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(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 Cl(9) + 2 e —2 СГ(aq) 1.360 0,() + 4 H,о"(аq) + 4 e — 6 н,0()| 1.229 2 Н,0() + 2 е → H2(g) + 2 OH'(aq) -0.828 Mg*(aq) + 2 e¯ Mg(s) -2.370 Half-reaction at anode: + Half-reaction at cathode: + (b) What is the expected decomposition potential? V

(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 Cl(9) + 2 e —2 СГ(aq) 1.360 0,() + 4 H,о"(аq) + 4 e — 6 н,0()| 1.229 2 Н,0() + 2 е → H2(g) + 2 OH'(aq) -0.828 Mg*(aq) + 2 e¯ Mg(s) -2.370 Half-reaction at anode: + Half-reaction at cathode: + (b) What is the expected decomposition potential? V

Chemistry
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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Enter electrons as e". Use smallest possible integer coefficients. States are not required. If a box is not needed, leave it blank. An aqueous MgCl, 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 CI'(aq) 1.360 O2(g) + 4 H30*(aq) + 4 e → 6 H,0(1)| 1.229 2 Н,0() + 2 е H2(g) + 2 OH´(aq) |-0.828 Mg**(aq) + 2 e"- → Mg(s) -2.370 Half-reaction at anode: + + + Half-reaction at cathode: + (b) What is the expected decomposition potential? V
Transcribed Image Text:Enter electrons as e". Use smallest possible integer coefficients. States are not required. If a box is not needed, leave it blank. An aqueous MgCl, 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 CI'(aq) 1.360 O2(g) + 4 H30*(aq) + 4 e → 6 H,0(1)| 1.229 2 Н,0() + 2 е H2(g) + 2 OH´(aq) |-0.828 Mg**(aq) + 2 e"- → Mg(s) -2.370 Half-reaction at anode: + + + Half-reaction at cathode: + (b) What is the expected decomposition potential? V
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