A chemist designs a galvanic cell that uses these two half-reactions: standard reduction potential half-reaction 2 H₂O(1)+2e ->>> H₂(9)+2OH (aq) 3+ 2+ Fe2(aq) Fe (aq)+e → Fe (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 ☐ O Yes standard conditions? If you said it was possible to calculate the cell O No voltage, do so and enter your answer here. Round your answer to 3 significant digits. Ον E =-0.83 V red = +0.771 V red ローロ ē X G
A chemist designs a galvanic cell that uses these two half-reactions: standard reduction potential half-reaction 2 H₂O(1)+2e ->>> H₂(9)+2OH (aq) 3+ 2+ Fe2(aq) Fe (aq)+e → Fe (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 ☐ O Yes standard conditions? If you said it was possible to calculate the cell O No voltage, do so and enter your answer here. Round your answer to 3 significant digits. Ον E =-0.83 V red = +0.771 V red ローロ ē X G
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 107QRT
Related questions
Question
![A chemist designs a galvanic cell that uses these two half-reactions:
standard reduction potential
half-reaction
2 H₂O(1)+2e
->>>
H₂(9)+2OH (aq)
3+
2+
Fe2(aq)
Fe (aq)+e → Fe (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
☐
O Yes
standard
conditions?
If you said it was
possible to
calculate the cell
O No
voltage, do so and
enter your answer
here. Round your
answer to 3
significant digits.
Ον
E
=-0.83 V
red
= +0.771 V
red
ローロ
ē
X
G](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F93e02f2d-b0b4-40f2-b59c-ee2919cc5490%2F8caebdcd-a191-4b6d-8c29-bcb8b5819080%2F1nvo1nc_processed.jpeg&w=3840&q=75)
Transcribed Image Text:A chemist designs a galvanic cell that uses these two half-reactions:
standard reduction potential
half-reaction
2 H₂O(1)+2e
->>>
H₂(9)+2OH (aq)
3+
2+
Fe2(aq)
Fe (aq)+e → Fe (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
☐
O Yes
standard
conditions?
If you said it was
possible to
calculate the cell
O No
voltage, do so and
enter your answer
here. Round your
answer to 3
significant digits.
Ον
E
=-0.83 V
red
= +0.771 V
red
ローロ
ē
X
G
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