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Consider the following two half- reactions: V 2H+ + 2e → H₂ (g) Pb2+ + 2e → Pb(s) 0.126 V They give the following cell reaction: Pb2+ pH = 4.7 At what pH does the reaction become spontaneous? pH = 11.1 pH (aq) + H2(g) = Pb(s) + 2H+ (aq) = E° = 0 E° = 2.1

Consider the following two half- reactions: V 2H+ + 2e → H₂ (g) Pb2+ + 2e → Pb(s) 0.126 V They give the following cell reaction: Pb2+ pH = 4.7 At what pH does the reaction become spontaneous? pH = 11.1 pH (aq) + H2(g) = Pb(s) + 2H+ (aq) = E° = 0 E° = 2.1

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.88QP: Calculate the cell potential of a cell operating with the following reaction at 25C, in which...
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Consider the following two half- reactions: 2H+ 2e → H₂ (g) Pb2+ + 2e → Pb(s) 0.126 V They give the following cell reaction: Pb2+ (aq) + H2(g) Pb(s) + 2H+ (aq) pH = 4.7 pH At what pH does the reaction become spontaneous? 11.1 pH = 2.1 E° = 0 E° = pH = 6.8 pH = 9.3
Transcribed Image Text:Consider the following two half- reactions: 2H+ 2e → H₂ (g) Pb2+ + 2e → Pb(s) 0.126 V They give the following cell reaction: Pb2+ (aq) + H2(g) Pb(s) + 2H+ (aq) pH = 4.7 pH At what pH does the reaction become spontaneous? 11.1 pH = 2.1 E° = 0 E° = pH = 6.8 pH = 9.3
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