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Introductory Chemistry - 1st Canadian Edition: Appendix E: Standard Reduction Potentials by Value

Introductory Chemistry - 1st Canadian Edition
Appendix E: Standard Reduction Potentials by Value
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table of contents
  1. Cover
  2. Title Page
  3. Copyright
  4. Table Of Contents
  5. Acknowledgments
  6. Dedication
  7. About BCcampus Open Education
  8. Chapter 1. What is Chemistry
    1. Some Basic Definitions
    2. Chemistry as a Science
  9. Chapter 2. Measurements
    1. Expressing Numbers
    2. Significant Figures
    3. Converting Units
    4. Other Units: Temperature and Density
    5. Expressing Units
    6. End-of-Chapter Material
  10. Chapter 3. Atoms, Molecules, and Ions
    1. Acids
    2. Ions and Ionic Compounds
    3. Masses of Atoms and Molecules
    4. Molecules and Chemical Nomenclature
    5. Atomic Theory
    6. End-of-Chapter Material
  11. Chapter 4. Chemical Reactions and Equations
    1. The Chemical Equation
    2. Types of Chemical Reactions: Single- and Double-Displacement Reactions
    3. Ionic Equations: A Closer Look
    4. Composition, Decomposition, and Combustion Reactions
    5. Oxidation-Reduction Reactions
    6. Neutralization Reactions
    7. End-of-Chapter Material
  12. Chapter 5. Stoichiometry and the Mole
    1. Stoichiometry
    2. The Mole
    3. Mole-Mass and Mass-Mass Calculations
    4. Limiting Reagents
    5. The Mole in Chemical Reactions
    6. Yields
    7. End-of-Chapter Material
  13. Chapter 6. Gases
    1. Pressure
    2. Gas Laws
    3. Other Gas Laws
    4. The Ideal Gas Law and Some Applications
    5. Gas Mixtures
    6. Kinetic Molecular Theory of Gases
    7. Molecular Effusion and Diffusion
    8. Real Gases
    9. End-of-Chapter Material
  14. Chapter 7. Energy and Chemistry
    1. Formation Reactions
    2. Energy
    3. Stoichiometry Calculations Using Enthalpy
    4. Enthalpy and Chemical Reactions
    5. Work and Heat
    6. Hess’s Law
    7. End-of-Chapter Material
  15. Chapter 8. Electronic Structure
    1. Light
    2. Quantum Numbers for Electrons
    3. Organization of Electrons in Atoms
    4. Electronic Structure and the Periodic Table
    5. Periodic Trends
    6. End-of-Chapter Material
  16. Chapter 9. Chemical Bonds
    1. Lewis Electron Dot Diagrams
    2. Electron Transfer: Ionic Bonds
    3. Covalent Bonds
    4. Other Aspects of Covalent Bonds
    5. Violations of the Octet Rule
    6. Molecular Shapes and Polarity
    7. Valence Bond Theory and Hybrid Orbitals
    8. Molecular Orbitals
    9. End-of-Chapter Material
  17. Chapter 10. Solids and Liquids
    1. Properties of Liquids
    2. Solids
    3. Phase Transitions: Melting, Boiling, and Subliming
    4. Intermolecular Forces
    5. End-of-Chapter Material
  18. Chapter 11. Solutions
    1. Colligative Properties of Solutions
    2. Concentrations as Conversion Factors
    3. Quantitative Units of Concentration
    4. Colligative Properties of Ionic Solutes
    5. Some Definitions
    6. Dilutions and Concentrations
    7. End-of-Chapter Material
  19. Chapter 12. Acids and Bases
    1. Acid-Base Titrations
    2. Strong and Weak Acids and Bases and Their Salts
    3. Brønsted-Lowry Acids and Bases
    4. Arrhenius Acids and Bases
    5. Autoionization of Water
    6. Buffers
    7. The pH Scale
    8. End-of-Chapter Material
  20. Chapter 13. Chemical Equilibrium
    1. Chemical Equilibrium
    2. The Equilibrium Constant
    3. Shifting Equilibria: Le Chatelier’s Principle
    4. Calculating Equilibrium Constant Values
    5. Some Special Types of Equilibria
    6. End-of-Chapter Material
  21. Chapter 14. Oxidation and Reduction
    1. Oxidation-Reduction Reactions
    2. Balancing Redox Reactions
    3. Applications of Redox Reactions: Voltaic Cells
    4. Electrolysis
    5. End-of-Chapter Material
  22. Chapter 15. Nuclear Chemistry
    1. Units of Radioactivity
    2. Uses of Radioactive Isotopes
    3. Half-Life
    4. Radioactivity
    5. Nuclear Energy
    6. End-of-Chapter Material
  23. Chapter 16. Organic Chemistry
    1. Hydrocarbons
    2. Branched Hydrocarbons
    3. Alkyl Halides and Alcohols
    4. Other Oxygen-Containing Functional Groups
    5. Other Functional Groups
    6. Polymers
    7. End-of-Chapter Material
  24. Chapter 17. Kinetics
    1. Factors that Affect the Rate of Reactions
    2. Reaction Rates
    3. Rate Laws
    4. Concentration–Time Relationships: Integrated Rate Laws
    5. Activation Energy and the Arrhenius Equation
    6. Reaction Mechanisms
    7. Catalysis
    8. End-of-Chapter Material
  25. Chapter 18. Chemical Thermodynamics
    1. Spontaneous Change
    2. Entropy and the Second Law of Thermodynamics
    3. Measuring Entropy and Entropy Changes
    4. Gibbs Free Energy
    5. Spontaneity: Free Energy and Temperature
    6. Free Energy under Nonstandard Conditions
    7. End-of-Chapter Material
  26. Appendix A: Periodic Table of the Elements
  27. Appendix B: Selected Acid Dissociation Constants at 25°C
  28. Appendix C: Solubility Constants for Compounds at 25°C
  29. Appendix D: Standard Thermodynamic Quantities for Chemical Substances at 25°C
  30. Appendix E: Standard Reduction Potentials by Value
  31. Glossary
  32. About the Authors
  33. Versioning History

5

Appendix E: Standard Reduction Potentials by Value

Standard Cathode (Reduction) Half-ReactionStandard Reduction Potential E° (volts)

Li+(aq) + e– ⇌ Li(s)

–3.040

Ba2+ + 2e−⇌ Ba(s)

–2.92

Rb+ + e– ⇌ Rb (s)

-2.98

K+(aq) + e– ⇌ K(s)

-2.93

Cs+(aq) + e– ⇌ Cs(s)

-2.92

Ba2+(aq) + 2e- ⇌ Ba(s)

-2.91

Sr2+(aq) + 2e- ⇌ Sr(s)

-2.89

Ca2+(aq) + 2e- ⇌ Ca(s)

–2.84

Na+(aq) + e– ⇌ Na(s)

–2.713

Mg(OH)2(s) + 2e−⇌ Mg(s) + 2OH−

–2.687

La3+ + 3e−⇌ La(s)

–2.38

Mg2+(aq) + 2e– ⇌ Mn(s)

-2.356

Ce3+ + 3e−⇌ Ce(s)

–2.336

Al(OH)4− + 3e−⇌ Al(s) + 4OH−

–2.310

AlF63− + 3e−⇌ Al(s) + 6F−

–2.07

Be2+ + 2e−⇌ Be(s)

–1.99

B(OH)4− + 3e−⇌ B(s) + 4OH−

–1.811

U3+ + 3e−⇌ U(s)

–1.66

Al3+(aq) + 3e– ⇌ Al(s)

–1.676

SiF62− + 4e−⇌ Si(s) + 6F−

–1.37

Zn(CN)42− + 2e−⇌ Zn(s) + 4CN

–1.34

Zn(OH)42− + 2e−⇌ Zn(s) + 4OH−

–1.285

Mn2+ + 2e−⇌ Mn(s)

–1.17

V2+ + 2e−⇌ V(s)

–1.13

2SO32− + 2H2O(l) + 2e− ⇌ S2O42− + 4OH−

–1.13

Zn(NH3)42+ + 2e− ⇌ Zn(s) + 4NH3

–1.04

O2 (aq) + e– ⇌ O2–(aq)

-1.0

Cd(CN)42− + 2e−⇌ Cd(s) + 4CN−

–0.943

MoO42− + 4H2O(l) + 6e−⇌Mo(s) + 8OH−

–0.913

SiO2(s) + 4H+ + 4e−⇌ Si(s) + 2H2O(l)

–0.909

SO42− + H2O(l) + 2e− ⇌ SO32−+ 2OH−

–0.936

Cr2+ + 2e− ⇌ Cr(s)

–0.90

B(OH)3 + 3H+ + 3e− ⇌ B(s) + 3H2O(l)

–0.890

2H2O(l) + 2e– ⇌ H2(g) + 2OH–(aq)

-0.828

Zn2+(aq) + 2e– ⇌ Zn(s)

–0.7618

Co(OH)2(s) + 2e−⇌ Co(s) + 2OH−

–0.746

Cr3+(aq) + 3e– ⇌ Cr(s)

–0.424

Ni(OH)2 + 2e−⇌ Ni(s) + 2OH−

–0.72

Ag2S(s) + 2e−⇌ 2Ag(s) + S2−

–0.71

Se(s) + 2e−⇌ Se2−

–0.67 in 1 M NaOH

Cd(NH3)42+ + 2e−⇌ Cd(s) + 4NH3

–0.622

2SO32− + 3H2O(l) + 4e− ⇌S2O32− + 6OH−

–0.576 in 1 M NaOH

U4+ + e− ⇌ U3+

–0.52

SiO2(s) + 8H+ + 8e− ⇌ SiH4(g) + 2H2O(l)

–0.516

Sb + 3H+ + 3e− ⇌ SbH3(g)

–0.510

H3PO3+ 2H+ + 2e− ⇌ H3PO2 + H2O(l)

-0.50

Ni(NH3)62+ + 2e− ⇌ Ni(s) + 6NH3

–0.49

2CO2(g) + 2H+ +2e−⇌ H2C2O4

–0.481

Cr3+ + e−⇌ Cr2+

–0.424

Fe2+(aq) + 2e– ⇌ Fe(s)

-0.44

S(s) + 2e−⇌ S2−

–0.407

Cd2+(aq) + 2e– ⇌ Cd(s)

–0.4030

Ag(NH3)2+ + e−⇌ Ag(s) + 2NH3

–0.373

Ti3+ + e−⇌ Ti2+

–0.37

PbSO4(s) + 2e−⇌ Pb(s) + SO42−

–0.356

Co2+(aq) + 2e– ⇌ Co(s)

–0.277

2SO42− + 4H+ + 2e− ⇌ S2O62− + 2H2O(l)

–0.25

N2(g) + 5H+ + 4e−⇌ N2H5+

–0.23

H3PO4 + 2H+ + 2e−⇌ H3PO3 + H2O(l)

-0.28

Ni2+(aq) + 2e– ⇌ Ni(s)

–0.257

V3+ + e− ⇌ V2+

–0.255

As + 3H+ + 3e− ⇌ AsH3(g)

–0.225

CO2(g) + 2H+ + 2e− ⇌ HCO2H

–0.20

Mo3+ + 3e− ⇌ Mo(s)

–0.2

Sn2+ + 2e− ⇌ Sn(s)

–0.19 in 1 M HCl

Ti2+ + 2e−⇌ Ti(s)

–0.163

MoO2(s) + 4H+ + 4e−⇌ Mo(s) + 2H2O(l)

–0.152

AgI(s) + e− ⇌ Ag(s) + I−

–0.152

Sn2+(aq) + 2e– ⇌ Sn(s)

-0.14

Pb2+(aq) + 2e– ⇌ Pb(s)

-0.126

CrO42− + 4H2O(l) + 3e− ⇌2Cr(OH)4− + 4OH−

–0.13 in 1 M NaOH

WO2(s) + 4H+ + 4e−⇌ W(s) + 2H2O(l)

–0.119

Se(s) + 2H+ + 2e−⇌ H2Se(g)

–0.115

CO2(g) + 2H+ + 2e−⇌ CO(g) + H2O(l)

–0.106

WO3(s) + 6H+ + 6e−⇌ W(s) + 3H2O(l)

–0.090

Hg2I2(s) + 2e−⇌ 2Hg(l) + 2I−

–0.0405

Fe3+(aq) + 3e– ⇌ Fe(s)

-0.037

2H+(aq) + 2e– ⇌ H2(g)

0.00

P(s,white) + 3H+ + 3e−⇌ PH3(g)

0.06

AgBr(s) + e−⇌ Ag(s) + Br−

0.071

S4O62− + 2e−⇌2S2O32−

0.080

Co(NH3)63+ +e−⇌Co(NH3)62+

0.1

Ru(NH3)63+ + e−⇌ Ru(s) + Ru(NH3)62+

0.10

S(s) + 2H+ + 2e−⇌ H2S

0.144

Sn4+(aq) + 2e– ⇌ Sn2+(aq)

0.154

Cu2+(aq) + e– ⇌ Cu+(aq)

0.159

UO22+ + e− ⇌UO2+

0.16

Co(OH)3(s) + e−⇌ Co(OH)2(s) + OH−

0.17

ClO4–(aq) + H2O(l) + 2e- ⇌ ClO3–(aq) + 2OH–(aq)

0.17

SO42− + 4H+ + 2e− ⇌ H2SO32−+ H2O(l)

0.172

BiCl4− + 3e−⇌ Bi(s) + 4Cl−

0.199

SbO+ + 2H+ + 3e−⇌ Sb(s) + H2O(l)

0.212

AgCl(s) + e– ⇌ Ag(s) + Cl–(aq)

0.2223

HCHO + 2H+ + 2e−⇌ CH3OH

0.2323

HAsO2 + 3H+ + 3e−⇌ As(s) + 2H2O(l)

0.240

Ru3+ + e−⇌ Ru2+

0.249

IO3−+ 3H2O(l) + 6e−⇌ I− + 6OH−

0.257

Hg2Cl2(s) + 2e−⇌ 2Hg(l) + 2Cl−

0.2682

UO2+ + 4H+ + e− ⇌U4+ + 2H2O(l)

0.27

Bi3+ + 3e−⇌ Bi(s)

0.317

UO22+ + 4H+ + 2e− ⇌ U4+ + 2H2O(l)

0.327

VO2+ + 2H+ +e−⇌V3+ + H2O(l)

0.337

Cu2+(aq) + 2e– ⇌ Cu(s)

0.3419

ClO3–(aq) + H2O(l) + 2e– ⇌ ClO2–(aq) + 2OH–(aq)

0.35

Fe(CN)63− + e− ⇌ Fe(CN)64−

0.356

O2(g) + 2H2O(l) + 4e−⇌ 4OH−

0.401

ClO− + H2O(l) + e− ⇌ ½Cl2(g) + 2OH−

0.421 in 1 M NaOH

 Ag2C2O4(s) + 2e−⇌ 2Ag(s) + C2O42−

0.47

Cu+(aq) + e– ⇌ Cu(s)

0.52

I2(s) + 2e– ⇌ 2I–(aq)

0.5355

I3− + 2e−⇌ 3I−

0.536

Ga3+ + 3e−⇌ Ga(s)

-0.56

Cu2+ + Cl− + e−⇌ CuCl(s)

0.559

S2O62− + 4H+ + 2e−⇌ 2H2SO3

0.569

H3AsO4 + 2H+ + 2e−⇌ HAsO2 + 2H2O(l)

0.560

ClO2–(aq) + H2O(l) + 2e– ⇌ ClO–(aq) + 2OH–(aq)

0.59

MnO4− + 2H2O(l) + 3e−⇌ MnO2(s) + 4OH−

0.60

Sb2O5(s) + 6H+ + 4e−⇌ 2SbO+ + 3H2O(l)

0.605

PtCl62− + 2e−⇌ PtCl42- + 2Cl−

0.68

RuO2(s) + 4H+ + 4e−⇌ Ru(s) + 2H2O(l)

0.68

O2(g) + 2H+ + 2e−⇌ H2O2

0.695

PtCl42− + 2e−⇌ Pt(s) + 4Cl−

0.73

H2SeO3 + 4H+ + 4e−⇌ Se(s) + 3H2O(l)

0.74

Tl3+ + 3e−⇌ Tl(s)

0.742

Fe3+(aq) + e– ⇌ Fe2+(aq)

0.771

Hg22+(aq) + 2e– ⇌ 2Hg(l)

0.7960

Ag+(aq) + e- ⇌ Ag(s)

0.7996

Hg2+(aq) + 2e– ⇌ Hg(l)

0.8535

Cu2+ + I− +e−⇌ CuI(s)

0.86

Ru(CN)63− +e−⇌ Ru(s) + Ru(CN)64−

0.86

ClO− + H2O(l) + 2e−⇌ Cl− + 2OH−

0.890 in 1 M NaOH

2Hg2+(aq) + 2e– ⇌ Hg22+(aq)

0.911

HgO(s) + 2H+ + 2e−⇌ Hg(l) + H2O(l)

0.926

NO3− + 3H+ + 2e−⇌ HNO2 + H2O(l)

0.94

MnO2(s) + 4H+ + e– ⇌ Mn3+ (aq) + H2O(I)

0.95

NO3–(aq) + 4H+(aq) + 3e– ⇌ NO(g) + 2H2O(l)

0.96

HIO + H+ + 2e−⇌ I− + H2O(l)

0.985

HNO2 + H+ +e−⇌ NO(g) + H2O(l)

0.996

VO22+ + 2H+  +e−⇌ VO2+ + H2O(l)

1.000

AuCl4− + 3e−⇌ Au(s) + 4Cl−

1.002

NO2 (g) + H+ (aq) + e– ⇌ HNO2 (aq)

1.07

Br2(l) + 2e– ⇌ 2Br–(aq)

1.087

Fe(phen)63+ +e− ⇌ Fe(phen)62+

1.147

SeO43− + 4H+ + e−⇌ H2SeO3 + H2O(l)

1.151

ClO3− + 2H+ + e−⇌ ClO2(g) + H2O

1.175

ClO3− + 3H+ + 2e− ⇌ HClO2 + H2O

1.181

IO3− + 6H+ + 5e−⇌ ½I2(s) + 3H2O(l)

1.195

Pt2+ + 2e−⇌ Pt(s)

1.2

ClO4− + 2H+ + 2e− ⇌ ClO3− + H2O

1.201

O2(g) + 4H+(aq) + 4e– ⇌ 2H2O(l)

1.229

MnO2(s) + 4H+ + 2e−⇌ Mn2+ + 2H2O(l)

1.23

Tl3+ + 2e− ⇌ Tl+

0.77 in 1 M HCl

2HNO2 + 4H+ + 4e−⇌ N2O(g) + 3H2O(l)

1.297

HOBr + H+ + 2e−⇌ Br− + H2O(l)

1.341

Cr2O72-(aq) + 14H+(aq) + 6e– ⇌ 2Cr3+(aq) + 7H2O(l)

1.36

Cr2O72− + 14H+ + 6e− ⇌ 2Cr3+ + 7H2O(l)

1.36

Cl2(g) + 2e– ⇌ 2Cl–(aq)

1.396

Au3+ + 2e−⇌ Au+

1.36

Hg2Br2(s) + 2e−⇌ 2Hg(l) + 2Br−

1.392

Ce4+(aq) + e– ⇌ Ce3+(aq)

1.44

PbO2(s) + 4H+ +2e– ⇌ Pb2+(aq) + 2H2O(l)

1.46

BrO3− + 6H+ + 6e−⇌ Br− + 3H2O

1.478

Mn3+ + e−⇌ Mn2+

1.5

MnO4–(aq) + 8H+(aq) + 5e– ⇌ Mn2+(aq) + 4H2O(l)

1.51

BrO3− + 6H+ + 5e−⇌ ½Br2(l) + 3H2O

1.5

Au3+ + 3e−⇌ Au(s)

1.52

2NO(g) + 2H+ + 2e−⇌ N2O(g) + H2O(l)

1.59

HOBr + H+ + e−⇌ ½Br− + H2O(l)

1.604

HClO2 + 2H+ + 2e−⇌ HOCl + H2O

1.64

PbO2(s) + 4SO42− + 4H+ + 2e−⇌ PbSO4(s) + 2H2O(l)

1.690

MnO4− + 4H+ +3e−⇌ MnO2(s) + 2H2O(l)

1.70

Ce4+ + e−⇌ Ce3+

1.72

N2O(g) + 2H+ + 2e−⇌ N2(g) + H2O(l)

1.77

H2O2(aq) + 2H+(aq) + 2e– ⇌ 2H2O(l)

1.763

Au+ + e−⇌ Au(s)

1.83

Co3+(aq) + e− ⇌ Co2+(aq)

1.92

S2O82− + 2e−⇌2SO42−

1.96

O3(g) + 2H+(aq) + 2e− ⇌ O2(g) + H2O(l)

2.07

BaO(s) + 2H+ + 2e−⇌ Ba(s) + H2O(l)

2.365

F2(g) + 2e− ⇌ 2F−(aq)

2.87

F2(g) + 2H+ + 2e−⇌ 2HF

3.053

From UC Davis Chem Wiki (Creative Commons licence): UC Davis GeoWiki by University of California, Davis. CC-BY-NC-SA-3.0

Original source materials: Bard, A. J.; Parsons, B.; Jordon, J., eds. Standard Potentials in Aqueous Solutions, Dekker: New York, 1985; Milazzo, G.; Caroli, S.; Sharma, V. K. Tables of Standard Electrode Potentials, Wiley: London, 1978; Swift, E. H.; Butler, E. A. Quantitative Measurements and Chemical Equilibria, Freeman: New York, 1972.

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