Which species is the strongest oxidizing agent, why? And which is the strongest reducing agent, why? Consider the following half-reactions:Cl2(g) 2e 2cI (ag)Eo = 1.36 V%3DI2G) • 2e 21 (aq)I2(g) *Eo= 0.535 V%3DPb* + 2e →(aq)Pb(s)Eo = - 0.126 VCr3* (ag) + 3e Cres)Cr(s)Eo = - 0.74 V2+Mg (ag) + 2e →Mg(s)E, = -2.375 V

From given data , based on the E° value given for the half actions we can predict the strongest…

Consider the following half-reactions: Cl2(9) + 2e - 2cF (ag) = 1. %3D I2(9) + 2e - → 21 (aq) E, = 0. %3D Pb2*(ag) + 2e → Pb(s) Eo = - 0 Crs*(og) + 3e→ Cris) Ea = -

Consider the following half-reactions: Cl2(9) + 2e - 2cF (ag) = 1. %3D I2(9) + 2e - → 21 (aq) E, = 0. %3D Pb2(ag) + 2e → Pb(s) Eo = - 0 Crs(og) + 3e→ Cris) Ea = -

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter20: Electrochemistry

Section: Chapter Questions

Problem 60A

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Question

Which species is the strongest oxidizing agent, why? And which is the strongest reducing agent, why?

Consider the following half-reactions:
Cl2(g) 2e 2cI (ag)
Eo = 1.36 V
%3D
I2G) • 2e 21 (aq)
I2(g) *
Eo= 0.535 V
%3D
Pb* + 2e →
(aq)
Pb(s)
Eo = - 0.126 V
Cr3* (ag) + 3e Cres)
Cr(s)
Eo = - 0.74 V
2+
Mg (ag) + 2e →
Mg(s)
E, = -2.375 V

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