6L.9

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JamieVu_2C
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Joined: Thu Jul 25, 2019 12:16 am

6L.9

Postby JamieVu_2C » Sun Mar 01, 2020 2:31 am

(a) Write balanced half-reactions for the redox reaction of an acidified solution of potassium permanganate and iron(II) chloride. (b) Write the balanced equation for the cell reaction and devise a galvanic cell to study the reaction (write its cell diagram).

The half reactions are:
anode:
cathode:

Which gives the overall reaction:


The cell diagram given in the textbook solutions is: Pt(s)|Fe3+(aq), Fe2+(aq)||H+(aq), MnO4-(aq), Mn2+(aq)|Pt(s)
Why is H+ included in the cell diagram? I thought it's usually omitted in the cell diagram unless it's a hydrogen electrode being used since H+ is used to balance the H atoms in the oxidation reaction.

Chem_Mod
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Re: 6L.9

Postby Chem_Mod » Sun Mar 01, 2020 4:45 pm

The H+ is included to indicate that you have your reaction taking place in acidic solution. Additionally, your anode and cathode reactions should be switched; oxidation takes place at the anode and reduction takes place at the cathode.


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