Question

I am on my last try and would really appreciate if someone could give me the right answers for all the parts. thanks

Electrolysis in Aqueous Solutions -- Overvoltage Refer to data from a table of standard reduction potentials for common half-reactions and/or the following half-reaction to answer the questions below. S20g2- + 2€® 25042 [° = 2.01 v During the electrolysis of an aqueous solution of Na2SO4, which reaction occurs at the (platinum) anode? 2H20 02 + 4H+ + 4e 25042- 52082- + 2e 5042- + 4H+ + 2e" — H2O + H2SO3 2H20 + 2 H2 + 20H Na+ + 2Na During the electrolysis of water containing 0.01 M sodium sulfate, using platinum electrodes, the overvoltage for the oxidation of water results in: The production of slightly more than a 2/1 volume ratio of H2(g)/O2(9) A required potential of less than 1.23 V The production of sodium hydroxide The production of H2(g) and O2(g) in the exact volume ratio 2/1 In the electrolysis of brine (chlor-alkali process), which element is produced at the anode? O2 Cl2 Na O H₂ You might want to consider how pH influences the Nernst equation for certain half-reactions. Refer to sections 11.7 and 11.8 in Zumdahl Chemical Principles' 8th ed.

Answer 1

1) During the electrolysis of an aqueous solution of Na₂SO4, which reaction occurs at the (platinum) anode ? 2 H₂O +200 H₂ + 2040 2) During the electrolysis q water containing 0.01m sodium sulfate using platinum electrodes the overvoltage for the oxidation of water, results in T The required potential of less than 1.23v 5). In the electrolysis of brine C Chlor - alkali process), which element is produced at the anode Cl produced at anode. 200 200 + Cl2. [ anode]