Standard Reduction Potentials at 25°C (298 K) for Many Common Half-reactionsHalf-reaction8° (V)Half-reactionF₂ +2e2F-Ag2+ + eAg+Co³+ + e→→ Co²+H₂O₂ + 2H+ + 2eCe4++e Ce³+→ 2H₂OPbO₂ + 4H+ + SO42MnO4 + 4H+ + 3eIO4 + 2H+ + 2e →MnO4 + 8H+ + SeAu³+ + 3e → AuPbO₂ + 4H+ + 2eCl₂ +2e2C1-Hg₂2+ + 2eFe³+ + e+2e →→ PbSO4 + 2H₂O→ MnO₂ + 2H₂OIO3 + H₂O→ Mn²+ + 4H₂O→ Pb²+ + 2H₂OCr₂O72- + 14H+ + 6e- →2Cr³+ + 7H₂OO₂ + 4H+ + 4e → 2H₂OMnO₂ + 4H+ + 2eIO3 + 6H+ + Se-Br₂ 2e 2BrVO₂+ + 2H+ + eAuCl4 + 3e →NO3 + 4H+ClO₂ + e2Hg2+ + 2eAge → Ag→ Mn²+ + 2H₂O→ 1₂ + 3H₂O→ VO2+ + H₂OAu + 4CI-+ 3e → NO + 2H₂OClO₂-→ Hg₂²+→ 2HgFe2+O₂ + 2H+ + 2e → H₂O₂MnO4 + e→→ MnO4²-1₂ +2e → 21-CuteCu2.871.991.821.781.701.691.681.601.511.501.461.361.331.231.211.201.091.000.990.960.9540.910.800.800.770.680.560.540.52O₂ + 2H₂O + 4e4OH-Cu2+ + 2e → CuHg₂Cl₂ + 2e →→ 2Hg + 2Cl-AgCl +eAg + Cl-SO4 + 4H+ + 2eCu²+ + e2H+ + 2eFe³+ + 3eCu+→→ H₂→→ Fe→→ Pb→→ Sn→→ NiPb²+ + 2eSn²+ + 2eNi2+ + 2ePbSO4 + 2eCd2+ + 2e→→ Pb + SO4²-→→ Cd→→→ FeFe2+ + 2eCr³+ + eCr²+Cr³+ + 3e→ Cr→ ZnZn²+ + 2e2H₂O + 2e→ H₂ + 2OH-Mn²+ + 2e → MnAl³+ + 3e →→ AlH₂ +2e → 2H-Mg2+ + 2e → MgLa³+ + 3e → La→→→ NaNa+ + eCa2+ + 2eBa2+ + 2eK++eK→→ Ca→→ Ba→ H₂SO3 + H₂OLite Li8° (V)0.400.340.270.220.200.160.00-0.036-0.13-0.14-0.23-0.35-0.40-0.44-0.50-0.73-0.76-0.83-1.18-1.66-2.23-2.37-2.37-2.71-2.76-2.90-2.92-3.05 Using data from the Standard Reduction Potentials table, place the following in order of increasing strength as oxidizing agents (all under standard conditions). (Use the appropriate <, , or > symbolto separate substances in the list.)Al3+, Cr³+, Zn2+, H₂O, 104, and 1₂chemPad|XX"HelpGreek-

Use data from standard reduction potential table and place the following in order of increasing…

Using data from the Standard Reduction Potentials table, place the following in order of increasing strength as oxidizing agents (all under standard conditions). (Use the appropriate <, =, or > symbol to separate substances in the list.) Al3+, Cr3+, Zn2+, H₂O, 104, and 1₂ chemPad XX→← Help Greek

Using data from the Standard Reduction Potentials table, place the following in order of increasing strength as oxidizing agents (all under standard conditions). (Use the appropriate <, =, or > symbol to separate substances in the list.) Al3+, Cr3+, Zn2+, H₂O, 104, and 1₂ chemPad XX→← Help Greek

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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Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

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Standard Reduction Potentials at 25°C (298 K) for Many Common Half-reactions
Half-reaction
8° (V)
Half-reaction
F₂ +2e2F-
Ag2+ + e
Ag+
Co³+ + e→→ Co²+
H₂O₂ + 2H+ + 2e
Ce4++e Ce³+
→ 2H₂O
PbO₂ + 4H+ + SO42
MnO4 + 4H+ + 3e
IO4 + 2H+ + 2e →
MnO4 + 8H+ + Se
Au³+ + 3e → Au
PbO₂ + 4H+ + 2e
Cl₂ +2e2C1-
Hg₂2+ + 2e
Fe³+ + e
+2e →→ PbSO4 + 2H₂O
→ MnO₂ + 2H₂O
IO3 + H₂O
→ Mn²+ + 4H₂O
→ Pb²+ + 2H₂O
Cr₂O72- + 14H+ + 6e- →2Cr³+ + 7H₂O
O₂ + 4H+ + 4e → 2H₂O
MnO₂ + 4H+ + 2e
IO3 + 6H+ + Se-
Br₂ 2e 2Br
VO₂+ + 2H+ + e
AuCl4 + 3e →
NO3 + 4H+
ClO₂ + e
2Hg2+ + 2e
Age → Ag
→ Mn²+ + 2H₂O
→ 1₂ + 3H₂O
→ VO2+ + H₂O
Au + 4CI-
+ 3e → NO + 2H₂O
ClO₂-
→ Hg₂²+
→ 2Hg
Fe2+
O₂ + 2H+ + 2e → H₂O₂
MnO4 + e→→ MnO4²-
1₂ +2e → 21-
Cute
Cu
2.87
1.99
1.82
1.78
1.70
1.69
1.68
1.60
1.51
1.50
1.46
1.36
1.33
1.23
1.21
1.20
1.09
1.00
0.99
0.96
0.954
0.91
0.80
0.80
0.77
0.68
0.56
0.54
0.52
O₂ + 2H₂O + 4e4OH-
Cu2+ + 2e → Cu
Hg₂Cl₂ + 2e →→ 2Hg + 2Cl-
AgCl +eAg + Cl-
SO4 + 4H+ + 2e
Cu²+ + e
2H+ + 2e
Fe³+ + 3e
Cu+
→→ H₂
→→ Fe
→→ Pb
→→ Sn
→→ Ni
Pb²+ + 2e
Sn²+ + 2e
Ni2+ + 2e
PbSO4 + 2e
Cd2+ + 2e
→→ Pb + SO4²-
→→ Cd
→→→ Fe
Fe2+ + 2e
Cr³+ + e
Cr²+
Cr³+ + 3e
→ Cr
→ Zn
Zn²+ + 2e
2H₂O + 2e
→ H₂ + 2OH-
Mn²+ + 2e → Mn
Al³+ + 3e →→ Al
H₂ +2e → 2H-
Mg2+ + 2e → Mg
La³+ + 3e → La
→→→ Na
Na+ + e
Ca2+ + 2e
Ba2+ + 2e
K++eK
→→ Ca
→→ Ba
→ H₂SO3 + H₂O
Lite Li
8° (V)
0.40
0.34
0.27
0.22
0.20
0.16
0.00
-0.036
-0.13
-0.14
-0.23
-0.35
-0.40
-0.44
-0.50
-0.73
-0.76
-0.83
-1.18
-1.66
-2.23
-2.37
-2.37
-2.71
-2.76
-2.90
-2.92
-3.05

Using data from the Standard Reduction Potentials table, place the following in order of increasing strength as oxidizing agents (all under standard conditions). (Use the appropriate <, , or > symbol
to separate substances in the list.)
Al3+, Cr³+, Zn2+, H₂O, 104, and 1₂
chemPad
|XX"
Help
Greek-

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