An aqueous FeF₂ 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 F (aq) F₂(g) +2 e 2.870 O₂(g) + 4 H3O*(aq) + 4e¯ 6 H₂001) 1.229 2 H₂O(l) +2 e →→→ H₂(g) + 2 OH¯¨(aq) -0.828 Fe²+ (aq) + 2 e Fe(s) -0.440 Half-reaction at anode: Half-reaction at cathode: + + (b) What is the expected decomposition potential? -> + +
An aqueous FeF₂ 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 F (aq) F₂(g) +2 e 2.870 O₂(g) + 4 H3O*(aq) + 4e¯ 6 H₂001) 1.229 2 H₂O(l) +2 e →→→ H₂(g) + 2 OH¯¨(aq) -0.828 Fe²+ (aq) + 2 e Fe(s) -0.440 Half-reaction at anode: Half-reaction at cathode: + + (b) What is the expected decomposition potential? -> + +
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 18.47QE
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Transcribed Image Text:An aqueous FeF₂ 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
2 F (aq)
F₂(g) +2 e
2.870
O₂(g) + 4 H3O*(aq) + 4 e¯ →→ 6 H₂O(l) 1.229
2 H₂O(1) +2 eH₂(g) + 2 OH(aq) -0.828
Fe²+ (aq) + 2 e Fe(s)
+
(b) What is the expected decomposition potential?
-0.440
+
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