2. The following half reactions can be coupled to create a galvanic cell. Use the data below to answer the following questions. Pb2+ (a (aq) + 2e → Pb(s) = Ered -0.132 V at 293 K Cu2+(a (aq) + 2e → Cu(s) Ered +0.339 V at 293 K a. Write the balanced net redox reaction for an electrochemical cell created by coupling the half reactions above under standard conditions of concentration. Write this reaction in the spontaneous direction. What is E° cell at 293 K? Pb2+ 2e- Pb €= -0.132V 4 = 0.132V Cu2+ + ae" Cu Pb+ Cu Cu E° = 0.339 V E° = (0.132 + 0.339) E cell = 0.471 V e. An electrochemical cell that couples the half reactions above is created with 0.4 M CuSO4 solution in one half cell and 2x10-7 M Pb(NO3)2 in the other at 293 K. What is Qc under these conditions? What is Ecell under these conditions? f. Given a standard (1 M) concentration of CuSO4 in the copper half-cell, determine the concentration of Pb(NO3)2 that would be required in the lead half-cell to achieve Ecell = 0.44 V at 293 K. Given that Ksp of Pb(NO3)2 is 23.3 at this temperature, is this electrochemical cell feasible? Briefly justify your answer by calculating and making reference to the molar solubility of Pb(NO3)2 at this temperature. g. What is the equilibrium constant Kc for the overall reaction from part a at 293 K?
2. The following half reactions can be coupled to create a galvanic cell. Use the data below to answer the following questions. Pb2+ (a (aq) + 2e → Pb(s) = Ered -0.132 V at 293 K Cu2+(a (aq) + 2e → Cu(s) Ered +0.339 V at 293 K a. Write the balanced net redox reaction for an electrochemical cell created by coupling the half reactions above under standard conditions of concentration. Write this reaction in the spontaneous direction. What is E° cell at 293 K? Pb2+ 2e- Pb €= -0.132V 4 = 0.132V Cu2+ + ae" Cu Pb+ Cu Cu E° = 0.339 V E° = (0.132 + 0.339) E cell = 0.471 V e. An electrochemical cell that couples the half reactions above is created with 0.4 M CuSO4 solution in one half cell and 2x10-7 M Pb(NO3)2 in the other at 293 K. What is Qc under these conditions? What is Ecell under these conditions? f. Given a standard (1 M) concentration of CuSO4 in the copper half-cell, determine the concentration of Pb(NO3)2 that would be required in the lead half-cell to achieve Ecell = 0.44 V at 293 K. Given that Ksp of Pb(NO3)2 is 23.3 at this temperature, is this electrochemical cell feasible? Briefly justify your answer by calculating and making reference to the molar solubility of Pb(NO3)2 at this temperature. g. What is the equilibrium constant Kc for the overall reaction from part a at 293 K?
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter19: Principles Of Chemical Reactivity: Electron Transfer Reactions
Section19.9: Corrosion: Redox Reactions In The Environment
Problem 2.5ACP: Assume the following electrochemical cell simulates the galvanic cell formed by copper and zinc in...
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Transcribed Image Text:2. The following half reactions can be coupled to create a galvanic cell. Use the data below to
answer the following questions.
Pb2+ (a
(aq) + 2e →
Pb(s)
=
Ered -0.132 V at 293 K
Cu2+(a
(aq)
+ 2e → Cu(s)
Ered +0.339 V at 293 K
a. Write the balanced net redox reaction for an electrochemical cell created by coupling the half
reactions above under standard conditions of concentration. Write this reaction in the spontaneous
direction. What is E° cell at 293 K?
Pb2+
2e-
Pb
€= -0.132V
4 = 0.132V
Cu2+ +
ae"
Cu
Pb+ Cu
Cu
E° = 0.339 V
E° = (0.132 + 0.339)
E cell = 0.471 V
Transcribed Image Text:e. An electrochemical cell that couples the half reactions above is created with 0.4 M CuSO4
solution in one half cell and 2x10-7 M Pb(NO3)2 in the other at 293 K. What is Qc under these
conditions? What is Ecell under these conditions?
f. Given a standard (1 M) concentration of CuSO4 in the copper half-cell, determine the
concentration of Pb(NO3)2 that would be required in the lead half-cell to achieve Ecell = 0.44 V at
293 K. Given that Ksp of Pb(NO3)2 is 23.3 at this temperature, is this electrochemical cell feasible?
Briefly justify your answer by calculating and making reference to the molar solubility of
Pb(NO3)2 at this temperature.
g. What is the equilibrium constant Kc for the overall reaction from part a at 293 K?
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