A chemist designs a galvanic cell that uses these two half-reactions: MnO4(aq)+2 H₂O(+3e Br₂(1)+2e Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. half-reaction Answer the following questions about this cell. Do you have enough information to calculate the cell voltage under standard conditions? OYes No If you said it was possible to calculate the cell voltage, do so and enter your answer v here. Round your answer to 2 significant digits. 1 MnO₂(s)+4 OH (aq) 1 2 Br (aq) standard reduction potential Ed=+0.59 V red Ered=+1.065 V
A chemist designs a galvanic cell that uses these two half-reactions: MnO4(aq)+2 H₂O(+3e Br₂(1)+2e Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. half-reaction Answer the following questions about this cell. Do you have enough information to calculate the cell voltage under standard conditions? OYes No If you said it was possible to calculate the cell voltage, do so and enter your answer v here. Round your answer to 2 significant digits. 1 MnO₂(s)+4 OH (aq) 1 2 Br (aq) standard reduction potential Ed=+0.59 V red Ered=+1.065 V
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 14P
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![A chemist designs a galvanic cell that uses these two half-reactions:
1
MnO4(aq) + 2 H₂O(1)+3e
Write a balanced
equation for the
half-reaction that 0
happens at the
cathode.
Write a balanced
equation for the
half-reaction that
happens at the
anode.
Answer the following questions about this cell.
Write a balanced
equation for the
overall reaction
that powers the
cell. Be sure the
reaction is
spontaneous as
written.
Do you have
enough
information to
calculate the cell
voltage under
standard
conditions?
half-reaction
Br₂(1)+2e - 2 Br (aq)
0
O Yes
1
O No
If you said it was
possible to
calculate the cell
voltage, do so and
enter your answer v
here. Round your
answer to 2
significant digits.
MnO₂ (s) +4 OH (aq)
standard reduction potential
Ered
= +0.59 V
Ered
=+1.065 V](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F98ddc1e7-1afc-4f0e-b623-cf5e11e78fa9%2F8d575e5f-a6ec-4ed3-a5e7-65d32d594a7b%2Ft8esob6_processed.jpeg&w=3840&q=75)
Transcribed Image Text:A chemist designs a galvanic cell that uses these two half-reactions:
1
MnO4(aq) + 2 H₂O(1)+3e
Write a balanced
equation for the
half-reaction that 0
happens at the
cathode.
Write a balanced
equation for the
half-reaction that
happens at the
anode.
Answer the following questions about this cell.
Write a balanced
equation for the
overall reaction
that powers the
cell. Be sure the
reaction is
spontaneous as
written.
Do you have
enough
information to
calculate the cell
voltage under
standard
conditions?
half-reaction
Br₂(1)+2e - 2 Br (aq)
0
O Yes
1
O No
If you said it was
possible to
calculate the cell
voltage, do so and
enter your answer v
here. Round your
answer to 2
significant digits.
MnO₂ (s) +4 OH (aq)
standard reduction potential
Ered
= +0.59 V
Ered
=+1.065 V
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