Moderators: Chem_Mod, Chem_Admin

Posts: 108
Joined: Thu Jul 25, 2019 12:16 am


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:

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.

Posts: 18400
Joined: Thu Aug 04, 2011 1:53 pm
Has upvoted: 435 times

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.

Return to “Galvanic/Voltaic Cells, Calculating Standard Cell Potentials, Cell Diagrams”

Who is online

Users browsing this forum: No registered users and 0 guests