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 °C2 F (aq)F₂(g) +2 e2.870O₂(g) + 4 H3O*(aq) + 4 e¯ →→ 6 H₂O(l) 1.2292 H₂O(1) +2 eH₂(g) + 2 OH(aq) -0.828Fe²+ (aq) + 2 e Fe(s)+(b) What is the expected decomposition potential?-0.440+

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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

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...

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Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

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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