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i) Consider an electrochemical cell involving Cadmium and Silver. Cd2* (aq) + 2e- → Cd(s) E° = -0.40 V Ag*(aq) + e-→ Ag(s) E° = +0.80 V a) What is the standard reduction potential of anode? b) What is the standard reduction potential of cathode?

i) Consider an electrochemical cell involving Cadmium and Silver. Cd2* (aq) + 2e- → Cd(s) E° = -0.40 V Ag*(aq) + e-→ Ag(s) E° = +0.80 V a) What is the standard reduction potential of anode? b) What is the standard reduction potential of cathode?

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
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i) Consider an electrochemical cell involving Cadmium and Silver. Cd2+ (aq) +2e- → Cd(s) E° = -0.40 V Ag*(aq) + e- → Ag(s) E° = +0.80 V a) What is the standard reduction potential of anode? b) What is the standard reduction potential of cathode? c) Calculate the potential of this cell under standard conditions(E°cell).
Transcribed Image Text:i) Consider an electrochemical cell involving Cadmium and Silver. Cd2+ (aq) +2e- → Cd(s) E° = -0.40 V Ag*(aq) + e- → Ag(s) E° = +0.80 V a) What is the standard reduction potential of anode? b) What is the standard reduction potential of cathode? c) Calculate the potential of this cell under standard conditions(E°cell).
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