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 H30¹(aq) + 4 e6 H₂O(1) 1.229 2 H₂O(1) +2 eH₂(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? V ↑ ↑ + + + +
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 H30¹(aq) + 4 e6 H₂O(1) 1.229 2 H₂O(1) +2 eH₂(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? V ↑ ↑ + + + +
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 59P
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Plz solve both parts correctly in clear handwriting asap I'll upvote your answer
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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