The half-reaction that should occur at the cathode during electrolysis of an aqueous Cadmium iodide solution is Standard Reduction Potentials at 25°C Half-reaction E° (V) 02 (g) + 4H+ (aq) +4 e 2 H₂O (1) 12 (s) +2 e 2 (aq) Cd2+ (aq) + 2 e¯→ Cd (s) 2 H₂0 (1) +2e → H2(g) + 2 OH (aq) O cd → Cd2+ + 2 €¯ O2 H₂O +2e → H₂ + 2 OH- 1₂+2e →21 O2 H2O → O2+4H+46 OCd2+ + 2e → Cd 021-1+2e 1.23 0.53 -0.40 - 0.83

The half-reaction that should occur at the cathode during electrolysis of an aqueous Cadmium iodide solution is Standard Reduction Potentials at 25°C Half-reaction E° (V) 02 (g) + 4H+ (aq) +4 e 2 H₂O (1) 12 (s) +2 e 2 (aq) Cd2+ (aq) + 2 e¯→ Cd (s) 2 H₂0 (1) +2e → H2(g) + 2 OH (aq) O cd → Cd2+ + 2 €¯ O2 H₂O +2e → H₂ + 2 OH- 1₂+2e →21 O2 H2O → O2+4H+46 OCd2+ + 2e → Cd 021-1+2e 1.23 0.53 -0.40 - 0.83

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...

See similar textbooks

Similar questions

What mass of material will be deposited at the cathode when a current of 10.5 A is applied for 2.0 hours to the following cell: Cr(s) | Cr² (aq) || Al*(aq) | Al(s)
What is the electrical current, in Amperes, that must be applied if 6.50 g Ag is deposited at the cathode in 2.00 hrs during the electrolysis of AgNO3 (aq)? Please show your work
What is AG" for the following reaction? Use data given in the table. 2Br (ag) + Cla (g) -→ Bra (1) + 2C1 (ag) Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Standard Half-Reaction Potential, E (V) Lit (ag) + e Li(s) Na+(ag) + e Na(s) Mg+ (ag) + 2e Mg(s) -3.04 -2.71 -2.38 Al* (ag) + 3e - Al(s) -1.66 2H20(1) + 2e H2(9) + 20H (ag) -0.83 Zn+ (ag) + 2e Zn(s) -0.76 Cr** (aq) + 3e Cr(s) --0.74 Fe+ (ag) + 2e Fe(s) -0.41 Ca2+ (aq) + 2e Cd(s) -0.40 Ni* (ag) + 2e Ni(s) -0.23 Sn* (aq) + 2e Sn(s) -0.14 Pb+ (ag) + 2e = Pb(s) --0.13 Fe* (ag) + 3e Fe(s) 2H* (ag) + 2e H2 (9) -0.04 0.00 Sn+ (ag) + 2e Sn+ (ag) 0.15
Calculate the equilibrium constant, K, for the reaction shown at 25 °C. Fe+(aq)+B(s) + 6 H, O(1) → Fe(s) + H,BO,(s) + 3 H,O*(aq) The balanced reduction half-reactions for the equation and their respective standard reduction potential values (E") are Fe3+ (aq) + 3 e- → Fe(s) H,BO, (s) + 3 H,0*(aq) + 3 e- – B(s) + 6 H, O(1) E' = -0.04 V E' = -0.8698 V K =
Help with the following question Please round the answer to 3 sig figs
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3Cu2* (ag) +2A1 (s) –- 3Cu (s) + 2AI³* (aq) 2+ in one half-cell and 4.12 M Al" in the other. 3+ Suppose the cell is prepared with 3.11 M Cu Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.