A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential HNO2(aq)+H(aq)+e NO(g)+H₂O(1) - Cl(9)+2e 2 Cl (aq) Answer the following questions about this cell. 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. Do you have ☐ enough information to calculate the cell voltage under standard conditions? Yes No If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 2 significant digits. Ον = +1.00 V red 0 Ered = +1.359 V 0-0 0 0 ē X G
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential HNO2(aq)+H(aq)+e NO(g)+H₂O(1) - Cl(9)+2e 2 Cl (aq) Answer the following questions about this cell. 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. Do you have ☐ enough information to calculate the cell voltage under standard conditions? Yes No If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 2 significant digits. Ον = +1.00 V red 0 Ered = +1.359 V 0-0 0 0 ē X G
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...
Question
![A chemist designs a galvanic cell that uses these two half-reactions:
half-reaction
standard reduction potential
HNO2(aq)+H(aq)+e
NO(g)+H₂O(1)
-
Cl(9)+2e 2 Cl (aq)
Answer the following questions about this cell.
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.
Do you have
☐
enough
information to
calculate the cell
voltage under
standard
conditions?
Yes
No
If you said it was
possible to
calculate the cell
voltage, do so and
enter your answer
here. Round your
answer to 2
significant digits.
Ον
= +1.00 V
red
0
Ered
= +1.359 V
0-0 0 0
ē
X
G](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F93e02f2d-b0b4-40f2-b59c-ee2919cc5490%2F4eaddca0-d7a5-4e77-bb07-600eb8f005c5%2Fapi3tvh_processed.jpeg&w=3840&q=75)
Transcribed Image Text:A chemist designs a galvanic cell that uses these two half-reactions:
half-reaction
standard reduction potential
HNO2(aq)+H(aq)+e
NO(g)+H₂O(1)
-
Cl(9)+2e 2 Cl (aq)
Answer the following questions about this cell.
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.
Do you have
☐
enough
information to
calculate the cell
voltage under
standard
conditions?
Yes
No
If you said it was
possible to
calculate the cell
voltage, do so and
enter your answer
here. Round your
answer to 2
significant digits.
Ον
= +1.00 V
red
0
Ered
= +1.359 V
0-0 0 0
ē
X
G
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