Question

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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. 52082- + 2e → 25042- E° = 2.01 v During the electrolysis of an aqueous solution of Na2SO4, which reaction occurs at the (platinum) cathode? 2H20 + 2e - H2 + 20H SO42- + 4H+ + 2 H2O + H2SO3 2H20 0 2 + 4H+ + 4e 25042- 52032- + 2e ONa+ + Na During the electrolysis of water containing 0.01 M sodium sulfate, using platinum electrodes, the overvoltage for the oxidation of water results in: O A required potential of greater than 1.23 V O A required potential of exactly 1.23 V The production of slightly less than a 2/1 volume ratio of H2(9)/02(9) The production of sodium metal In the electrolysis of brine (chlor-alkali process), which element is produced at the anode? она Na Cl2 O 02 Refer to sections 11.7 and 11.8 in Zumdahl 'Chemical Principles' 8th ed. Submit Answer Tries 0/5

Answer 1

A. in the electrolysis of an aqueous solution of Na2So4 , the reaction occured is

Na+ + e- gives Na

When water containing a small amount of (~0.01) of sodium sulfate is electrolyzed , measurement of the volume of gases generated consistantly gives a result that the volume ratio of hydrogen to oxygen is not quite 2:1 .

the more the E value , the more the reaction has a tendancy to proceed in the direction indicated. so the reaction taking place at cathode will be reduction of H2O

B. a solution is 0.01 concentrated sodium sulphate is added to the solution. assuming only the sulphates of these cations will precipitates first . later on second ion begins to precipitate

during electrolysis the water containing 0.01 M sodium sulfide using platinum electrodes the over voltage of oxygen of water results in a required potential of greater than 1.23V

3. During electrolysis of brine CHLORINE is produced