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6M.11D

Posted: Tue Feb 25, 2020 8:30 pm
by JamieVu_2C
Suppose that each of the following pairs of redox couples is combined to form a galvanic cell that generates a current under standard conditions. Identify the oxidizing agent and the reducing agent, write a cell diagram, and calculate the standard cell potential from the standard potentials of the electrodes.
(d) O3/O2,OH- and Ag+/Ag

O3/O2,OH- forms the cathode and Ag+/Ag forms the anode. I wrote the cell diagram as Ag(s)|Ag+(aq)||O3(g),O2(g),OH-(aq)|Pt(s). Since the reaction for the cathode is O3(g) +H20(l) + 2e- --> O2(g) + 2OH-(aq), shouldn't the cathode side of the cell diagram be written with the species in this order to show the electron flow? Instead, the textbook solutions shows the cathode side of the cell diagram as ||OH-(aq)|O3(g),O2(g)|Pt(s). Does it matter if OH-(aq) is before or after O3(g) and O2(g)?

Re: 6M.11D

Posted: Tue Feb 25, 2020 8:34 pm
by Benjamin Feng 1B
Dr. Lavelle writes it like that to show the flow of electrons and to make it more clear for us, but it isn't convention and you can write it in either order.