Problem question

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Jane Burgan 1C
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Problem question

Postby Jane Burgan 1C » Sun Feb 24, 2019 10:05 pm

For the 6th edition for problem 14-17, it says (a) Write balanced half-reactions for the redox reaction of an acidic 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).
For part b, the solutions manual shows the answer to be Pt/Fe3+/Fe3//H+/MnO4-/Mn2+/Pt
How do we know to add the inert conductor Pt to the cell diagram, and why is H+ on the cathode side of the cell diagram?

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Re: Problem question

Postby Chem_Mod » Mon Feb 25, 2019 3:03 pm

The solutions manual actually says:
Pt(s)|Fe3+(aq), Fe2+(aq)||H+(aq), MnO4(aq), Mn2+(aq)|Pt(s)
The Pt(s) is necessary because there is no pure conductor involved in the reaction. The H+(aq) is included because the permanganate solution was specified as acidic.


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