(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).
How do we know that the chlorine in iron(II) chloride will not be a part of the redox rxn? The solution does not have it in the oxidation rxn ?
6L.9
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Re: 6L.9
Most compounds with chlorine in them are soluble in aqueous solutions, so the iron (III) chloride will be dissociated into Fe3+ and 3Cl-. The same applies for the potassium permanganate; it will dissociated into K+ and MnO4-. When the iron chloride and potassium permanganate are oxidized/reduced, the oxidation states of Cl- and K+ remain the same because that is their most stable state.
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Re: 6L.9
Oxidation number rules can help with this. You know that halogens will be -1, and that alkali will be +1. This means those substances are highly unlikely to change.
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Re: 6L.9
Because it is ionic and we need the Fe to take its lower energy state and Cl is a salt bridge ion it wont partake in the reaction.
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