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
100%
39 a. What is produced at each electrode in the electrolysis of NaBr(aq)?
Please note incorrect answer:
Anode: Br2
Cathode: H2
Not produced: Na, O2
![Refer to this table of standard reduction potentials to
answer the questions.
Reduction half-reaction
Potential
(V)
+2.87
+1.23
+1.07
+0.80
Ag+ +eAg(s)
2H₂O(1)+2e-H₂(g) + 2OH(aq) -0.83
Na (aq) +e-Na(s)
-2.71
F₂(g) +2e-2F (aq)
O₂(g) + 4H+ (aq) + 4e¯→2H₂O(1)
Br₂ (1)+2e-2Br (aq)
Note that at [H]-10-7 M. the electrode potential
for O₂(g) + 4H+ (aq) + 4e¯→2H₂O(1) under
these nonstandard conditions is E= +0.82 V.
At [OH-] = 107 M, the electrode potential for
2H₂O(1)+2e →H₂(g) + 2OH(aq) under
these nonstandard conditions is E= -0.41 V.
Review I Constants I Periodic Table
two inert electrodes (usually platinum), which serve as the electrical connection between the power source
and the substance undergoing electrolysis.
As with any cell, oxidation occurs at the anode and reduction occurs at the cathode. The oxidation of water, which
produces oxygen (O₂) gas, will compete with the oxidation of the anion, and the reduction of water, which produces
hydrogen (H₂) gas, will compete with the reduction of the cation. Only the reaction with the higher (more positive)
potential will occur. Keep in mind that the potentials for the oxidation reaction have the opposite sign as those for the
corresponding reduction reactions. For example, the oxidation reaction Ag(s)-Ag +e would have an Ex of -
0.80 V.
▾ Part A
What is produced at each electrode in the electrolysis of NaBr(aq)?
Drag the appropriate items to their respective bins.
▸ View Available Hint(s)
Anode
Submit
Br₂ (1)
Cathode
Previous Answers
H₂(g)
X Incorrect; Try Again; 4 attempts remaining
Reset Help
Not produced
Na(s) O₂(g)
Anode
Bra(1)
ANSWER 2: Deduction: -3%
Anode
Cathode
Bra(1) O₂(g)
H₂(g)
You sorted 2 out of 4 items incorrectly. Compare the potentials for two species that could be oxidized at the cathode.
For example, the oxidation of water has a potential of -0.82 V, since the conditions are nonstandard and potential
for the oxidiation of a species is the opposite that for the reduction. The species with the less negative potential will
be oxidized at the anode.
Cathode
Not produced
H₂(g) Na(s)
Na(s) O₂(g)
Reset Help
Not produced](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb0be78df-234d-4653-8235-8227b9098990%2F8868fd29-add6-441e-9117-def1de4d7d84%2Fkr4owj_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Refer to this table of standard reduction potentials to
answer the questions.
Reduction half-reaction
Potential
(V)
+2.87
+1.23
+1.07
+0.80
Ag+ +eAg(s)
2H₂O(1)+2e-H₂(g) + 2OH(aq) -0.83
Na (aq) +e-Na(s)
-2.71
F₂(g) +2e-2F (aq)
O₂(g) + 4H+ (aq) + 4e¯→2H₂O(1)
Br₂ (1)+2e-2Br (aq)
Note that at [H]-10-7 M. the electrode potential
for O₂(g) + 4H+ (aq) + 4e¯→2H₂O(1) under
these nonstandard conditions is E= +0.82 V.
At [OH-] = 107 M, the electrode potential for
2H₂O(1)+2e →H₂(g) + 2OH(aq) under
these nonstandard conditions is E= -0.41 V.
Review I Constants I Periodic Table
two inert electrodes (usually platinum), which serve as the electrical connection between the power source
and the substance undergoing electrolysis.
As with any cell, oxidation occurs at the anode and reduction occurs at the cathode. The oxidation of water, which
produces oxygen (O₂) gas, will compete with the oxidation of the anion, and the reduction of water, which produces
hydrogen (H₂) gas, will compete with the reduction of the cation. Only the reaction with the higher (more positive)
potential will occur. Keep in mind that the potentials for the oxidation reaction have the opposite sign as those for the
corresponding reduction reactions. For example, the oxidation reaction Ag(s)-Ag +e would have an Ex of -
0.80 V.
▾ Part A
What is produced at each electrode in the electrolysis of NaBr(aq)?
Drag the appropriate items to their respective bins.
▸ View Available Hint(s)
Anode
Submit
Br₂ (1)
Cathode
Previous Answers
H₂(g)
X Incorrect; Try Again; 4 attempts remaining
Reset Help
Not produced
Na(s) O₂(g)
Anode
Bra(1)
ANSWER 2: Deduction: -3%
Anode
Cathode
Bra(1) O₂(g)
H₂(g)
You sorted 2 out of 4 items incorrectly. Compare the potentials for two species that could be oxidized at the cathode.
For example, the oxidation of water has a potential of -0.82 V, since the conditions are nonstandard and potential
for the oxidiation of a species is the opposite that for the reduction. The species with the less negative potential will
be oxidized at the anode.
Cathode
Not produced
H₂(g) Na(s)
Na(s) O₂(g)
Reset Help
Not produced
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