);= +0.645 V

We have to tell which option is correct from given choices of options by telling correct product…

Answered: Given the following two half-reactions,…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 77AP

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Given the following two half-reactions, write the overall reaction in the direction in which it is product- favored, and calculate the standard cell potential. Pb2*(aq) + 2 e- → Pb(s) E° = -0.126 V