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Standard Reduction Potentials at 25°C: Half-Reactions & Electrode Potentials, Exams of Chemistry

Parker UniversityChemistry

A list of standard reduction potentials for various half-reactions at a temperature of 25°c. Each half-reaction is accompanied by its corresponding electrode potential in volts. This information is essential for understanding electrochemical processes and redox reactions.

Typology: Exams

2021/2022

Uploaded on 09/12/2022

chiara44
chiara44 🇺🇸

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Standard Reduction Potentials at 25°C
Half-Reaction E° (V)
Ag+(aq) + e- → Ag (s) +0.799
AgBr (s) + e- → Ag (s) + Br-(aq) +0.095
AgCl (s) + e- → Ag (s) + Cl-(aq) +0.222
Ag(CN)2-(aq) + e- → Ag (s) + 2CN-(aq) -0.310
Ag2CrO4 (s) + 2e- → 2Ag (s) + CrO42-(aq) +0.446
AgI (s) + e- → Ag (s) + I-(aq) -0.151
Ag(S2O3)23-(aq) + e- → Ag (s) + 2S2O32-(aq) +0.010
Al3+(aq) + 3e- → Al (s) -1.660
H3AsO4 (aq) + 2H+(aq) + 2e- → H3AsO3(aq) + H2O (l) +0.559
Ba2+(aq) + 2e- → Ba (s) -2.900
BiO+(aq) + 2H+(aq) + 3e- → Bi (s) + H2O (l) +0.320
Br2 (l) + 2e- → 2Br-(aq) +1.065
BrO3-(aq) + 6H+(aq) +5e- → Br2 (l) + 3H2 O (l) +1.520
2CO2 (g) + 2H+(aq) + 2e- → H2C2O4 (aq) -0.490
Ca2+(aq) + 2e- → Ca (s) -2.870
Cd2+(aq) + 2e- → Cd (s) -0.403
Ce4+(aq) + e- → Ce3+(aq) +1.610
Cl2 (g) + 2e- → 2Cl-(aq) +1.359
HClO (aq) + H+(aq) + e- → Cl2 (g) + H2O (l) +1.630
ClO-(aq) + H2O (l) + 2e- → Cl-(aq) + 2OH-(aq) +0.890
ClO3-(aq) + 6H+(aq) + 5e- → Cl2 (g) + 3H2O (l) +1.470
Co2+(aq) + 2e- → Co (s) -0.277
pf3

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Standard Reduction Potentials at 25 ° C

Half-Reaction (^) E ° (V) Ag

(aq) + e

  • → Ag (^) (s) +0. AgBr (^) (s) + e

→ Ag (^) (s) + Br

(aq) +0. AgCl (^) (s) + e-^ → Ag (^) (s) + Cl-(aq) +0. Ag(CN) 2 - (aq) + e-^ → Ag (^) (s) + 2CN-(aq) -0. Ag 2 CrO4 (s) + 2e

→ 2Ag (^) (s) + CrO 4 2- (aq) +0. AgI (^) (s) + e

→ Ag (^) (s) + I

(aq) -0. Ag(S 2 O 3 ) 2 3- (aq) + e

→ Ag (^) (s) + 2S 2 O 3 2- (aq) +0. Al3+(aq) + 3e-^ → Al (^) (s) -1. H 3 AsO4 (aq) + 2H+(aq) + 2e-^ → H 3 AsO3(aq) + H 2 O (^) (l) +0. Ba 2+ (aq) + 2e

→ Ba (^) (s) -2. BiO

(aq) + 2H

(aq) + 3e

→ Bi (^) (s) + H 2 O (^) (l) +0. Br2 (l) + 2e

→ 2Br

(aq) +1. BrO 3 - (aq) + 6H+(aq) +5e-^ → Br2 (l) + 3H 2 O (^) (l) +1. 2CO2 (g) + 2H+(aq) + 2e-^ → H 2 C 2 O4 (aq) -0. Ca 2+ (aq) + 2e

→ Ca (^) (s) -2. Cd 2+ (aq) + 2e

→ Cd (^) (s) -0. Ce 4+ (aq) + e

→ Ce 3+ (aq) +1. Cl2 (g) + 2e-^ → 2Cl-(aq) +1. HClO (^) (aq) + H+(aq) + e-^ → Cl2 (g) + H 2 O (^) (l) +1. ClO

(aq) + H 2 O^ (l) + 2e

→ Cl

(aq) + 2OH

(aq) +0. ClO 3

(aq) + 6H

(aq) + 5e

→ Cl2 (g) + 3H 2 O (^) (l) +1. Co 2+

→ Co (^) (s) -0.

Co3+(aq) + e-^ → Co2+(aq) +1. Cr3+(aq) + 3e-^ → Cr (^) (s) -0. Cr 3+ (aq) + e

  • → Cr 2+ (aq) -0. Cr 2 O 7 2- (aq) + 14H

(aq) + 6e

→ 2Cr 3+ (aq) + 7H 2 O^ (l) +1. CrO 4 2- (aq) + 4H 2 O^ (l) + 3e

→ Cr(OH)3 (s) + 5OH

(aq) -0. Cu2+(aq) + 2e-^ → Cu (^) (s) +0. Cu2+(aq) + e-^ → Cu+(aq) +0. Cu

(aq) + e

→ Cu (^) (s) +0. CuI (^) (s) + e

→ Cu(s) + I

(aq) -0. F2 (g) + 2e

→ 2F

(aq) +2. Fe2+(aq) + 2e-^ → Fe (^) (s) -0. Fe3+(aq) + e-^ → Fe2+(aq) +0. Fe(CN) 6 3- (aq) + e

→ Fe(CN) 6 4- (aq) +0. 2H

(aq) + 2e

→ H2 (g) 0. 2H 2 O (^) (l) + 2e

→ H2 (g) + 2OH

(aq) -0. HO 2 - (aq) + H 2 O (^) (l) + 2e-^ → 3OH-(aq) +0. H 2 O2 (aq) + 2H+(aq) + 2e-^ → 2H 2 O (^) (l) +1. Hg 2 2+ (aq) + 2e

→ 2Hg (^) (l) +0. 2Hg 2+ (aq) + 2e

→ Hg 2 2+ (aq) +0. Hg 2+ (aq) + 2e

→ Hg (^) (l) +0. I2 (s) + 2e-^ → 2I-(aq) +0. IO 3 - (aq) + 6H+(aq) + 5e-^ → I2 (s) + 3H 2 O (^) (l) +1. K

(aq) + e

→ K (^) (s) -2. Li

(aq) + e

→ Li (^) (s) -3. Mg 2+

→ Mg (^) (s) -2.