Chemists are working on the electrochemistry of bromine species. They prepared the following electrochemical cells (Table 1) at 298 K. Table 1. Two electrochemical cells to study the electrochemistry of bromine species. Cell L: Pt(s) | Br21) | Br-(aq) (1.0 M) || Br-(aq) (x M) from [PbBr4]2-| Br2(1) | Pt(s) Cell H: Pt(s) | Br21) | Br-(aq) (x M) || BrO3-(aq) (0.43 M), H+(aq) (1.00 M) | Br2(1)| Pt(s) A concentration cell (L) where the cathode half-cell uses an equilibrium solution of [PbBr4]2-(aq) as the source of bromide ions was prepared. A galvanic cell (H), where the bromide ion concentration in the anode is equal to that in the cathode of cell L was also prepared. Given: Eºred Br2(1)/Br-(aq) = +1.07 V Given that the electrochemical cell L gives a potential of 0.0570 V, determine the concentration of bromide ions present in its cathode half-cell. ● The equilibrium concentration of Pb2+(aq) and [PbBr4]2-(aq) in the cathode half-cell of L are 0.15 M and 0.32 M, respectively. Determine the equilibrium constant for the formation of [PbBr4]2-.
Chemists are working on the electrochemistry of bromine species. They prepared the following electrochemical cells (Table 1) at 298 K. Table 1. Two electrochemical cells to study the electrochemistry of bromine species. Cell L: Pt(s) | Br21) | Br-(aq) (1.0 M) || Br-(aq) (x M) from [PbBr4]2-| Br2(1) | Pt(s) Cell H: Pt(s) | Br21) | Br-(aq) (x M) || BrO3-(aq) (0.43 M), H+(aq) (1.00 M) | Br2(1)| Pt(s) A concentration cell (L) where the cathode half-cell uses an equilibrium solution of [PbBr4]2-(aq) as the source of bromide ions was prepared. A galvanic cell (H), where the bromide ion concentration in the anode is equal to that in the cathode of cell L was also prepared. Given: Eºred Br2(1)/Br-(aq) = +1.07 V Given that the electrochemical cell L gives a potential of 0.0570 V, determine the concentration of bromide ions present in its cathode half-cell. ● The equilibrium concentration of Pb2+(aq) and [PbBr4]2-(aq) in the cathode half-cell of L are 0.15 M and 0.32 M, respectively. Determine the equilibrium constant for the formation of [PbBr4]2-.
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 77AP
Related questions
Question
![Chemists are working on the electrochemistry of bromine species. They prepared the
following electrochemical cells (Table 1) at 298 K.
Table 1. Two electrochemical cells to study the electrochemistry of bromine species.
Cell L:
Pt(s) | Br2(1) | Br-(aq) (1.0 M) || Br-(aq) (x M) from [PbBr4]2-| Br2(1) | Pt(s)
Cell H:
Pt(s) | Br21) | Br-(aq) (x M) || BrO3-(aq) (0.43 M), H+(aq) (1.00 M) | Br2(1) | Pt(s)
A concentration cell (L) where the cathode half-cell uses an equilibrium solution of [PbBr4]2-(aq)
as the source of bromide ions was prepared. A galvanic cell (H), where the bromide ion
concentration in the anode is equal to that in the cathode of cell L was also prepared.
Given: Eºred Br2(1)/Br-(aq) = +1.07 V
Given that the electrochemical cell L gives a potential of 0.0570 V, determine the
concentration of bromide ions present in its cathode half-cell.
●
The equilibrium concentration of Pb2+(aq) and [PbBr4]2-(aq) in the cathode half-cell of L are
0.15 M and 0.32 M, respectively. Determine the equilibrium constant for the formation
of [PbBr4]2-.
Write the overall redox reaction for the electrochemical cell H.
Given that the electrochemical cell H gives a potential of 0.350 V, determine the
standard potential for the reduction of BrO3-(aq) to Br2(1).
Construct a Latimer diagram that shows the three bromine species (BrO3-, Br2, and Br.)
in this problem. Include the skip potential for the reduction of BrO3-(aq) to Br-(aq) under
standard conditions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcc8bbb83-2fce-471a-9f22-61032a99fe9d%2F5d1cc4b7-d5a8-4c28-8824-b58d41136255%2F7yt21cc_processed.png&w=3840&q=75)
Transcribed Image Text:Chemists are working on the electrochemistry of bromine species. They prepared the
following electrochemical cells (Table 1) at 298 K.
Table 1. Two electrochemical cells to study the electrochemistry of bromine species.
Cell L:
Pt(s) | Br2(1) | Br-(aq) (1.0 M) || Br-(aq) (x M) from [PbBr4]2-| Br2(1) | Pt(s)
Cell H:
Pt(s) | Br21) | Br-(aq) (x M) || BrO3-(aq) (0.43 M), H+(aq) (1.00 M) | Br2(1) | Pt(s)
A concentration cell (L) where the cathode half-cell uses an equilibrium solution of [PbBr4]2-(aq)
as the source of bromide ions was prepared. A galvanic cell (H), where the bromide ion
concentration in the anode is equal to that in the cathode of cell L was also prepared.
Given: Eºred Br2(1)/Br-(aq) = +1.07 V
Given that the electrochemical cell L gives a potential of 0.0570 V, determine the
concentration of bromide ions present in its cathode half-cell.
●
The equilibrium concentration of Pb2+(aq) and [PbBr4]2-(aq) in the cathode half-cell of L are
0.15 M and 0.32 M, respectively. Determine the equilibrium constant for the formation
of [PbBr4]2-.
Write the overall redox reaction for the electrochemical cell H.
Given that the electrochemical cell H gives a potential of 0.350 V, determine the
standard potential for the reduction of BrO3-(aq) to Br2(1).
Construct a Latimer diagram that shows the three bromine species (BrO3-, Br2, and Br.)
in this problem. Include the skip potential for the reduction of BrO3-(aq) to Br-(aq) under
standard conditions.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 6 steps with 2 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:
9781337398909
Author:
Lawrence S. Brown, Tom Holme
Publisher:
Cengage Learning
General Chemistry - Standalone book (MindTap Cour…
Chemistry
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:
Cengage Learning