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An aqueous CdCl₂ solution is electrolyzed under 1 bar pressure using platinum electrodes. (a) Write the half-reactions predicted to occur at the anode and cathode, based on the standard cell potentials given below. Half-reaction at anode: Half-reaction at cathode: + + Standard Reduction Potentials (Volts) at 25 °C Cl₂(g) + 2 e 2 Cl-(aq) 1.360 O₂(g) + 4 H30+(aq) + 4 e¯ →→→ 6 H₂O(l) 1.229 2 H₂O(l) + 2 e² →→→ H₂(g) + 2 OH-(aq) -0.828 Cd²+ (aq) + 2 e² → Cd(s) -0.403 + + (b) What is the expected decomposition potential? + + + +

An aqueous CdCl₂ solution is electrolyzed under 1 bar pressure using platinum electrodes. (a) Write the half-reactions predicted to occur at the anode and cathode, based on the standard cell potentials given below. Half-reaction at anode: Half-reaction at cathode: + + Standard Reduction Potentials (Volts) at 25 °C Cl₂(g) + 2 e 2 Cl-(aq) 1.360 O₂(g) + 4 H30+(aq) + 4 e¯ →→→ 6 H₂O(l) 1.229 2 H₂O(l) + 2 e² →→→ H₂(g) + 2 OH-(aq) -0.828 Cd²+ (aq) + 2 e² → Cd(s) -0.403 + + (b) What is the expected decomposition potential? + + + +

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 18.49QE: A half-cell that consists of a copper wire in a 1.00 M Cu(NO3)2 solution is connected by a salt...
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Half-reaction at anode: Use the References to access important values if needed for this question. An aqueous CdCl₂ solution is electrolyzed under 1 bar pressure using platinum electrodes. (a) Write the half-reactions predicted to occur at the anode and cathode, based on the standard cell potentials given below. Standard Reduction Potentials (Volts) at 25 °C 2 Cl-(aq) 1.360 Cl₂(g) + 2 e- O₂(g) + 4 H3O+(aq) + 4 e¯ →→→ 6 H₂O(l) 1.229 2 H₂O(1) + 2 e¯ →→ H₂(g) + 2 OH-(aq) Cd²+(aq) + 2 e² →→ Cd(s) -0.828 -0.403 Half-reaction at cathode: Enter electrons as e. Use smallest possible integer coefficients. States are not required. If a box is not needed, leave it blank. + (b) What is the expected decomposition potential? V + + + +
Transcribed Image Text:Half-reaction at anode: Use the References to access important values if needed for this question. An aqueous CdCl₂ solution is electrolyzed under 1 bar pressure using platinum electrodes. (a) Write the half-reactions predicted to occur at the anode and cathode, based on the standard cell potentials given below. Standard Reduction Potentials (Volts) at 25 °C 2 Cl-(aq) 1.360 Cl₂(g) + 2 e- O₂(g) + 4 H3O+(aq) + 4 e¯ →→→ 6 H₂O(l) 1.229 2 H₂O(1) + 2 e¯ →→ H₂(g) + 2 OH-(aq) Cd²+(aq) + 2 e² →→ Cd(s) -0.828 -0.403 Half-reaction at cathode: Enter electrons as e. Use smallest possible integer coefficients. States are not required. If a box is not needed, leave it blank. + (b) What is the expected decomposition potential? V + + + +
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