An aqueous CdF2 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 F2(g) + 2 e- 2 F-(aq) 2.870 O2(g) + 4 H3O+(aq) + 4 e- 6 H2O(l) 1.229 2 H2O(l) + 2 e- H2(g) + 2 OH-(aq) -0.828 Cd2+(aq) + 2 e- Cd(s) -0.403 Half-reaction at anode: + + + + Half-reaction at cathode: + + + + (b) What is the expected decomposition potential? V
An aqueous CdF2 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 F2(g) + 2 e- 2 F-(aq) 2.870 O2(g) + 4 H3O+(aq) + 4 e- 6 H2O(l) 1.229 2 H2O(l) + 2 e- H2(g) + 2 OH-(aq) -0.828 Cd2+(aq) + 2 e- Cd(s) -0.403 Half-reaction at anode: + + + + Half-reaction at cathode: + + + + (b) What is the expected decomposition potential? V
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Chapter1: Chemical Foundations
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An aqueous CdF2 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 | |
|---|---|
| F2(g) + 2 e- 2 F-(aq) | 2.870 |
| O2(g) + 4 H3O+(aq) + 4 e- 6 H2O(l) | 1.229 |
| 2 H2O(l) + 2 e- H2(g) + 2 OH-(aq) | -0.828 |
| Cd2+(aq) + 2 e- Cd(s) | -0.403 |
Half-reaction at anode:
| + | + | + | + |
Half-reaction at cathode:
| + | + | + | + |
(b) What is the expected decomposition potential? V
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