Docsity
Docsity

Prepare for your exams
Prepare for your exams

Study with the several resources on Docsity


Earn points to download
Earn points to download

Earn points by helping other students or get them with a premium plan


Guidelines and tips
Guidelines and tips

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

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 🇺🇸

4.7

(11)

245 documents

1 / 3

Toggle sidebar

This page cannot be seen from the preview

Don't miss anything!

bg1
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

Partial preview of the text

Download Standard Reduction Potentials at 25°C: Half-Reactions & Electrode Potentials and more Exams Chemistry in PDF only on Docsity!

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.