Is there a minimum standard reduction potential that the half-reaction used at the cathode of this cell can have? If so, 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. Is there a maximum standard reduction potential that the half-reaction used at the cathode of this cell can have? If so, 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. By 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. Note: write the half reaction as it would actually occur at the cathode. 0 yes, there is a minimum. no minimum yes, there is a maximum. no maximum 0 E = red Ov 0 E Ov red =
Is there a minimum standard reduction potential that the half-reaction used at the cathode of this cell can have? If so, 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. Is there a maximum standard reduction potential that the half-reaction used at the cathode of this cell can have? If so, 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. By 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. Note: write the half reaction as it would actually occur at the cathode. 0 yes, there is a minimum. no minimum yes, there is a maximum. no maximum 0 E = red Ov 0 E Ov red =
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 16P
Related questions
Question
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)+SO42-(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 |
Cr2O72-(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 |
SO42-(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 |
CrO42-(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 |
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