An aqueous ScCl3 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 °CCl2(g) + 2 e- 2 Cl-(aq)1.360O2(g) + 4 H3O+(aq) + 4 e- 6 H2O(l)1.2292 H2O(l) + 2 e- H2(g) + 2 OH-(aq)-0.828Sc3+(aq) + 3 e- Sc(s)-2.080Half-reaction at anode: + + --> + + Half-reaction at cathode: + + --> + + (b) What is the expected decomposition potential? ________V

The anode is a positively charged electrode. The oxidation will occur at the anode and it has greater oxidation potential. However, the cathode is a negatively charged electrode. The reduction will occur at the cathode and it has greater reduction potential.a) The possible reactions at the anode are shown as follows. 2Cl-aq→Cl2g+2e- E∘oxi=-1.360 V 6H2Ol→O2g+4H3O+aq+4e- E∘oxi=-1.229 V We know that the greater the oxidation potential, the oxidation would occur easily. Therefore, from the above two reactions, the second reaction will occur at anode because of its greater E∘oxi. The possible reactions at the cathode are shown as follows. Sn3+aq+3e-→Sns E∘red=-2.080 V 2H2Ol+2e-→H2g+2OH-aq E∘red=-0.828 V We know that the greater the reduction potential, the reduction would occur easily. Therefore, from the above two reactions, the second reaction will occur at anode because of its greater E∘red. Therefore, the two half-reactions are shown as follows. At anode : 6H2Ol→O2g+4H3O+aq+4e- E∘oxi=-1.229 V At cathode : 2H2Ol+2e-→H2g+2OH-aq E∘red=-0.828 V b) The expected decomposition potential in terms of standard reduction potentials is calculated as shown below. E∘cell =E∘cathode-E∘anode E∘cell =-0.828 V - +1.229 VE∘cell =-2.057 V Thus, the expected decomposition potential is -2.057 V.

Answered: An aqueous ScCl3 solution is…

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

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An aqueous ScCl₃ 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
Cl₂(g) + 2 e^- 2 Cl^-(aq)	1.360
O₂(g) + 4 H₃O⁺(aq) + 4 e^- 6 H₂O(l)	1.229
2 H₂O(l) + 2 e^- H₂(g) + 2 OH^-(aq)	-0.828
Sc³⁺(aq) + 3 e^- Sc(s)	-2.080

Half-reaction at anode:

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Half-reaction at cathode:

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(b) What is the expected decomposition potential? ________V

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