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Use the References to access important values if needed for this question. Use standard reduction potentials to calculate the equilibrium constant for the reaction: Co²+ (aq) + Cd(s) → Co(s) + Cd²+ (aq) Co2+ (aq) + 2e →Co(s) = -0.280 V Cd2+ (aq) +2e → Cd(s) F = -0.403 V red red Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at 298 K: AGO for this reaction would be Retry Entire Submit Answer 9 more group attempts remaining than zero. greater

Use the References to access important values if needed for this question. Use standard reduction potentials to calculate the equilibrium constant for the reaction: Co²+ (aq) + Cd(s) → Co(s) + Cd²+ (aq) Co2+ (aq) + 2e →Co(s) = -0.280 V Cd2+ (aq) +2e → Cd(s) F = -0.403 V red red Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at 298 K: AGO for this reaction would be Retry Entire Submit Answer 9 more group attempts remaining than zero. greater

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter17: Electrochemistry And Its Applications
Section: Chapter Questions
Problem 50QRT
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Use the References to access important values if needed for this question. Use standard reduction potentials to calculate the equilibrium constant for the reaction: Co2+(aq) +Cd(s) → Co(s) +Cd2+ (aq) Co2+ (aq) +2e → Co(s) Ed=-0.280 V red Cd2+ (aq) + 2e → Cd(s) Ed = -0.403 V red Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at 298 K: AGO for this reaction would be Retry Entire Submit Answer 9 more group attempts remaining >than zero. greater less ?
Transcribed Image Text:Use the References to access important values if needed for this question. Use standard reduction potentials to calculate the equilibrium constant for the reaction: Co2+(aq) +Cd(s) → Co(s) +Cd2+ (aq) Co2+ (aq) +2e → Co(s) Ed=-0.280 V red Cd2+ (aq) + 2e → Cd(s) Ed = -0.403 V red Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at 298 K: AGO for this reaction would be Retry Entire Submit Answer 9 more group attempts remaining >than zero. greater less ?
A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode ( PH₂)= 1 atm) immersed in a solution of unknown [H*]. If the cell potential is 0.189 V, what is the pH of the unknown solution at 298 K? pH =
Transcribed Image Text:A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode ( PH₂)= 1 atm) immersed in a solution of unknown [H*]. If the cell potential is 0.189 V, what is the pH of the unknown solution at 298 K? pH =
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