Question

Post Lecture Homework Chapter 19 Electrolysis of Aqueous Salts < 13of15 Electrolytic cells use electricity to cause a nonspontaneous redox reaction to occur. An electrolytic cell is constructed using the following components a power source, such as a battery Review | Constants Periodic Table the substance that will undergo electrolysis, and two inert electrodes (usually platinum), which serve as the electrical connection between the power source and the substance undergoing electrolysis. Refer to this table of reduction s to answer the questions. As with any cell, oxidation occurs at the anode and reduction occurs at the cathode. The oxidation of water, which produces oxygen (02) gas, will compete with the oxidation of the anion, and the reduction of water, which produces hydrogen (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 the corresponding reduction reactions. For example, the oxidation reaction Ag(s Ag +e would have an of-080 V Reduction half-reaction F2(8)+2e-+2F (aq) +2.87 02()4H a)+4e-2H(+1.23 Br2(1) +2c+2Br (aq) Ag +eAg(s) Part A +0.80 2H201)2e H2(g 20H (aq) -083 2.71 What is produced at each electrode in the electrolysis of NaBr(aq)? Na(ag) e-Na(s) Drag the appropriate items to their respective bins. View Available Hint(s) Reset Help 02() Na s) Br2) H2(g) Anode Cathode Not produced

Answer 1

Electrode where oxidation takes place called anode while at cathode reduction takes place.

Anode - Br2

Cathode- H2

Not produced = Na,O2