F2(g)+2e-→2F-(aq)2.866O3(g)+2H+(aq)+2e-→O2(g)+H2O(l)2.076Co3+(aq)+e-→Co2+(aq)1.92H2O2(aq)+2H+(aq)+2e-→2H2O(l)1.776Ce4+(aq)+e-→Ce3+(aq)1.72Au+(aq)+e-→Au(s)1.692PbO2(s)+4H+(aq)+SO42-(aq)+2e-→PbSO4(s)+2H2O(l)1.691MnO4-(aq)+8H+(aq)+5e-→Mn2+(aq)+4H2O(l)1.507Au3+(aq)+3e-→Au(s)1.498Cr2O72-(aq)+14H+(aq)+6e-→2Cr3+(aq)+7H2O(l)1.36Cl2(g)+2e-→2Cl-(aq)1.358O2(g)+4H+(aq)+4e-→2H2O(l)1.229MnO2(s)+4H+(aq)+2e-→Mn2+(aq)+2H2O(l)1.2242IO3-(aq)+12H+(aq)+10e-→I2(s)+6H2O(l)1.195Br2(l)+2e-→2Br-(aq)1.066VO2+(aq)+2H+(aq)+e-→VO2+(aq)+H2O(l)0.991HNO2(aq)+H+(aq)+e-→NO(g)+H2O(l)0.983NO3-(aq)+4H+(aq)+3e-→NO(g)+2H2O(l)0.9572Hg2+(aq)+2e-→Hg22+(aq)0.92Hg2+(aq)+2e-→Hg(l)0.851Ag+(aq)+e-→Ag(s)0.800Hg22+(aq)+2e-→2Hg(l)0.797Fe3+(aq)+e-→Fe2+(aq)0.771O2(g)+2H+(aq)+2e-→H2O2(aq)0.695MnO4-(aq)+2H2O(l)+3e-→MnO2(s)+4OH-(aq)0.595I2(s)+2e-→2I-(aq)0.536Cu+(aq)+e-→Cu(s)0.521O2(g)+2H2O(l)+4e-→4OH-(aq)0.401Cu2+(aq)+2e-→Cu(s)0.342HSO4-(aq)+3H+(aq)+2e-→H2SO3(aq)+H2O(l)0.172SO42-(aq)+4H+(aq)+2e-→SO2(g)+2H2O(l)0.172Cu2+(aq)+e-→Cu+(aq)0.153Sn4+(aq)+2e-→Sn2+(aq)0.1512H+(aq)+2e-→H2(g)0.000Fe3+(aq)+3e-→Fe(s)-0.037Pb2+(aq)+2e-→Pb(s)-0.126CrO42-(aq)+4H2O(l)+3e-→Cr(OH)3(s)+5OH-(aq)-0.13Sn2+(aq)+2e-→Sn(s)-0.138N2(g)+5H+(aq)+4e-→N2H5+(aq)-0.214Ni2+(aq)+2e-→Ni(s)-0.257Co2+(aq)+2e-→Co(s)-0.28PbSO4(s)+H+(aq)+2e-→Pb(s)+HSO4-(aq)-0.359Cd2+(aq)+2e-→Cd(s)-0.403Cr3+(aq)+e-→Cr2+(aq)-0.407Fe2+(aq)+2e-→Fe(s)-0.447Cr3+(aq)+3e-→Cr(s)-0.744Zn2+(aq)+2e-→Zn(s)-0.7622H2O(l)+2e-→H2(g)+2OH-(aq)-0.828Cr2+(aq)+2e-→Cr(s)-0.913N2(g)+4H2O(l)+4e-→4OH-(aq)+N2H4(aq)-1.16Mn2+(aq)+2e-→Mn(s)-1.185Al3+(aq)+3e-→Al(s)-1.676Be2+(aq)+2e-→Be(s)-1.847Sc3+(aq)+3e-→Sc(s)-2.077Mg2+(aq)+2e-→Mg(s)-2.372Na+(aq)+e-→Na(s)-2.71Ca2+(aq)+2e-→Ca(s)-2.868Sr2+(aq)+2e-→Sr(s)-2.899Ba2+(aq)+2e-→Ba(s)-2.912K+(aq)+e-→K(s)-2.931Li+(aq)+e-→Li(s)-3.040 A certain half-reaction has a standard reduction potential \( E_{\text{red}}^0 = +0.69 \, \text{V} \). An engineer proposes using this half-reaction at the anode of a galvanic cell that must provide at least 0.60 V of electrical power. The cell will operate under standard conditions.*Note for advanced students: assume the engineer requires this half-reaction to happen at the anode of the cell.* ### Educational Module: Understanding Standard Reduction Potentials**1. Minimum Standard Reduction Potential**- **Question:** Is there a minimum standard reduction potential that the half-reaction used at the cathode of this cell can have? - Options: - ☑ yes, there is a minimum. - \( E_{\text{red}}^0 = \) [Enter value] V - ☐ no minimum- **Instructions:** - If there is a minimum, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. - If there is no lower limit, check the "no" box.---**2. Maximum Standard Reduction Potential**- **Question:** Is there a maximum standard reduction potential that the half-reaction used at the cathode of this cell can have? - Options: - ☐ yes, there is a maximum. - \( E_{\text{red}}^0 = \) [Enter value] V - ☑ no maximum- **Instructions:** - If there is a maximum, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. - If there is no upper limit, check the "no" box.---**3. Writing a Balanced Half-Reaction**- **Task:** Using the information in the ALEKS Data tab, write a balanced equation describing a half-reaction that could be used at the cathode of this cell. - \( \boxed{\text{[Enter half-reaction here]}} \)- **Note:** Write the half-reaction as it would actually occur at the cathode.

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Answered: Is there a minimum standard reduction…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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F₂(g)+2e^-→2F^-(aq)	2.866
O₃(g)+2H⁺(aq)+2e^-→O₂(g)+H₂O(l)	2.076
Co³⁺(aq)+e^-→Co²⁺(aq)	1.92
H₂O₂(aq)+2H⁺(aq)+2e^-→2H₂O(l)	1.776
Ce⁴⁺(aq)+e^-→Ce³⁺(aq)	1.72
Au⁺(aq)+e^-→Au(s)	1.692
PbO₂(s)+4H⁺(aq)+SO₄^2-(aq)+2e^-→PbSO₄(s)+2H₂O(l)	1.691
MnO₄^-(aq)+8H⁺(aq)+5e^-→Mn²⁺(aq)+4H₂O(l)	1.507
Au³⁺(aq)+3e^-→Au(s)	1.498
Cr₂O₇^2-(aq)+14H⁺(aq)+6e^-→2Cr³⁺(aq)+7H₂O(l)	1.36
Cl₂(g)+2e^-→2Cl^-(aq)	1.358
O₂(g)+4H⁺(aq)+4e^-→2H₂O(l)	1.229
MnO₂(s)+4H⁺(aq)+2e^-→Mn²⁺(aq)+2H₂O(l)	1.224
2IO₃^-(aq)+12H⁺(aq)+10e^-→I₂(s)+6H₂O(l)	1.195
Br₂(l)+2e^-→2Br^-(aq)	1.066
VO₂⁺(aq)+2H⁺(aq)+e^-→VO²⁺(aq)+H₂O(l)	0.991
HNO₂(aq)+H⁺(aq)+e^-→NO(g)+H₂O(l)	0.983

NO₃^-(aq)+4H⁺(aq)+3e^-→NO(g)+2H₂O(l)	0.957
2Hg²⁺(aq)+2e^-→Hg₂²⁺(aq)	0.92
Hg²⁺(aq)+2e^-→Hg(l)	0.851
Ag⁺(aq)+e^-→Ag(s)	0.800
Hg₂²⁺(aq)+2e^-→2Hg(l)	0.797
Fe³⁺(aq)+e^-→Fe²⁺(aq)	0.771
O₂(g)+2H⁺(aq)+2e^-→H₂O₂(aq)	0.695
MnO₄^-(aq)+2H₂O(l)+3e^-→MnO₂(s)+4OH^-(aq)	0.595
I₂(s)+2e^-→2I^-(aq)	0.536
Cu⁺(aq)+e^-→Cu(s)	0.521
O₂(g)+2H₂O(l)+4e^-→4OH^-(aq)	0.401
Cu²⁺(aq)+2e^-→Cu(s)	0.342
HSO₄^-(aq)+3H⁺(aq)+2e^-→H₂SO₃(aq)+H₂O(l)	0.172
SO₄^2-(aq)+4H⁺(aq)+2e^-→SO₂(g)+2H₂O(l)	0.172
Cu²⁺(aq)+e^-→Cu⁺(aq)	0.153
Sn⁴⁺(aq)+2e^-→Sn²⁺(aq)	0.151
2H⁺(aq)+2e^-→H₂(g)	0.000
Fe³⁺(aq)+3e^-→Fe(s)	-0.037
Pb²⁺(aq)+2e^-→Pb(s)	-0.126
CrO₄^2-(aq)+4H₂O(l)+3e^-→Cr(OH)₃(s)+5OH^-(aq)	-0.13
Sn²⁺(aq)+2e^-→Sn(s)	-0.138
N₂(g)+5H⁺(aq)+4e^-→N₂H₅⁺(aq)	-0.214
Ni²⁺(aq)+2e^-→Ni(s)	-0.257
Co²⁺(aq)+2e^-→Co(s)	-0.28
PbSO₄(s)+H⁺(aq)+2e^-→Pb(s)+HSO₄^-(aq)	-0.359
Cd²⁺(aq)+2e^-→Cd(s)	-0.403
Cr³⁺(aq)+e^-→Cr²⁺(aq)	-0.407
Fe²⁺(aq)+2e^-→Fe(s)	-0.447
Cr³⁺(aq)+3e^-→Cr(s)	-0.744
Zn²⁺(aq)+2e^-→Zn(s)	-0.762
2H₂O(l)+2e^-→H₂(g)+2OH^-(aq)	-0.828
Cr²⁺(aq)+2e^-→Cr(s)	-0.913
N₂(g)+4H₂O(l)+4e^-→4OH^-(aq)+N₂H₄(aq)	-1.16
Mn²⁺(aq)+2e^-→Mn(s)	-1.185
Al³⁺(aq)+3e^-→Al(s)	-1.676
Be²⁺(aq)+2e^-→Be(s)	-1.847
Sc³⁺(aq)+3e^-→Sc(s)	-2.077
Mg²⁺(aq)+2e^-→Mg(s)	-2.372
Na⁺(aq)+e^-→Na(s)	-2.71
Ca²⁺(aq)+2e^-→Ca(s)	-2.868
Sr²⁺(aq)+2e^-→Sr(s)	-2.899
Ba²⁺(aq)+2e^-→Ba(s)	-2.912
K⁺(aq)+e^-→K(s)	-2.931
Li⁺(aq)+e^-→Li(s)	-3.040

A certain half-reaction has a standard reduction potential \( E_{\text{red}}^0 = +0.69 \, \text{V} \). An engineer proposes using this half-reaction at the anode of a galvanic cell that must provide at least 0.60 V of electrical power. The cell will operate under standard conditions.

*Note for advanced students: assume the engineer requires this half-reaction to happen at the anode of the cell.*

### Educational Module: Understanding Standard Reduction Potentials

**1. Minimum Standard Reduction Potential**

- **Question:** Is there a minimum standard reduction potential that the half-reaction used at the cathode of this cell can have?

- Options:
- ☑ yes, there is a minimum.
- \( E_{\text{red}}^0 = \) [Enter value] V
- ☐ no minimum

- **Instructions:**
- If there is a minimum, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places.
- If there is no lower limit, check the "no" box.

---

**2. Maximum Standard Reduction Potential**

- **Question:** Is there a maximum standard reduction potential that the half-reaction used at the cathode of this cell can have?

- Options:
- ☐ yes, there is a maximum.
- \( E_{\text{red}}^0 = \) [Enter value] V
- ☑ no maximum

- **Instructions:**
- If there is a maximum, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places.
- If there is no upper limit, check the "no" box.

---

**3. Writing a Balanced Half-Reaction**

- **Task:** Using the information in the ALEKS Data tab, write a balanced equation describing a half-reaction that could be used at the cathode of this cell.

- \( \boxed{\text{[Enter half-reaction here]}} \)

- **Note:** Write the half-reaction as it would actually occur at the cathode.

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