Can someone please help with question 11 1302 - 4.3 - Electrolysis of Aqueous Salts - Copy - Copy11 of 15I Review | Constants I Periodic TableRefer to this table of reduction potentials to answer the questions.PotentialReduction half-reaction(V)F2 (g) + 20→2F¯(aq)O2 (g) + 4H (aq) + 4 ¯→2H2O(1)Br2 (1) + 2e→2Br¯ (aq)+2.87+1.23+1.07Ag+ +e→Ag(s)+0.802H+ (aq) + 20→H2(g)2H2 O(1) + 20→H2(g)+2OH¯ (aq)Na+(aq) +e¯→Na(s)-0.83-2.71Electrolytic cells use electricity to cause a nonspontaneous redox reaction to occur. An electrolytic cell is constructedusing the following components:• a power source, such as a battery,• the substance that will undergo electrolysis, and• two inert electrodes (usually platinum), which serve as the electrical connection between the powersource and the substance undergoing electrolysis.As with any cell, oxidation occurs at the anode and reduction occurs at the cathode. The oxidation of water, whichproduces oxygen (O2) gas, will compete with the oxidation of the anion, and the reduction of water, which produceshydrogen (H2 ) gas, will compete with the reduction of the cation. Only the reaction with the higher (more positive)potential will occur. Keep in mind that the potentials for the oxidation reaction have the opposite sign as those for thecorresponding reduction reactions. For example, the oxidation reaction Ag(s)→Ag+ +e¯ would have an Ex of-0.80 V.

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Science

Chemistry

Can someone please help with question 11

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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